Greenwich chemistry lab session - titration
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The University of Greenwich is offering a free chemistry practical session on thermometric titration of a strong acid on March 28th from 12:30-3:00 PM. Students will determine the concentration of hydrochloric acid by titrating it with sodium hydroxide and recording the temperature changes. They will draw a graph of temperature vs. volume of acid added and use it to find the endpoint and calculate the concentration of the strong acid. Proper safety procedures will be followed when handling the corrosive acids and bases.
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Thermometric titration
This document discusses thermometric titration, where the endpoint of a titration reaction is determined by measuring the temperature change. Key points:
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- The temperature change observed is directly related to the enthalpy change of the reaction.
- Factors like heat losses, temperature differences between titrant and analyte, and stirring must be controlled for accurate results.
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- The temperature change observed is directly proportional to the heat of reaction and moles of analyte. Second derivatives of temperature curves can precisely locate inflection points.
- Parameters like mixing, probe placement, data density, and software filtering must be optimized for accurate results.
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This document discusses thermometric titration, where the endpoint of a titration reaction is determined by measuring the temperature change. Key points:
- Titrant is added continuously and the temperature change is measured, with the endpoint identified by an inflection point on the temperature curve.
- The temperature change observed is directly related to the enthalpy change of the reaction.
- Factors like heat losses, temperature differences between titrant and analyte, and stirring must be controlled for accurate results.
- Automated systems use burets for precise titrant addition, a thermistor probe for temperature measurement, and software for data collection and endpoint determination.
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- Thermometric titration measures temperature changes that occur during chemical reactions to locate endpoints precisely. It has advantages over subjective visual methods.
- The temperature change observed is directly proportional to the heat of reaction and moles of analyte. Second derivatives of temperature curves can precisely locate inflection points.
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The deviation observed above the base (zero) line is called exothermic transition and below is called endothermic transition.
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LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docx
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Additivity of Heats of Reaction:
Hess’s Law
In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by
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Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the
sum of the heats of reaction for the other two. This concept is sometimes referred to as the
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The reactions we will use in this experiment are:
(1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions.
NaOH(s) Na+(aq) + OH–(aq) H1 = ?
(2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous
solution of sodium chloride.
NaOH(s) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H2 = ?
(3)
Solution
s of aqueous sodium hydroxide and hydrochloric acid react to form water and
aqueous sodium chloride.
Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H3 = ?
In the space below, combine two of the above equations algebraically to obtain the third
equation. Indicate the number of each reaction on the shorter lines.
______ __________________________________________________________________
______ __________________________________________________________________
______ __________________________________________________________________
You will use a Styrofoam cup in a beaker as a calorimeter, as shown in Figure 1. For purposes of
this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is
negligible. Even if heat is lost to either of these, it is a fairly constant factor in each part of the
experiment, and has little effect on the final results. You will make three grand assumptions in
this experiment:
1. The specific heat of solution is equivalent to the specific heat of water.
2. The density of solution is equivalent to the density of water.
3. All solutions are identical in temperature before mixing.
OBJECTIVES
In this experiment, you will
Combine equations for two reactions to obtain the equation for a third reaction.
Use a calorimeter to measure the temperature change in each of three reactions.
Calculate the heat of reaction, H, for the three reactions.
Use the results to confirm Hess’s law.
LabQuest 18
18 - 2 Chemistry with Vernier
MATERIALS
LabQuest 4.00 g of solid NaOH
LabQuest App ring stand
Temperature Probe utility clamp
50 mL of 1.0 M NaOH stirring rod
50 mL of 1.0 M HCl Styrofoam cup
100 mL of 0.50 M HCl 250 mL beaker
100 mL of water
PROCEDURE
Reaction 1
1. Obtain and wear goggles.
2. Connect the Temperature Probe to LabQuest and choose New from the File menu. If you
have an older sensor that does not auto-ID, manually ...
Rates of reaction
Here are the effects on the rate of reaction of changing each condition:
- If the concentration of acid is increased, the rate of reaction will increase. This is because there will be more reactant particles per unit volume, resulting in more frequent collisions between reactants.
- If calcium carbonate powder is used instead of small pieces, the rate of reaction will increase. This is because powder has a larger surface area, allowing for more reactant particles at the interface where the reaction occurs.
