Acid Base Titration Lab

Acid Base Titration Lab
What is the Concentration of Acetic Acid in Each Sample of Vinegar?
Throughout this Acid–base titration and neutralization reaction lab, the goal was to determine the
concentration of acetic acid within three given samples of vinegar. This titration is based on the
argument that acids and bases neutralize each other when they are mixed together using an exact
stoichiometric ratio. During this investigation we determined the concentration by performing an
acid–base titration with the use of an universoul indicator. We also verified the data using a
stoichiometric ratio and other molar equations. We completed the lab in this way in order to receive
the most accurate results we could, despite experimental errors. In sample A of vinegar, the ... Show
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In sample A, the concentration of acetic acid was: 11.2 moles. In sample B, the concentration of
acetic acid was: .432 moles. In sample C, the concentration of acetic acid was: .8064 moles. In order
to determine these values we had to record data on the amount of titrant we added to the burette and
then had to average these amounts after completing 3 trails. For example, in sample A, Trial 1, we
first filled the burette to 1, after this amount ran out, we stopped the flow of the titrant, and filled the
burette up to 37. When this still wasn't enough, we had to add more titrant, filling it up to 38. To
determine the final amount of titrant used in this first trial, we subtracted these values from one
another. After doing this, we added that amount, as well as the final amounts from the following two
trials in order to determine the average amount of titrant added. In sample B, trial 1, we started the
burette at 22.5 and ended at 50. We did not have to add extra titrant to the burette before the change
in color occurred. From this data, we then determined the change in the amount of titrant from the
beginning point to the end point. Then after retrieving the data from the next two trails, we were
able to average the amount of titrant used for sample B. In sample C, we started off with the the
amount of titrant at 23, and ending at 39. We also did not
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Acid-Base Titration Lab Report
Beau Renegar
May 3rd, 2017
Acid–Base Titration Lab Report
The purpose of this lab was to determine the molarity of a sulfuric acid solution. The materials used
include a buret, a pipet, two 250 mL Erlenmeyer flasks, water, phenophthalein, potassium
hydroxide, and sulfuric acid. Safety concerns included working with potentially dangerous
substances like sulfuric acid.
Procedure and Observations
Procedure
Data and Observations
1. Pipet 10.00 mL of the sulfuric acid solution into each of the 250–mL Erlenmeyer flasks
10.00 mL solution measured into the flasks
2. Add some water to the sulfuric acid solution to see amount in flask
Amount of water does not matter because it does not affect the moles of sulfuric acid
3. Add several drops of phenolphthalein ... Show more content on Helpwriting.net ...
We started with a 10.00 mL of sulfuric acid solution that was pipetted into an Erlenmeyer flask. The
volume and concentration of the base must be known so that we know three of the four
volumes/concentrations. The base concentration was given and the volume was obtained during the
experiment. The titration resulted in the two flasks having the desired pale pink color. The volume
of the base was obtained using the buret. After titration with KOH, the results of the two titrations
are the molarities 0.01357 M and 0.01235

The Effect Of Ph Solution Of Feed Phase On The Removal...
Figure. 7. Effect of pH solution of feed phase on the removal efficiency of citric acid
Transport conditions: Feed phase: citric acid 10–2 M, pH 2–12. Stripping phase: deionized water,
pH=6.8. Membrane: 12.60 cm2 of surface area, Calix[4]resorcinarene (0.15 g/g mixture of
polymers), 0.03 ml 2–NPOE/g mixture of polymers. Values obtained after 5 days of
experimentation.
3.8 Stability of PIMs
In this study, one PIM was reused, whereas the feed and strip phases were replaced after one cycle
with fresh ones in 5 experiments and each experiment lasted from 4 days. As observed in Fig. 8. The
initial flux of PIM shows a gradual decrease with increasing of cycle's reuse, which may be caused
by the loss of carrier from membrane [37]. ... Show more content on Helpwriting.net ...
Conclusion
In this study, a polymer inclusion membrane was prepared and succevally applied for the removal of
citric acid from synthetic wastewater. The mixture of CTA and CA was found to be the optimum
base polymer for quantitative transport of citric acid. Moreover, the nature of carrier especially alkyl
chain length, stirring rate, and pH of feed phase are also important factors affecting the increased
rate of citric acid transport. Hence, from results obtained it can be seen that the investigated
calix[4]resorcinarene are effective extractants for citric acid and that their extraction abilities depend
on the alkyl chain length of the substituent in the macrocycle. Choosing the appropriate length of
alkyl chain, very selective system can be designed. The excellent efficiency for the citric acid
transport by the proposed PIM system reveals its potential application for the selective removal,
concentration and purification of citric acid from different media.
References
[1] K.L. Kalra, H.S. Grewal, Fungal production of citric acid, Biotechnol. Adv., 13 (2) (1995) 209–
234.
[2] M. Pazouki, P.A. Felse, J. Sinha, T. Panda, Comparative studies on citric acid production by
Aspergillus niger and Candida lipolytica using molasses and glucose, Bioprocess Eng., 22 (2000)
353–361.
[3] A.A. Ghoreyshi, F.A. Farhadpour, M. Soltanieh, M. Abdelghani, Transport of small polar
molecules across nonporous

Case Study On Metabolic Sacidosis
Metabolic sacidosis occurs when the chemical sbalance of acids and sbases in a patient's blood gets
sthrown off. This can happen when a spatient's body is making too much sacid, isn't getting rid of
senough acid, or doesn't have senough base to offset a normal samount of acid. Metabolic sacidosis
is defined as shaving an arterial blood pH less than s7.35 with plasma bicarbonate sless than 22
mmol/L. The patient in sthis case had a blood pH of 7.34 with sa plasma bicarbonate slevel of 14
mmol/L. Additionally, the patient had a sdecreased PaCO2 of 26 mm Hg and an elevated sPaO2 of
92 mm Hg, which scould be compensatory for the metabolic sacidosis. The patient has been taking
ssalsalate and aspirin medications, which are common ssalicylates. Salicylate ... Show more content
on Helpwriting.net ...
Patients are soften symptomatic at salicylate concentrations shigher than 40–50 mg/dL. Patients
with ssalicylate sconcentrations approaching sor exceeding 100 mg/dL usually shave serious or life–
threatening stoxicity. Patients with chronic spoisoning who have levels of 60 mg/dL or greater
soften have serious toxicity. In overdoses, the peak serum sconcentration may not occur for 4–6
hours, so sconcentrations obtained before that time smay not reflect speak levels. levels from 15–30
mg/dL are sconsidered to be within the therapeutic range. Signs and symptoms sof toxicity begin sto
appear at levels higher sthan 30 mg/dL. A 6–hour salicylate slevel higher sthan 100 mg/dL is
considered spotentially lethal and is an indication for hemodialysis. Chronic singestion can increase
sthe half–life to longer sthan 20

Concentration Of Acid-Base Titration
Acid–Base titration is defined as using a solution of known concentration and volume to find the
concentration of a solution with known volume but unknown concentration. Acid–Base titration can
be used when mixing strong acids and strong bases because strong acids and bases neutralize each
other. Phenolphthalein indicators, substances that change color based on pH, can be used to
determine when the titration is complete and when both of the solutions are neutralized. In this
experiment, Acid–Base titration will be used to determine the concentration of 10mL of an HCl
solution by adding a known volume 0.1003 M NaOH solution using a buret. The chemical equation
for this reaction is NaOH(aq)+HCl(aq) → NaCl(aq)+H2O(l). Because the moles of NaOH equals
the moles of HCl, the number of moles of NaOH that are added to the solution in order to neutralize
it will equal the moles of HCl in the solution. The number of moles of NaOH added to the solution
will be used to determine the moles of HCl, which will then be used to determine the molarity of the
HCl solution by dividing the number of moles of HCl by the volume of HCl, according to the
formula: Moles/Volume=Molarity.
Results
The average HCl molarity was found to be 0.090 M. Our actual values were 0.091, 0.091, and
0.089. These molarities were found according to the formula mass/volume=molarity. For example,
0.089 was found by dividing the moles of NaOH added to the solution (8.9x10–4) by the volume of
HCl

Concentration Of Acid-Base Titration
Acid–base titrations are a commonly used laboratory practice, used to determine the concentration
of a particular acid or a particular base by neutralizing them with a known concentration of another
acid or base. Acid–base titrations are tracked and measured with the use of an indicator, which
causes a color change whenever the pH changes between specific values. An indicator is composed
of an acid or base whose conjugate acid or conjugate base has a color different from that of the
original compound.1 The use of the indicator allows us to observe and note the neutralization of a
titration which occurs at the end point. Hydrochloric acid (strong acid) and sodium hydroxide
(strong base), are the most commonly used acid and base in experiments. A strong acid dissociates
(or ionizes) completely in aqueous solution to form hydronium ions (H3O+), while a strong base
dissociates completely in aqueous solution to form hydroxide ions (OH–).1 In this experiment we
used potassium hydrogen phthalate and sodium carbonate as primary standards. These two are
compounds used as primary standards, which are tools that aid in determining the exact
concentration of acids and bases due to their characteristics (See Discussion).
In this experiment, we standardized the strong base sodium hydroxide (NaOH) using potassium
hydrogen phthalate (C8H5KO4) also known as "KHP", as the primary standard and using
phenolphthalein as the indicator. This titration follows the reaction scheme:

Determining The Molarity Of An Acidic Solution
Title: Find the unknown concentration of the acidic solution with use of titration
Problem/Objective: To determine the molarity of an acidic solution given the molarity of a basic
solution
Materials/Equipment: 50 ml–buret, double buret clamp, graduated cylinder (50 ml or 100 ml), 250
ml beaker, dropper pipette, Unknown concentration of HCL (75 ml), phenolphthalein
Procedure: 1. Set up the titration apparatus as indicated by your teacher
2. Place 1250 ml beaker containing 75 ml HCl underneath the buret (buret already set up with the
volume recorded) for titration and apparatus.
3. Record the initial volumes of the acid and base to the nearest 0.1 ml and record HCl volume of 75
ml
4. Add 2–3 drops of phenolphthalein into your beaker of acid ... Show more content on
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Titration has application to be as blood sugar and pregnancy test. For pregnancy test it applies to
titration, as it test the concentration of the blood to identify whether a person is pregnant or not. The
concept is same for blood sugar testing, from the concentration of the blood can help determine the
amount of glucose in the blood (Nurul Syazwanie (Nov, 9, 2011) "Titration uses in everyday life" ).
Titration is not relying use in chemical reaction, but rather other important real life use.
Errors: Percent error: Measured value–Accepted value/Accepted value X 100
0.468–0.5/0.5 X 100= –6.4% percent error
Sources of error: One possible error can be during the process of putting the base solution into acid
beaker until it turns pink. There maybe a possibly that there are more base in the acidic solutions.
This would related to the outcome of the percent error to be negative. If there was less base than the
actually amount than the titration calculation would be lower.
Second potential error could be some incorrect measurement on the buret for base solution volume.
In some case measuring is hard tell in decimal number and is not always accurate, there maybe a
slight chance the measurement could have been lower than usual. If this were the error, this would
affect the outcome of molarity because if there is low measured volume it will ultimately result in a
low

Respiratory Acidosis Essay
Acidosis and Alkalosis are both conditions in which the levels of acids and bases are not controlled.
The typical pH value for the body is between 7.35 and 7.45. If the pH is above 7.45, it's called
alkalosis, and if the pH is below 7.35 it's called acidosis.
Acidosis Acidosis is an increased acidity in the blood, kidneys, lungs, or other body tissues. There
are two types of acidosis, respiratory and metabolic.
Respiratory: Respiratory acidosis is a condition where too much carbon dioxide builds up in the
body, specifically in the lungs. Some of the symptoms of respiratory acidosis are drowsiness,
confusion, shortness of breath, sleepiness, and headaches. If caught early, the symptoms can be
treated and a full recovery is possible. Some common causes of respiratory acidosis are asthma, an
injury to the chest, obesity, sedative misuse, overuse of alcohol, chest muscle weakness, nervous
system issues, and deformed chest structures. Treatment plans for respiratory acidosis include oral
drugs to dilate airways or a CPAP device. A CPAP device is a continuous positive airway pressure
device. This device opens up airways and helps many people breathe ... Show more content on
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Some of the early symptoms of metabolic alkalosis are nausea, numbness, prolonged muscle
spasms, muscle twitching, and hand tremors. Some of the late stage symptoms are dizziness,
difficulty breathing, confusion, stupor (a state of near–unconsciousness), and even coma. Some of
the possible causes of metabolic alkalosis are vomiting, overuse of diuretics (any substance that
promotes the increased production of urine), adrenal disease (when your glands make too much or
not enough hormones), loss of potassium, antacids, ingestion of bicarbonate, laxatives, and alcohol
abuse. Treatment plans for metabolic alkalosis are to take oral medications or supplements to make
up for acid loss, or to combat base

Investigating The Concentration Of A Hydrochloric Acid A...
The objective of the lab was to prepare standardize solution (titrant: NaOH) of sodium hydroxide,
and to determine the concentration of a hydrochloric acid and KHP solution using acid‐base
titration. Standardization is the process of determining the exact concentration (molarity) of a
solution. The molarity (M) of a solution is used to represent the amount of moles of solute per liter
of the solution. Titration is one type of procedure often used in standardization process. A titration is
a technique where a solution of known concentration is used to determine the concentration of an
unknown solution.
In a titration, an exact volume of one substance(NaOH) was reacted with a known amount of
another substance (HCl). The point at which the reaction was complete in a titration is referred to as
the endpoint. We recognized a solution which reached the endpoint: when we saw a solution
completely turned into pink color. A chemical substance known as an indicator was used to indicate
the endpoint. An indicator is a substance that undergoes a distinct observable change (pink color)
when conditions in its solution change. The indicator we used in this experiment was
phenolphthalein because Phenolphthalein is a weak acid. The weak acid is colourless and its ion is
bright pink. And the solution turned pink when we added a basic solution (NaOH) into the solution
because adding hydroxide ions removes the hydrogen ions from the equilibrium which replace them
turning the indicator

Acid Base Balance Research Paper
Acid–base balance in the body is important to maintain our normal functions. The regulation of
hydrogen ions is essential for the body to perform normally and to achieve homeostasis. Our bodies
maintain a pH level between a small margin of 7.35 to 7.45. If the pH level becomes too low, the
body goes into a state called acidosis. On the contrary, if it elevates too far, the body enters into a
state called alkalosis.
Acidosis is caused by an overproduction of acid in the blood, an excessive loss of bicarbonate from
the blood, or by a buildup of carbon dioxide in the blood. Acidosis is categorized into two separate
categories; Metabolic acidosis and Respiratory acidosis. As the pH in the blood lowers, the body
starts to react to the drop. Respirations can become faster and deeper to try and release carbon
dioxide which is slightly acidic, and the kidneys will excrete more acid into the urine. If the body
cannot compensate for the drop in pH, it can enter into a coma.
Metabolic acidosis occurs when the ... Show more content on Helpwriting.net ...
Just as in acidosis, the two types of alkalosis are metabolic and respiratory. When the pH becomes
too high due to too much base in the blood, the body can start to have uncontrolled skeletal muscle
contractions.
Metabolic alkalosis occurs when the body gains too much base or loses too much acid. Some causes
of this would be vomiting for long periods of time where stomach acid is lost or too much fluid and
electrolytes such as sodium or potassium is lost. Ingestion of large amounts of a base can also cause
alkalosis. An overactive adrenal gland and the use of diuretics are also a major cause of metabolic
alkalosis. Treatment of metabolic alkalosis includes the replacement water and electrolyte loss and
treating the underlying issue of alkalosis. Diluted acid can also be given for alkalotic