- If the volume of acid is increased, the rate of reaction will initially increase but then level off. This is because there will be more reactant particles initially, but the reaction will use them up over time.
- If the
NCHE 211 UNIT 2 VOLUMETRY and Complexometry titration.pdf
This module consists of six study units that are further divided into study sections. The study units include basic concepts, volumetry, gravimetry, surface characterization, atomic spectrometry, and separation methods. The document then provides an overview of analytical chemistry and its branches, classification of quantitative analysis methods, and learning outcomes related to volumetric analysis and titrations. [/SUMMARY]
Chapter 1 Rate of Reactions
The document discusses rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. It describes several factors that affect rate based on collision theory, including surface area, concentration, temperature, catalysts, and pressure. It gives examples of how scientific understanding of rate of reaction enhances quality of life, such as refrigeration, pressure cooking, cutting food into smaller pieces, making margarine, and burning coal.
Titrimetric Methods
This document discusses different types of titrimetry including volumetric, coulometric, and gravimetric titrimetry. It describes key concepts in titrimetric analysis including standard solutions, equivalence points, end points, titration curves, and sources of error. Specific techniques are covered such as back titration, precipitation titrimetry using silver nitrate, and different types of indicators that can be used for argentometric (silver-based) titrations including chromate, fluorescein, and iron (III). Diagrams illustrate the titration process and how curves are affected by concentration and reaction completeness.
INTRODUCTIONChemical reactions are generally accompanied by some.docx
INTRODUCTION
Chemical reactions are generally accompanied by some heat change. The chemical reactions which involve energy changes are referred to as thermochemical reactions. During many chemical reactions, energy is converted to heat energy and result in increase in the temperature of the surrounding. These reactions are called exothermic reactions. Some chemical changes absorb energy from the surrounding and are known as endothermic reactions.
Enthalpy change always result from changes in a chemical system, hence, the heat changes are classified according to the type of chemical reactions. For instance, enthalpy change from the dissolution of a substance is called the heat of solution. The enthalpy change involved in a chemical change stays constant regardless of the route taken during the chemical change provided the initial and final conditions remain the same. This is the Hess' law of constant heat summation.
PROCEDURE
1. The heat of neutralization of HCl (aq) with NaOH (aq).
Using a graduated cylinder, about 50.0mL of 1.0M HCl was carefully measured and transferred into the calorimeter that was setup as instructed. Then 50.0mL ofNaOH into a small beaker. The stirring plate was then switched on and the stirring bar was adjusted until it spun rapidly and smoothly. The time duration was changed to 180 seconds in the LabQuest. The probe was checked to ensure it was placed properly in the calorimeter and the green arrow in the LabQuest was pressed to continue with the experiment. NaOH solution was added into the calorimeter after 40s. After data was taken, a graph was projected onto the display and the data was then analysed as instructed.
2. The heat of solution of NaOH (s)
About 4.00g of solid NaOH was carefully weighedusing a weighing bottle. Then 100mL of distilled water was carefully added into the calorimeter. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s r. The probe was checked to ensure that it was beneath the liquid level. Solid NaOH was poured into the calorimeter after 40s. After data was obtained, it was then analysed using the procedure given.
3. The heat of reaction of HCl (aq) with NaOH (s)
About 55.0mL of 1.0M HCl was carefully measured using and poured into the calorimeter. Using the cylinder, 45.0mL of distilled water was carefully measured and poured into the calorimeter. About 2.00g of solid NaOH was carefully weighed in a capped vial. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s . The temperature probe was properly placed in the calorimeter. Solid NaOH was added to the calorimeter after 40.5s. After the data was obtained, a drop of phenolphthalein indicator was added into the calorimeter and mixed well. The data was then analyzed following the instructions that were given.
DATA
1. The heat of neutralization of HCl (a.
Discussion on rate of reaction =for quiz 1 and 2
The document discusses factors that affect the rate of chemical reactions including temperature, concentration, surface area, and the use of catalysts. It explains how increasing temperature, concentration, or surface area increases the frequency of particle collisions, leading to a faster reaction rate. Catalysts provide an alternative reaction pathway with lower activation energy, allowing more particles to have sufficient energy for reaction. Examples are provided of calculating reaction rates from graphs and sketching how rate curves would change with different conditions.
Volumetric analysis ppt
1) The document discusses volumetric analysis, which is a quantitative chemical analysis method that involves titration. It is defined as determining the concentration of an unknown solution by titrating a known volume of it with a solution of known concentration.