Mariam Sy May 8, 2014
Acid– Base Titration Lab Write–up
Introduction:
Titration is the process of adding measured volumes of a base or acid with a known concentration to
an acid or base with an unknown concentration in order to determine the unknown concentration.
Volume measurements play an important role in titration. It involves measuring the exact volume of
a solution with a known concentration that will react with a measured volume of a solution that has
an unknown concentration. The solution that has a known concentration is called a standard
solution. Acid– base titration is based on neutralization that occurs in the reaction. If a base is added
to an acid until the acid is neutralized, then the moles of base and the moles of acid will be equal. In
other words, the moles of H+ ions must equal the number of moles of OH– ions. The following
equation can be used to calculate the unknown molarity of an acidic or basic solution: (Molarity of
the acid) * (Volume of the acid) = (Molarity of the Base) * (Volume of the Base) or MaVa = MbVb.
Equivalence point is when there is enough of the standard solution to neutralize the unknown
solution.
The endpoint is when the indicator changes color. The difference between the equivalence point and
the endpoint is that the equivalence point is when the pH of the solution is 7 which means that it is
neutral. However, the endpoint is when the indicator turns either white which shows that the
solution is acidic or pink which

Assignment Notes On Respiratory Acidosis
Assignment Template
Name: Janett Perez Respiratory Acidosis
Respiratory Alkalosis
Metabolic Acidosis
Metabolic Alkalosis
Define condition
Respiratory Acidosis is a condition that occurs when the lungs cannot remove all the carbon dioxide
the body produces. This causes body fluids, mainly the blood to become too acidic.
Respiratory Alkalosis is an acid imbalance due to a condition called hyperventilation which is where
you take in too much oxygen and it decreases the carbon dioxide being produced in your body.
Metabolic Acidosis is a condition that occurs when the body produces excessive quantities of acid or
when the kidneys are not removing enough acid from the body.
Metabolic alkalosis is a metabolic condition in which the pH of tissue is elevated beyond the normal
range (7.35 –7.45) Causing Increased bicaronate in the blood.
List PCO2 levels
The normal range for Pco2 is between 35–45 mmHg. Anything above 45mmhg would be high.
(Tortora & Derrickson, 2013)
The normal ranges are 35–45 mmHg. Anything below 35 mmHg causes respiratory alkalosis.
(Tortora & Derrickson,2013)
N/A
N/A
List HCO3– levels
N/A
N/A
When metabolic acidosis happens, it means that the HCO3 levels drop below 22mEq/liter. (Tortora
&Derrickson, 2013)
When metabolic alkalosis happens, this means the HCO3 levels rises above 26 mEq/Liter. (Tortola
& Derrickson 2013)
List pH levels
Normal arterial blood pH is between 7.35 and 7.45 when respiratory acidosis is in affect your pH
level would be lower than 7.35.

Acid-Base Imbalance
Acid–Base Imbalance
Janet J Memoli
Grand Canyon University NUR 641E
September 30, 2015
Acid– Base Imbalance One of the basic concepts that new nurses need to learn is that homeostasis in
the body is maintained by the acid base balance in the body. That concept is critical when looking at
arterial blood gases. This can help guide the nurse to anticipate what the doctor will order and the
education that she needs to give the patient and the family. This case study should help to illustrate
the point.
Case Study The case study that was given to us is a 22 year old woman who reports being "sick with
the flu" She has been vomiting and having difficulty keeping food and drink down. In addition she
has been taking ... Show more content on Helpwriting.net ...
High pH is alkalosis, low pH is acidosis.. Next you look at carbon dioxide and bicarbonate.
Bicarbonate will go the same way as pH. So if the pH is high then the bicarbonate will be up, if the
pH is low then the bicarbonate will be low. Carbon dioxide is the opposite. If the pH is high then the
carbon dioxide is low, if the ph is low then the carbon dioxide is high ( Fournier, 2011). The possible
causes of this acid base imbalance are the vomiting and the overuse of antacids. As the name implies
it is bicarbonate which has been added to the body. The vomiting reduces the extracellular fluid and
this in turn leads to a release of angiotensin and aldersterone. This release then increases the
bicarbonate absorption and increased hydrogen ion and potassium excreted. This patient may also
have hypokalemia which is very common in metabolic alkalosis and would need to be replaced if it
occurred ( Thomas, 2015). The respiratory rate would also slow to try and compensate for the
alkalosis. The treatment for this patient is to replace the fluid which should stop the release of
angiotensin and aldersterone. This should be accomplished with normal saline. If there is
hypokalemia you would need to supplement with potassium. A proton pump inhibitor would also
need to be used like prilosec to prevent further losses in hydrogen ions. If she was on any diuretics
they need to be discontinued and if renal failure is

There were many things that I learned in Module 7 . Some...
There were many things that I learned in Module 7 . Some of them where: what is the difference
between an acid and a base; what is pH; what is equilibrium, what is Le Châtelier's principle; and
what is oxidation. Here are some of the things that I learned in lesson 07.01 (Acids and Bases) and
lesson 07.02 (Acid–Base Reactions). An acid is a substance that produces hydrogen ions, H+ or
hydrodium ionsH3O+ in solution. There are three "kinds of acids": Arrhenius, BrØnsted–Lowry, and
Lewis Acid. An Arrhenius acid is a substance the increases the concentration of hydrogen ion, H+ or
hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted–Lowry acid is
any substance that donates a hydrogen ion, H+ to another substance. A ... Show more content on
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Here are some of the things that I learned in lessons 07.03 (pH), and 07.04 (Equilibrium). The
formula to calculate the pH of a solution is pH = – log [H3O+]. A titration is a laboratory technique
used to calculate the concentration of a chemical. You are performing an acid–base neutralization
reaction. For example, let's say we have some HCl that we do not know the concentration. We can
react it with a base, such as NaOH. You start by placing the substance of a known concentration in a
buret, such as a 0.25 M NaOH solution. Then, place the chemical that you do not know the
concentration of in a flask under the buret, such as HCl. We need to add an indicator to the flask
since most reactions are colorless. You will 'titrate' the NaOH until you reach the endpoint, which
means that you will allow the chemical in the buret, called the titrant, to flow into the flask. At the
end point, the solution will have a light pink color. Once you determine how much of the titrant,
NaOH you used, you can use stoichiometry to calculate the concentration of the unknown,
HCl.Chemical equilibrium is when the forward and the reverse reactions are occurring at the same
rate. If K is greater than 1, that means there are products than reactants are equilibrium. If K is less
than 1, there are more reactants than products at equilibrium.As more products are made, the rate of
the forward reaction will decrease.The rate of the

With Reference to Acid-Base Balance Explore the Role of...
School of Nursing, Midwifery and Interprofessional Studies.
With reference to acid–base balance explore the role of the respiratory system in maintaining blood
pH?
'We live and die at the cellular level' (Reid, 2011). Homeostasis is crucial for normal cellular
function. Acid–base homeostasis is the part of human homeostasis and refers to the balance between
the production and elimination of H+ hydrogen ions (pH) within the body fluids (William,
Simpkins, 2001, p.236). Metabolic reactions within the cells often produce a huge excess of H+.
Lack of any mechanism for its excretion would lead H+ levels in body fluids rise quickly to the
lethal levels (Tortora, Grabowski 2006, p.1001); therefore the homeostasis of the right H+ levels is
... Show more content on Helpwriting.net ...
Hypoventilation= CO2 = H+ =pH = Acidosis
Hypoventilation= CO2 = H+ =pH = Acidosis CO2
CO2
H+
H+
pH pH Normal blood pH (7.35–7.45)
Normal blood pH (7.35–7.45)
Chemoreceptors stimulate the respiratory centre
Breathing becomes slower and shallower
Breathing becomes slower and shallower
Breathing becomes deeper and faster
Breathing becomes deeper and faster
pH pH H+
H+
CO2
CO2
Hyperventilation=CO2 = H+ =pH = Alkalosis

Hyperventilation=CO2 = H+ =pH = Alkalosis
Fig.2: Respiratory regulation of blood pH.
Simple act of breathing also regulates blood's pH.. When the ventilation rate increases, more CO2
will be excreted, leading to decreased H+ concentration and raise in pH. Contrarily, when the
ventilation rate decreases, less carbon dioxide will get excreted, leading to its accumulation,
therefore increase in H+ and decrease in blood's pH (Tortora, Derrickson, 2009, p.1002).
As we can see, lungs and brain control blood's pH minute by minute.
When the respiratory system fails to control the pH of the blood through ventilation it can lead to
respiratory acidosis or alkalosis.
Respiratory acidosis is an excess of carbonic acid that is caused by conditions resulting in
hypoventilation and CO2 retention. The major effect of acidosis

Acid-Base Titration Lab
The purpose of the Acid–Base Titration Lab was to determine the concentration of sodium
hydroxide by titration against a standard solution. A titration is a laboratory method used to
determine the concentration of an acid or a base in a solution by performing a neutralization reaction
with a standard solution. It detects the equivalence point between the acid and base where they
neutralize each other. The materials used in this procedure were HCL solution, water, ring stand,
burette, burette clamp, unknown concentration of NaOH, phenolphthalein, erlenmeyer flask, and
graduated cylinder. To start the procedure, obtain a burette, and rinse the burette with water and
check if the burette is able to release the solution. Next the ring stand must ... Show more content on
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Trial two started with 0 mL of NaOH and ended at 17.3 mL. On trial three NaOH started at 0 mL
and it ended at 21.5 mL. The molarity of HCL was 0.1 M and its volume was 20 mL. The average of
sodium hydroxide used was 19 mL. Using the dilution equation, 0.1 M of hydrochloric acid
multiplied by 20 mL of hydrochloric acid is 2. Taking 2 divided by 19 mL of sodium hydroxide
gives 0.105 M as the molarity for NaOH. The calculated unknown molarity of NaOH was 0.105 M.
This compares to the known theoretical molarity of NaOH which was 0.1 M. The molarity of
sodium hydroxide from the experiment is close to its theoretical hydroxide meaning the results of
the experiment were accurate. The final volumes of NaOH were also close to each other therefore
the results were both accurate and precise. Hydrochloric acid is an example of an strong acid and
sodium hydroxide is an example of a strong base. When a strong acid and a strong base react, the
neutralize each other. Carrying out a titration between a strong acid and a strong base is done to find
the equivalence point. The point at which chemically equal amounts of the acid and base have been
mixed and neutralized each other. Neutralization between a strong acid and base such as HCl and
NaOH will result in a solution with a pH of 7.0. If the final solution does not have a pH of 7.0 errors
that might have occurred include misjudging of color indicator, using a contaminated

Acid Base Titration
29
EXPERIMENT 3. ACID–BASE TITRATIONS: DETERMINATION OF CARBONATE BY
TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this
experiment a solution of hydrochloric acid is prepared, standardized against pure sodium carbonate,
and used to determine the percentage of carbonate in a sample. An aqueous solution of hydrochloric
acid is almost completely dissociated into hydrated protons and chloride ions. Therefore, in a
titration with hydrochloric acid the active titrant species is the hydrated proton. This species is often
written H3O+, although the actual form in solution is more correctly (H2O)nH+. For convenience
we designate it simply H+. Carbonate in aqueous solution acts as a base; that is, it is able to accept a
... Show more content on Helpwriting.net ...
Calculation shows that [H2CO3] at Point A is negligibly small, so our assumption 2is valid. The
additional assumption that [CO3 ] is essentially 0.1 M also is confirmed because Equations (9) and
(11) show that [HCO3 ] is less than 5% of 2[CO3 ] . Kw Note from this discussion that K = Kb, or
Kw = K2Kb. Thus, if Ka for an 2 acid HA is known, Kb for the corresponding base A– can be
calculated in aqueous
33
solutions. An acid HA and base A– are called a conjugate acid–base pair; HA is the conjugate acid
of A– and A– the conjugate base of HA. pH at Point B. At Point B in Figure 1, 0.5 mole of
hydrochloric acid has been added for each mole of carbonate. The solution now contains an
equimolar mixture of carbonate and bicarbonate. We can calculate the pH at this point by
rearranging Equation (3) to [HCO3] K2 2[CO3 ]
[H+] =
(14)
Since the bicarbonate and carbonate concentrations are equal, the hydrogen ion concentration is
equal to K2, and the pH is 10.3. Accurate calculations of concentrations of species during titrations
must include the effect of dilution by the titrant, but thus far those caused by the addition of
hydrochloric acid have not been considered. To correct calculations of concentrations of the major
components for dilution, multiply each calculated concentration by the factor V/(V + v), where V is

the volume of the original solution and v is the volume of hydrochloric acid added at any point.
Although

Titration Lab
Titration is a technique that is used to determine and analyze the concentration of a substance. It is
based off of mole ratios between the two substances taking part in the lab. Burets are used in the
titration of substances, which are large glass tubes with a valve attached to the bottom to allow the
specially measured amount of substance into another. The amount of each substance must be very
precise and be recorded properly. The analysis of these reactions are usually simplified to a 1:1 ratio,
just as this lab was. Three of the most commonly tested reactions include an acid–base reaction, an
oxidation reaction, and a water analysis. An acid–base reaction consists of finding the amount of the
acid or the base when mixed together, which is what the first part of this lab ... Show more content
on Helpwriting.net ...
The process of titration is the adding of a base drop by drop into a flask of (in this case) 10.0 ml of
acid along with three drops of phenolphthalein. The solution must be swirled continuously
throughout the process until equilibrium is reached which will show a different color of solution
than the beginning. Phenolphthalein is an acid–base indicator commonly used in titrations. Its
molecular formula is C20H14O4 and it is a weak acid that can lose its H+ ions. In titrations, it turns
the solutions pink when the base is added. The first part of the lab is a forward titration, which was
explained above. The second part however, is what is called a back titration. A back titration is the
reaction of an unknown substance with a carefully measured known chemical. The known substance
is then analyzed to see exactly how much remains. Through stoichiometry, we can determine the
amount of the known substance that the unknown substance used during titration. The molecular
formula for Vitamin C, or ascorbic acid, is C6H8O6. Ascorbic acid is an organic compound derived
from glucose. The name "Ascorbic" means (a–) "no" and (scorbutus), a disease caused by not
having enough Vitamin C

Titration : An Acid Base Titration
3. Titration: A technological process in which a solution, known as the titrant, is added to another
solution, called the sample, until the reaction is judged to be complete. In an acid–base titration, an
acid neutralizes a base or vice versa.
Endpoint: The point in a titration analysis at which the addition of the titrant is stopped due to an
observable colour change seen through the presence of an indicator in the sample. The colour
changes is a result of rapid pH change in the sample.
Equivalence point: the point in a titration analysis at which chemically equal amounts of titrant and
sample (acid and base) have been combined.
4. It would be easiest to measure a different pH then what was predicted when the volume of HNO3
added is 25mL, this is because the PH drops rapidly from 11.61 to 2.4 with the addition of a single
mL. However, we cannot predict a PH value at this time either, because that would require finding
the –log of zero which is mathematically impossible. Thus we can only predict that the pH will fall
somewhere between 11.61 and 2.4.
5. a) H2SO4 is a strong acid just like HNO3 but it is a polyprotic acid meaning that their will be two
proton transfer reactions and thus two equivalence points. b) The graph will be mirrored, so that the
PH levels go from low to high rather than high to low, because the sample is now an acid becoming
more basic not a base becoming more acidic.. c) The use of a weak base, causes the equivalence
point to occur at a PH of