2) Key terms in volumetric analysis are discussed, including titration, titrant, equivalence point, indicator, end point, and titration error.
3) Requirements for volumetric analysis are that the reaction must be complete, stoichiometric, relatively fast, and have a detectable physical or chemical change at the equivalence point that can be identified using an indicator.
E q u i l i b r i u m D e t e r m i n a t i o n o f a n E
E q u i l i b r i u m :
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
P u r p o s e
To determine the equilibrium constant of a reaction.
L e a r n i n g O b j e c t i v e s
Take a reaction to equilibrium by setting up and monitoring a reaction in a reflux apparatus.
Measure the amount of acid at equilibrium by carrying out an acid-base titration.
Apply the information from a balanced chemical equation and data obtained in the laboratory to de-
termine the concentrations of reactants and products at equilibrium.
Calculate the value of the equilibrium constant using data obtained in the laboratory.
L a b o r a t o r y S k i l l s
To set up and monitor a reflux apparatus.
To carry out an acid-base titration.
E q u i p m e n t
Two 50-mL
graduated cylinders
Two 125-mL
Erlenmeyer flasks
1-mL pipet
25-mL buret
Equipment necessary
to assemble the
reflux apparatus
shown in Figure 1.
C h e m i c a l s
Anhydrous ethanol
(ethyl alcohol)
Anhydrous acetic
acid
Concentrated sulfuric
acid
I n t r o d u c t i o n
From the beginning of this course, we have generally assumed that chemical reactions go to completion, that is,
the reaction proceeds in the forward direction until one of the reactants is completely used up. However, many
reactions do not go to completion and are able to move both in the forward and reverse directions simultaneously.
Such a reaction is called a reversible reaction. A double arrow in the chemical equation designates a reversible
reaction, as shown in Reaction 1:
aA + bB −−−⇀↽−−− cC + dD (Reaction 1)
1
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
A reversible reaction has two reaction rates: a forward reaction rate, where the reactants A and B are consumed
andtheproductsCandDareproduced,andareversereactionrate,wheretheproductsCandDareconsumedand
thereactantsAandBareproduced. Allreversiblereactionseventuallyreachapointatwhichtheforwardreaction
rate equals the reverse reaction rate. This point is called equilibrium. At equilibrium, the concentration of
reactants and products do not change with time. It is important to remember that even though the concentration
of reactants and products do not change with time, the reaction has not stopped. Equilibrium is a dynamic state.
The state will persist as long as the reaction conditions remain constant.
A reaction at equilibrium follows the law of mass action which gives the relationship between concentrations
of the reactants and products at equilibrium. According to the law of mass action, the relationship between
concentrations of reactants and products at equilibrium for the above reaction is given in Equation 1:
𝐾eq =
[C]𝑐[D]𝑑
[A]𝑎[B]𝑏
(Equation 1)
Thisrelationshipiscalledtheequilibrium-constantexpression. Theconstant, 𝐾eq, isapositivenumberwhose
value depends on the reaction and temperature.
In today’s experiment, students will be determining the equilibrium constant for the reac
IB IA Chemistry HL Lab
1. The document describes an experiment to determine the equilibrium constant Kc for the esterification reaction of ethanoic acid and ethanol.
2. Initial concentrations of reactants and products were measured and the mixture was allowed to reach equilibrium. Samples were then titrated with sodium hydroxide and the volume added was used to calculate Kc.
3. The experimental value of Kc was found to be 4.80, which has a 20% error from the theoretical value of 4.07 given by the teacher. Sources of error are discussed.
Determination of enthalpies of neutralization
This document outlines several experiments to determine enthalpy of neutralization reactions and apply Hess's law. It describes neutralizing strong acids with strong bases, weak acids with strong bases, and measuring the enthalpies of dissolving hydrochloric acid with ammonia and ammonium chloride in water. The experiments involve measuring temperature changes in a calorimeter when reactants are mixed and using the recorded temperature vs. time graphs to calculate the enthalpies of reaction.
Acid-Base Titration
1) A mathematical titration model is constructed to determine the concentration of an unknown acid through acid-base titration.
2) The model relates the volume of base added to the pH of the solution based on chemical equations describing acid-base reactions and acid dissociation.