Investigating The Amount Of Calcium On The Calcium Oxide...
Discussion:
The purpose of this lab was to calculate the amount of calcium in Kirkland Signature's Calcium
600mg +D3 through the processes of vacuum filtration and acid–base titration. These two methods
were effective in determining the amount of calcium in the calcium supplement with an error of +/–
0.05 g; the amount of calcium stated on the label was 600 mg. The reactions that occurred during the
process of vacuum filtration were:
CaCO3 (s) + 2HCl(aq) → CaCl2 (aq) +CO2 (g) + H2O(l)
CaCl2(aq) + Na2CO3(aq) → CaCO3(s) +2NaCl(aq)
The amounts of calcium calculated from the two trials of vacuum filtration were 0.554 g and 0.573 g
respectively. The calculations from the trials are shown in Equation 2 and Equation 3. The results
from the vacuum filtration were very close to the amount stated on the bottle. The small deviation
from the original could be the result of inadequately removing all of the ground powder from the
mortar and pestle. This caused the original mass of the supplement to be less than what was
expected, hence the smaller final amount. There was a small difference in the procedures between
the two trials of vacuum filtration. During the second trial, more care and attention was given to
make sure that the entire calcium supplement was transferred from the mortar and pestle to the 250
mL Erlenmeyer flask. Because more care was given, the calculated amount of calcium increased by
0.019 g.
The other method used in this lab was an acid–base titration. The

Acid Base Titration Lab Report
Acid Base Titrations
Najib Chowdhury CHM1311–C03 Yayha Albkuri
Introduction:
Acids and Bases
The experiment involves with the investigation of the unknown solutions used and the determination
of their concentrations. The techniques and their expected outcomes are elaborated further in detail
in the following report. For the most part, Arrhenius's definition of an acid and base is employed in
this experiment as it is sufficient for this case. Acid can be represented visually using this equation:
〖HNO〗_3 (aq)⟺ H^(+ ) (aq)+ 〖〖NO〗_3〗^– (aq)
As per Arrhenius's definition, HNO3 donates its H+. Likewise, the base has the same underlying
design. In this case, NaOH donates a hydroxide ion.
NaOH (aq)⟺〖Na〗^+ (aq)+ 〖OH〗^(– ) (aq)
Concentration
For determining the concentration of an acid, it is imperative that the amount (in moles) of an acid
being used is known that is being mixed with a certain amount of water (in litres). The equation for
concentration is:
Concentration (mol/L)=(amount of acid(mol))/(volume of water (L))
Safety Precautions:
The experiment deals with the use of organic solutions that are corrosive in nature, the use of extra
precautions is strongly advised. It is highly recommended that the magnetic stirrer is not disturbed
during the dissolution of different solution, as

Lab Report Acid Base Titration
Title: ACID BASE TITRATION. Objectives: 1. To determine the concentration of acid using
titration. 2. Skills of titration techniques. Apparatus: 1. 250 volumetric flask 2. 10mL measuring
cylinder 3. 25mL pipette 4. 50mL burette 5. 250mL beaker 6. 150mL conical flask 7. Retord stand 8.
White tile 9. Stopwatch 10. Pipette bulb Chemicals: 1. HCl solution 2. 0.1M NaOH solution 3.
H2SO4 solution 4. Distilled water 5. phenolphthalein Introduction. An acid–base titration is the
determination of the concentration of an acid or base by exactly neutralizing the acid/base with an
acid or base of known concentration. This allows for quantitative analysis of the concentration of an
unknown acid ... Show more content on Helpwriting.net ...
For H2SO4: 2 mole of NaOH reacted with 1 mole of H2SO4. 2) Why are HCl and H2SO4 known as
strong acid? * Because they reacted 100%. 3) Give one example of a weak acid and explain why it
called a weak acid. * Ethanoic acid, when it reacted, it do not dissolves 100%. * It only dissolve 4%
and tend to return to its original state. Conclusion. ACID–

Acid–Base Titration
BQ: 1) what is the strength of the antacid?
2) How accurate/precise is this strength?
Safety consideration:
Goggles and gloves must be worn at all time during experiment to prevent any contact with eyes and
skin. If spilled any chemical in gloves throw it away and wear a new one immediately. Handle all
chemical carefully. Handle all carefully to prevent from breaking.
Procedure and Tests:
Week 1 1) 600ml of a 0.5M NaOH solution will be needed, 3MNaOH is provided. Determine how
much of the 3M NaOH will be needed. 2) Determine how many mls of a 0.5M NaOH solution will
be required to titrate 1.2g of potassium hydrogen phthalate to the nolphthalein endpoint. 3) Use
bromothymol blue or ... Show more content on Helpwriting.net ...
It is very likely for this strength not to be accurate because, it is likely to have errors on the previous
calculations and data.
Reading, Reflection:
The main possible source of errors on this experiment is based on the measurement of mass and
volume for the experiment, which could affect moles of NaOH and HCl, could as well affect the
antacid titration. One question I have after this experiment is that, how the increasing of mole of the
tablet would affect the titration? This experimental work can be related to lecture on how acid and
acid bases interact to each other, and also this experiment give a better understanding on term pH. A
real life application for acid base titration is that is use in medicine and most food

Titration Laboratory
Colegio Católico Notre Dame
Caguas, P.R
Laboratory:
Titration of an Acid with a Base
Tristian Pérez Rivera
12–136
AP Chemistry
Professor Judith Martínez PhD
Objective * The purpose of this laboratory is to recreate and understand what titration is.
Hypothesis
* If the experiment works correctly, we should determine the amount of a substance by adding a
carefully measured volume of a solution with known concentration until the reaction of both is
complete.
Materials
* Computer
Pre–lab
1. How will you know when your titration is finished? I will know that the titration is finished when
the color of the indicator changes, meaning that the equivalence point has been reached.
2. Draw and label the pH scale below with acid, base, ... Show more content on Helpwriting.net ...
Phenolphthalein changes from white to pink at a pH of 8.2–10.0. Bromothymol blue changes from
yellow to blue at a pH of 6.0–7.6. In my case, I used Bromothymol blue for all because the
equivalence point for a strong acid being titrated by a strong base is at a point near the neutral
position.
6. (a) Why is it important for the buret to be clean before using? How do you clean a buret?
It is important to clean the buret thoroughly before using it because it will help for the buret to
perform better and will minimize or even prevent error in the experiment.
(b) Why are air bubbles in the buret tip a possible source of error in a titration experiment? How do
you remove air bubbles from the buret tip? Air bubbles in the buret tip can cause error in a titration
experiment because it can cause the reader to read an inaccurate value of the volume in the buret.
One can remove air bubbles by draining several milliliters of the titrant into a waste beaker.

7. Predict the products of these reactions.
(a) HNO3 (aq) +KOH (aq) KNO3 (aq) + H2O (l)
(b) HCl (aq) + Ca (OH) 2(aq) CaCl2 (aq) + 2H2O (l)
(c) NH3 (aq) + H2SO4 (aq) HSO4– (aq) + NH4+ (aq)
8. For the reactions (a) and (b) in question 8, how many moles of the base are required to neutralize
one mole of the acid? How many mL of 0.100 M base are required to neutralize 10.00 mL of 0.100
M acid?
(a) It takes 10.0mL of the 0.100M base to neutralize the 10.0mL of the 0.100M acid

Authors: Quentin McCorvey, Scott McCartney, Craig Mathews, and Ross Mather. T.A. Maia
Popova, Professor Yasmin Jessa. 144 Section C. October 15, 2014.
Abstract:
While the goal of this lab was mainly to be able to perform an acid–base titration. Complete a
traditional titration and then and a pH electrode titration. Calculate the molarity of citric acid from
the titration volume of NaOH. Calculations should be fairly close in average and the ending point
should coincide with the equivalence point. All while effectively being able to compare and contrast
the two methods to detect the endpoints of an acid–base titration.
Introduction:
The goal of this lab is to understand the difference between polyprotic and monoprotic acids and to
be able to understand and perform an acid–base titration.
Method:
Traditional Titration ... Show more content on Helpwriting.net ...
After recording the volume of the NaOH. Obtain the 7–UP in an Erlenmeyer flask at about 40.0 mL
also containing 60.0 mL of water and 5 drops of indicator drops. After each trial repeat these steps.
Add the NaOH solution to the flask in 2 mL increments until a faint pink color appears and remains.
This is the endpoint of the titration. The titrant volume is the initial volume subtracted from the final
volume. After this is completed subtract 4 mL from the titrant volume and rapidly add that amount
to the new trial. Continue by adding NaOH drop wise into the flask until the faint pink color
persists. This should be done 3 times for a total of 4

Lab Report Acid Base Titration
Objective
The purpose of this lab was to perform acid base titrations using a pH electrode to monitor the
equivalence point. Standardized NaOH was titrated with HCl and acetic acid using phenolphthalein
as the indicator. Each titration was analyzed by the following plots to determine the equivalence
point volume: pH vs volume, first and second derivative plot and Gran plot.
Methods
The pH meter and glass electrode were calibrated using buffers of pH 7 and 4. 25.00 mL of HCl
solution was transferred using volumetric pipet to a beaker containing 75.00 mL of water (N2
bubbled), stir bar and phenolphthalein. Initial pH of the solution was recorded. After rinsing the
buret and filling it with NaOH solution (made the first week), the acid was titrated by adding NaOH
in increments to get a 0.25 pH unit change. As the equivalence point approached, NaOH was added
in increments of half a drop to collect as many reading at the equivalence point. After equivalence
point by 1.00 mL, NaOH was added in increments of 1.00 mL until all of the solution was used. pH
for each point was recorded after ~30 s of the addition. In between changing the solutions, pH
electrode was immersed in the buffer of pH 4.
The above procedure was repeated for acetic acid. Beaker containing 25.00 mL of acetic aicd,75.00
mL of water (N2 bubbled), stir bar and phenolphthalein was titrated with the NaOH solution.
Discussion
The purpose of this experiment was to determine the equivalence point of the two reactions:

Titration Of A Concentration And The Acid Base Titration
Summary
The purpose of this experiment was to find the molarity of a concentration and the acid–base
titration. In part A of this experiment, the molarity of an assigned concentration which was 0.040,
was found using formulas that represent molarity. Part B of this experiment, which was titration of
an acid and base, was found by a series of steps that involved dropping Sodium Hydroxide from a
buret into vinegar, until the perfect shade of pale pink occurred. With the Phenolphthalein, too much
acid causes the base to turn a dark pink. The molarity was then found of the titration. So the end
results will determine M HCH3O2.
Introduction A solution is a homogenous mixture of a solvent and one or more solutes. The
substance that dissolves in the solute is the solvent, and the solute is what gets dissolved. Solutions
can vary in concentration in great ratio differences. It is very important to be able to correctly
prepare solutions. There is always a proper amount of solution to be made to have a desired amount
of produced. So in the medical world, too much solute will most likely have harmful effects like
overdosing and too little could result in ineffective treatment. Also the money spent on solutions
could also be another reason for correct preparation of solutions, because the success of the drug has
an effect on future sales and profit. Solutions that are dilute, are weak, and solutions that are
concentrated are strong. A precise means of describing concentration is 1.

Vinegar Lab Report
How Much Acetic Acid Is in Vinegar?
The chemical makeup of certain acids and bases that are not managed reacted properly can be
harmful and a result of improperly measured acids and bases. This could have a negative effect on
humans pertaining to different liquids that could be consumed or physically hazardous to the body.
However, due to decades of research in the department of science, it can be confirmed that ideas like
the HSAB Principle and the Lewis Principle help categorize acids and bases between being harmful
or not and secondarily help humans be more cautious, according to professor Tse–Lok Ho.1
However, experimental these measurements can be specified and determined through titrations.
According to Jakub Ederer and other researchers, titrations have quick and determinable results and
do not require a lot of money and are commonly used for acids.2 The Lab Manual provides an
experiment that includes a titration to determine the moles of acetic acid (HC2H3O2) in a specific
amount of vinegar.3 To follow through with this experiment, the acid–base reaction has a known
molar concentration of NaOH solution that reacts with an unknown molar concentration of acetic
acid to make water and NaC2H3O2, resulting in a titration. Before the initial trial titration, a
thorough cleaning procedure of the buret and materials was necessary to ensure there is no
contamination of other chemicals or solutions. The buret was washed out with soap, tap water, and
distilled water with no

Determine The Identity Of An Unknown Weak Acid Lab Report
Determining the Identity of an Unknown weak acid (Vernier)
Formal Lab Report
Kelli McWatters
August 7, 2017
Chem 1121
Dr. Reed
Objective:
Observe and measure a weak acid neutralization and determine the unknown identity of an unknown
acid by titration.
Introduction:
Within an acid–base titration the titration curve resembles the strengths of the corresponding acids
and bases. A strong acid will correspond with a weak conjugate base, and a weak conjugate acid will
correspond with a strong base. This is based on the Bronsted–Lowry model. The weak acid will
donate protons to the hydroxide ion. Weak acids will have a low Ka value, the Ka value is the
tendency of the acid to dissociate: Ka= [H+] [A–] [HA] Ka is the acid dissociation constant and
[HA] is the concentration of the weak acid . Strong acids usually completely dissociate and has a Ka
value greater than 1. Weak acids don't dissociate completely and have a Ka value much smaller than
1. pKa values are often used for weak acids due to being able to work with whole numbers pKa =–
log Ka During a titration the pH of the solution will be monitored using a pH meter from that we get
a titration curve. The titration curve is then used to determine the equivalent molecular weight and
Ka value of the unknown weak acid, from that we are

Essay On Titration Of Carbonate And Bicarbonate
Determine the total alkalinity of (=[HCO–3 +2[CO2–3]) by preforming a titration with the use of
HCl.
Determine the Bicarbonate content (HCO–3 + OH– → CO2–3 + H2O) by preforming a titration
with the use of NaOH to convert HCO3– to CO2–3.
Calculate the composition of carbonate and bicarbonate in the solution.
Introduction
Acid–base titrations are common laboratory practices that are used to determine the concentration of
either an acid or a base, by neutralizing the substance with a known concentration of an acid or base.
Crude sodium carbonate, also called soda ash, is commonly used as a commercial neutralizing
agent. In this experiment, we will determine the composition of an unknown solid, knowing only
that it contains sodium ... Show more content on Helpwriting.net ...
Using this, the concentration of carbonate can be determined from the total alkalinity (see Results).
Experimental Information
Procedure
At the start of the experiment all the following glassware was cleaned with DI water, and soap; then
dried to remove traces of DI water that remained. The glassware used was a 50mL buret, (3) 150 mL
volumetric flask, a 25mL glass pipet, and a 250mL volumetric flask. 2.5 grams of solid unknown
was added to the 250mL volumetric flask with the use of a funnel, and DI water was filled to the
mark on the 250mL volumetric flask, making sure to rinse the funnel, so the unknown residue
presented on the funnel can rinse down into the flask. After removing the funnel, we diluted to the
mark with DI water, and swirled the flask, until all of the powder was dissolved. This experiment
involved two different titrations. The first titration we observed was for total alkalinity (=[HCO–3
+2[CO2–3]) which was measured by titrating the mixture with 0.1 M HCl to a bromocresol green
end point. After 2L of 0.1M HCl were prepared, and divided among all groups. 25.00–mL aliquot of
unknown solution was pipetted into a 150mL volumetric flask, using bromocresol green as the
indicator, to observe the color change from a tinted light blue to a tinted light green, being the