3) Using the model and experimental data, the dissociation constant, theoretical concentration, and actual concentration of the unknown acid are calculated, with the actual concentration found to be 0.044465437 M.
experiment Cstr 40l
This experiment involves conducting a saponification reaction between sodium hydroxide (NaOH) and ethyl acetate (Et(Ac)) in a continuous stirred tank reactor (CSTR) to determine the effect of residence time on conversion. A calibration curve will be prepared to relate conductivity measurements to conversion values for the 0.1M NaOH and 0.1M Et(Ac) reaction. The objectives are to determine conversion, the reaction rate constant, and the effect of residence time on conversion.
Scanned with CamScanner1 STANDARIZATION OF A B.docx
This document provides instructions for a two-part experiment involving titration. In part A, students will standardize a NaOH solution by titrating it against a primary standard of KHP. In part B, students will use their standardized NaOH solution to determine the concentration of acetic acid in a vinegar sample through titration. Key steps and concepts discussed include buret usage, endpoint determination, stoichiometric calculations to determine concentration from titration data, and the purpose and characteristics of primary standards.
Rate of reaction diagnostic
The document discusses the key concepts related to the rate of a chemical reaction:
1. The rate of reaction is affected by factors like concentration, temperature, surface area, and presence of a catalyst. A catalyst increases the rate by lowering the activation energy without being consumed in the reaction.
2. Collision theory states that molecules must collide with sufficient energy, called the activation energy, for a reaction to take place. Increasing effective collisions through factors like concentration and temperature increases the rate.
3. A catalyst facilitates the reaction by providing an alternative reaction pathway with lower activation energy, allowing more particles to react per unit time and increasing the rate.
CHM025-Topic-V_Acid-Base-Titrimetry_231215_154125.pdf
This document discusses acid-base titrations and buffer solutions. It begins by defining acid and base dissociation constants (Ka and Kb). It then discusses amphiprotic substances, solvent effects, and the autoionization of water. Next, it covers acid-base titration curves including types of curves and calculations at different points in the titration. It discusses titration of strong acids with strong bases and vice versa. Finally, it defines buffer solutions and the Henderson-Hasselbalch equation. It provides examples of calculating the pH of buffer solutions and how buffers resist pH changes upon dilution or addition of acids and bases.
Kinetic Study of Polymerization of Methyl Methacrylate Initiated by Ce(IV) – ...
1. The document describes a kinetic study of the polymerization of methyl methacrylate initiated by the Ce(IV)–vanillin redox system.
2. The effects of various reactants like Ce(IV), vanillin, H+, and reaction conditions like temperature, ionic strength, and micellar phase on the rate of polymerization and Ce(IV) consumption were examined.
3. The results show that the rate of polymerization increases with increasing concentrations of Ce(IV) and vanillin, and is dependent on [H+], while being independent of changes in [H+]. The activation and thermodynamic parameters were calculated from Arrhenius and Eyring plots.
Kinetics
The document discusses kinetics and the rate law for the decolorization of crystal violet. It describes using a spectroscopic colorimeter to monitor the concentration of crystal violet over time as it reacts with sodium hydroxide. The goals are to determine the overall rate law and rate constant k for the decolorization reaction. Experiments are conducted at different concentrations and the orders are determined by analyzing linear regression graphs of integrated rate laws versus time and concentration. The 1st order graph provided the best correlation, indicating the reaction is first order with respect to crystal violet concentration.
Chemistry Lab Report 2
1) The student conducted an experiment to determine the relationship between the mass of different antacid medicines (Rennie, Kompensan, Talcid) and the volume of hydrochloric acid needed for titration. Different masses of each medicine were reacted with hydrochloric acid and the volume required was measured.
2) The results were presented in tables showing the raw data and averages from multiple trials. As the mass of each medicine increased, the volume of hydrochloric acid needed for titration also increased.
3) Of the three medicines tested, Talcid required the greatest volume of hydrochloric acid on average, indicating it was the most effective at reducing acidity.
rate of rxns.pptx
The document discusses the rate of reaction and factors that affect it. It defines rate of reaction as the change in amount of reactants or products per unit time. The rate depends on several factors:
1) The surface area of solid reactants - Increasing the surface area by reducing particle size increases the rate, as there are more contact points for collisions.
2) Concentration of reactants - Higher concentrations increase the chance of collisions between reactant particles, speeding up the rate.