Solution Of A Weak Acid And Sodium Hydroxide Solution
Objectives:
To conduct a reaction between solutions of a weak acid and sodium hydroxide.
Determine the half–way point of titration of an acid–base reaction.
To calculate the pKa and the Ka for the weak acid.
To calculate Molar Mass of a weak acid from the titration results.
To determine the identity of a weak acid.
Introduction: The purpose of this experiment is to identify an unknown weak acid by titration with a
standard sodium hydroxide solution.
The pH of the titration solution will be monitored using a pH meter. The resulting titration curve
will then be used to determine the equivalent molecular weight and dissociation constant (Ka ) of
the unknown weak acid. These values will then let you determine the identity of the ... Show more
content on Helpwriting.net ...
At the halfway point of each titration, the concentration of acid remaining in the solution is equal to
half of its initial concentration.
At the halfway point of the "Titration 1" the concentration of H2X is
and
Taking the negative log of this yields: pH = pKa
From the titration curve, we can determine the pH at the halfway point of the titration and thus
determine the pKa of the acid. From pKa = Log Ka we can determine the Ka of the acid. Since
this is a diprotic acid, this corresponds to Ka1. This information can be used to help identify the acid
because pKa and Ka values for a large number of mono and polyprotic acids are known.
Table 1. Some Characteristics of Selected Weak Acids
Acid Name Molar Mass, g/mol pKa
Acetic Acid 60.05 4.76
Ascorbic Acid 176.12 4.10 (pKa1)
Benzoic Acid 122.12 4.202
Boric Acid 61.83 9.24 (pKa1)
KHP
204.23 5.4

Maleic Acid 116.07 1.9 (pKa1)
Sodium Phosphate Monobasic
NaH2PO4x H2O 137.99 7.21 (pKa2)
Procedure:
SAFETY NOTE: In case of a spill on the skin of an acid or a base, wash off immediately with
plenty of water for at least 15 minutes. Get medical attention if symptoms occur.
Waste Disposal: Do not return excess amount of NaOH solution into the original container, place it
in the properly labeled waste container instead. Solids can go into the "Solid Waste" jar. All
solutions

A Patient With Respiratory Acidosis Essay
a) In a patient with respiratory acidosis, the partial pressure of CO2 in the plasma (PCO2) rises
above normal levels of 40 mmHg (1). Airway resistance due to asthma, respiratory depression due
to drug use as well as chronic obstructive pulmonary disease all cause hypoventilation, lowering
partial pressure of plasma oxygen (PO2) to below its normal value of approximately 100 mm Hg (1)
and can lead to respiratory acidosis. The equation below describes the equation between CO2 and
H2O with H+ and HCO3–. According to the law of mass action, all reactions tend towards
equilibrium, and any disturbance in the amount of any of the products or reactants will shift the
reaction in a direction which leads to re–establishment of equilibrium. If CO2 concentration rises,
the new chemical equilibrium will favour further production of both H+ and HCO3– through
disassociation of H2CO3. Each additional molecule of CO2 would lead to production of one
molecule of H+ and HCO3–.
〖CO〗_2+H_2 O→ H_2 CO^3→H^++HCO_3^– (1).
Production of H+ will cause plasma pH to fall below 7.4. Normally, increases in H+ concentrations
are buffered mostly by haemoglobin, however buffers can only resist small changes in pH. The
HCO3– levels increase slightly, but are likely to still remain within normal levels of 22 to 26
mEq/L. This is because equilibrium changes in concentrations is slight compared to the large
compensatory changes (1). Renal mechanisms can assist in excreting H+ and reabsorbing HCO3–.

Abstract
By using acid–base titration, we determined the suitability of phenolphthalein and methyl red as
acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with
sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of
acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red.
And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of
the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were
unsuitable because their pH ranges for their color changes did not cover the equivalence points of
the trials in which they were used. However, the ... Show more content on Helpwriting.net ...
Results
Part I: Data and Calculations
Table 2: Titration Data Table
Trial 1 – HCl and NaOH (Strong–Acid + Strong–Base)
Trial 2 – CH3COOH and NaOH (Weak–Acid + Strong–Base)
Trial 3 – NH3 and HCl (Weak–Base + Strong–Acid)
(*) marks equivalence range
Trial 1Trial 2Trial 3
Titrant Volume (mL)
pHTitrant Volume (mL)pHTitrant Volume (mL)pH
0.001.70.003.10.0010.4
5.001.75.004.05.009.7
10.001.710.004.410.009.3

15.001.815.004.815.008.9
20.002.020.005.120.007.9*
21.002.121.005.321.006.0
22.002.122.005.421.503.8
23.002.223.005.522.003.1
24.002.224.005.722.502.9
25.002.325.006.2*23.002.7
26.002.425.506.723.502.6*
27.002.726.009.824.002.5
28.003.026.5010.524.502.4
29.003.3*27.0011.2*25.002.4
30.003.827.5011.426.002.3
30.509.428.0011.627.002.2
31.0010.3*29.0011.728.002.2
31.5010.830.0011.830.002.1
32.0011.031.0011.835.002.0
33.0011.232.0011.840.001.9
35.0011.534.0011.9
40.0011.835.0011.9
40.0012.0
Table 3: Equivalence Point values.
Equivalence Point
Titration of HCl with NaOH7.0

Titration of CH3COOH with NaOH8.6
Titration of NH3 with HCl 5.5
1)Initial pH
See Table 2.
2)Final pH
See Table 2.
3)Equivalence Range
Using Graph 1: The Volume of Titrant Added in order to reach the Endpoint and the Corresponding
pH Values, observe the vertical line of each titration and see the points in which the horizontal lines
intersect it. These points give the

Nucleic Acid Investigation
The purpose of the introductory activity was to analyze the pH of a mixture of a strong base and
weak acid. The purpose of the guided–inquiry lab was to analyze the concentration of sodium
carbonate by titrating the substance using a nitic acid solution.
Introductory Activity
5 mL of both 0.2 M ammonia and 0.1 M acetic acid were placed in separate test tubes and their pH
was determined with pH paper. A mixture was created by pouring both together and its final pH was
recorded. The strength of the acid and base was determined and whether the two had equal
concentration. Each indicator was researched (its colors when it's acidic/basic and its pH transition
range) and phenolphthalein was deemed suitable for this experiment. 5 mL of acetic acid was
poured into a test tube and 1–2 drops of phenolphthalein were added. The initial color was recorded.
10 mL of ammonia was obtained in a graduated cylinder and using the graduated pipet, the base was
added to the acid in 1 mL increments. Upon reaching the equivalence point, the indicator color and
the amount of base required to obtain this point were recorded. The relative concentrations of the
acid and base were then estimated.
Guided–Inquiry Design ... Show more content on Helpwriting.net ...
The indicator methyl red was deemed appropriate. A 60 mL Poorman's buret was placed on a
support stand above a beaker with a magnetic stirrer. The sides of the beaker and flask were rinsed
with water. 100 mL of nitric acid was collected and placed in the beaker below the buret.
Approximately 3 drops of methyl red indicator were added. After being rinsed with water and
sodium carbonate, the buret was filled with 60 mL of nitric acid. The beaker was placed 2 cm under
the buret. Then the sodium carbonate was titrated until the methyl red changed from red to yellow.
The final buret reading was recorded to determine the final volume of the base. The titration data
was used to graph a titration

Chemical Kinetcs – the Hydrolysis of Pna Ester
"Chemical Kinetcs – The hydrolysis of PNA Ester"
Introduction: Reaction of a compound with water can result in a splitting, or lysis, of the compound
into two parts. Organic molecules containing a group of atoms called an ester can be hydrolyzed by
water to form a –COOH group (carboxylic acid) and an HO–– group (alcohol) as follows:
RCOOR' + H2O ( RCOOH + HOR'
This reaction is spontaneous for almost all esters but can be very slow under typical conditions of
temperature and pressure. The reaction occurs at a much faster rate if there is a significant amount of
base (OH–) in the solution. In this lab experiment, the rate of this reaction will be studied using an
ester called para–nitrophenyl acetate (PNA), which produces an alcohol, ... Show more content on
Helpwriting.net ...
|Table 1 |
|Varying Exp |Test Tube|PNA [45mg/0.5L] |(PO4)3– Buffer| |H2O |Catalyst | | | |
|1.5x[PNA] |2 |3 |7 |2 |0 |– |– |– |– |
|1/2 [PNA] |3 |1 |7 |2 |2 |– |– |– |– |
|Imidazole |4 |2 |7 |2 |0 |Imidazole |0.025 |1 |0.005 |
|Super (10x) Imidazole|5 |2 |7 |2 |0 |Super (10x) Imidazole|0.25 |1 |0.05 |
|2–Me. Imid. |6 |2 |7 |2 |0 |2–Me. Imid. |0.025 |1 |0.005 |
|4–Me. Imid. |7 |2 |7 |2 |0 |4–Me. Imid. |0.025 |1 |0.005 |
|Acidic pH 6.5 |8 |2 |6.5 |2 |1 |– |– |– |– |
|Basic pH 7.5 |9 |2 |7.5 |2 |1 |– |– |– |– |
|Basic pH 8.0 |10

A Person 's Normal Ph Range
A person's normal pH range is between 7.35 and 7.45. (Tortora, G., Derrickson, B. H. ,2014–01–22).
This range is important for the body to function properly. There certain conditions that can cause the
pH range to fluctuate. Acidosis is a condition in which the blood pH is below 7.35 and alkalosis is a
condition in which the blood pH is higher than 7.45. Significant changes in pH range can affect
cellular function and possibly lead to death. "Your blood needs the right balance of acid and basic
(alkaline) compounds to function properly". (George, K., 2013)
Respiratory acidosis is a condition that happens when there is too much carbon dioxide in the lungs.
When this happens, the blood becomes too acidic. People with respiratory acidosis will have a pH
less than 7.35 with a PaCO2 greater than 45mm HG. (sitelms.org) This particular form of acidosis
can be caused by diseases of the airways, lungs, and chest. It can also be caused by diseases that
may affect the nerves and muscles that tell the lungs to inflate or deflate. Certain narcotics may
cause this to happen as well. If respiratory acidosis does not become too severe the kidneys will help
to raise the blood pH to the normal range. The kidneys increase the amount of hydrogen it releases
and the reabsorption of bicarbonate. When medical treatment is necessary, it is usually aimed at the
underlying disease, or cause of the condition. (.nlm.nih.gov, 2016) Bronchodilator drugs may be
prescribed to help reverse some types of

Acid Base Balance
Acid–Base Balance
Kelly Heffron
Grand Canyon University NUR–614
September 16, 2015
Acid–Base Balance
The acid base balance is a homeostatic process that aides the body in maintaining a pH in the arterial
blood between 7.35–7.45 (Patient, 2015). The body works together through multi–systems to ensure
that acidity or alkalinity never take over within the blood. The purpose of the following paper is
define the classification of the acid–base balance, define the factors from the case study, explain the
pathophysiology, describe the compensatory mechanisms, pharmacological interventions, and the
educational needs of patients with an imbalance.
Classification
In the following case study, the patient presents with metabolic alkalosis. ... Show more content on
Helpwriting.net ...
Another major factor that the patient did was self–prescribe antacids for the stomach issues (Grand
Canyon University, 2015). Metabolic alkalosis occurs from excessive intake of antacids. Antacids
are calcium carbonate, magnesium hydroxide and sodium bicarbonate (Human Touch of Chemistry,
2015). With the vomiting and loss of gastric secretions, HCO3 began to build–up in the body. For
the stomach upset, the patient began to add more HCO3 formularies to the stomach, which increased
the levels of HCO3 in the body.
Pathophysiology
There are different ways that metabolic alkalosis can occur. Generally, the imbalance occurs from a
loss of hydrogen ions, a shift of hydrogen ions into the intracellular space, and administration of
antacids (Medscape, 2015). Hydrogen ions are lost from the kidneys and the gastrointestinal tract,
which occurs from vomiting and diarrhea. When hydrogen ions are excreted from the body,
bicarbonate ions are added to the intracellular space (Medscape, 2015).
Compensation Mechanism
When homeostasis is disrupted, the body will respond in several ways. Depending upon the
imbalance, the body will work to quickly correct the problem and restore the body to homeostatic
state. There are organ systems involved to correct the issues, like the renal and respiratory systems.
When the body breathes, the lungs blow off carbon dioxide that has built up in the body.
Renal Compensation In the case study, the patient was suffering with

The purpose of this lab is to determine a weak acid and its acid dissociation constant (Ka) through a
process of an acid–base titration. A sample of the unknown weak acid was made into a 100 mL
solution, where 20 mL was take out for titration; phenolphthalein was added in as the indicator.
NaOH, as the titrant, is dripped into the weak acid solution until a slight change in coloration (from
clear to pink) was noted. At this point in time, the titrated solution is diluted with 20 mL more of the
weak acid; the pH is then measured by a pH probe. This process was done a second time for
comparative accuracy. Throughout this lab, there were a few concepts that were used and applied.
This experiment revolved around a titration: the addition ... Show more content on Helpwriting.net
...
The solid given probably was not a pure Hydrogen sulfite ion based compound, therefore bringing
to question the possibility of other compounds inadvertently reacting in the titration. When the acid
was dissolved, some of the impurities might have followed suit and dissipated. If that were so, the
impurities could also take effect on the reaction when the titrant, NaOH, was introduced to the
solution. If the impurity was acidic in nature, it would require the solution to take in more titrant
than necessary for a indicator color change. This would also make the pH (and concurrently the
pKa) at midpoint slightly lower than actuality. Because there is a greater presence of acid, the pH
would be lower, and a lower pH, would mean a lower pKa. Consequently, the acid dissociation
constant would be larger than the accurate value. If the impurity was basic in nature, it would cause
the inverse: it would take less NaOH to titrate the solution until the indicator changes color. A more
basic solution would also make the pH of the solution at midpoint, slightly larger than the needed
value. Ergo, the Ka value would be smaller than that of HSO3–. Another lab error would be from the
usage of phenolphthalein: the indicator's color change is not an instant occurrence. As a result, one
would stop the release of the titrant a little bit of time after the reaction has reached the equivalence
point. This, in turn would mean an

Using Acid Base Titration Methods
Abstract
The purpose of this experiment was to utilize acid–base titration methods to standardize NaOH, and
use the standardized NaOH to find the % KHP in an unknown mixture (unknown #46). The
standardization was precise, with the average molarity being 0.0917±0.3662 moles and each trial
varying by only 0.6621 %. The percent mass of KHP in the unknown sample was 55.75 % with a
percent variation between trials of 0.6621 %, which differed by the actual amount by 0.7883%;
showing the experiment was adequate.
Introduction
Potassium Hydrogen Phthalate (KHP) is an acidic salt compound with a molecular weight of 204.22
grams per mole. KHP is a white crystalline powder and is incompatible with strong oxidizing
agents. Titration is used as a method that allows scientists to determine the precise endpoint of a
reaction and is used to determine the precise quantity of reactant in the titration flask. The endpoint
of a reaction is the point at which the mixture is chemically balanced with equivalent quantities of
acid and base. Titration is used in a variety of fields. Titration is used for the mixing of drugs for
medical purposes as well as defines oils and fats in the food industry, etc. The analyte (titrand) is the
solution with an unknown molarity. The reagent (titrant) is the solution with a known molarity that
will react with the analyte. The molar amount of the titrant that is required for a

Acid Base Titration Lab

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