3) Temperature - Raising the temperature increases the kinetic energy of particles, making successful collisions that overcome the activation energy barrier for reaction more likely.
4) Pressure for gas reactions - Higher pressures increase the rate by squeezing
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Greenwich chemistry lab session - titration
- 1. The University of Greenwich is running a practical session for Chemistry students in Year 13 Assessed Chemistry Practical Lab Session for A2 Thermometric Titration of a Strong Acid Wednesday 28 March at 12.30 – 3.00 pm University of Greenwich, Medway Campus This free session is open to all students on a first come first served basis. Please see accompanying information for further information. Programme: 12.30 Arrival and briefing 1.00 Chemistry Practical session begins 2.30 Post-activity Assessment 3.00 End For bookings and enquiries, contact C.S.Bushnell@greenwich.ac.uk Partnership Division, University of Greenwich at Medway, Pembroke Building, Chatham Maritime ME4 4TB
- 2. Thermometric Titration of a Strong Acid (Time required for this experiment: 1.30 hr with an addition of 30 min for post assessment) Start: 1.00 PM on Wednesday the 28th of March till 3.00 PM Location: Link Lab (School of Science, University of Greenwich, Medway) Aims: The aims of the practical session are to use thermometric titration to determine the concentration of a strong acid HA. Neutralisation is an exothermic reaction and the maximum temperature is reached at the end-point. From your results, you will draw a graph of temperature against the volume of strong acid HA added. Assessment on: Your ability to work carefully and safely, making accurate measurements and detailed observations and record all your results clearly in an appropriate way. Carrying out the titration (reading and recording burette volumes and temperature values accurately). Drawing and interpreting the graph to find the volume added of the strong acid. You will be supplied with the followings: • 1.0 M sodium hydroxide solution • Concentrated hydrochloric acid (HA) The neutralisation point in this titration occurs when the optimum volume of sodium hydroxide solution (needed to exactly neutralise the amount of strong acid used) has been added to the acid. Neutralisation is an exothermic reaction and the maximum temperature is reached at the end-point Partnership Division, University of Greenwich at Medway, Pembroke Building, Chatham Maritime ME4 4TB
- 3. At the end point of the titration of a strong avid and base the temperature is maximum. An addition of a little amount of the acid in solution will take the temperature down. Methods: Transfer 50cm3 of sodium hydroxide solution to a polystyrene cup. Allow it to stand for a few minutes, and then record the temperature of the solution. Add 5.0cm3 of hydrochloric acid from a burette to the cup. Immediately stir the mixture with the thermometer and record its temperature. Repeat the above step until you have added a total of 50.0cm3 of acid (total 10 steps additions of 5.0cm3 HCl). Analysis: Plot a graph of temperature (vertical axis) against total volume of acid added (horizontal axis). Draw straight lines of best fit and extend them until they cross (see diagram above). The point at which the two lines meet corresponds to the volume of acid needed for neutralisation and to the maximum temperature. Record the volume needed for HCl Use information from your graph to calculate the concentration of the acid. Evaluations and post assessments: Comment on your results, their accuracy, and the likely sources of error in the experiment. Consider the limitations of the experiment, and possible improvements to it. Use the equation below to calculate the acid concentration Partnership Division, University of Greenwich at Medway, Pembroke Building, Chatham Maritime ME4 4TB
- 4. C b x Vb = C a x Va Where, Cb = concentration of base (NaOH) Vb = Volume of the base (NaOH) Ca = Concetration of HCl Va = Volume used of HCl Now calculate the volume of HCl needed to neutralise 25cm3 of NaOH 1.0M solutions. At this volume the solution shows the highest temperature during the titration. The concentration for the HCl used is 2.0M. Health and Safety Notes Hydrochloric acid: Corrosive. Refer to Hazcards for correct method to prepare the 2M (approx.) solution. Ethanoic acid: Corrosive. Harmful vapour. Refer to Hazcards for correct method to prepare the 2M (approx.) solution. Sodium hydroxide solid and solutions Sodium hydroxide is very caustic and forms strongly alkaline solutions. Exercise care in handling - wear gloves, Goggles, Labcoats and eye protection. If spilt, wash with a lot of water. Partnership Division, University of Greenwich at Medway, Pembroke Building, Chatham Maritime ME4 4TB