Calculations for chemistry_is_p_hun_
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The document provides instructions for students to complete calculations to design a buffer of their assigned pH for a chemistry lab experiment. Students are told to use provided resources to determine the appropriate acid-salt pair, calculate concentrations and volumes of solutions needed, and show all work for their teaching assistant to verify before starting the experiment.
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This document provides information about buffers and how to prepare a buffer solution in the laboratory. It defines a buffer as a solution that can maintain a constant pH level when small amounts of acid or base are added. Buffers are composed of an acid and its conjugate base. The key properties that should match the desired pH are the acid's pKa value and that its conjugate base only differs by one hydrogen ion. The document outlines how to calculate the mass of salt needed using the Henderson-Hasselbalch equation and dilute the acid solution, and describes various methods for measuring the pH of buffer solutions. It also defines buffer capacity and how it can be experimentally determined.
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Buffers maintain pH through small additions of acid or base and are composed of an acid and its conjugate base, with the pKa slightly above the desired pH. Dilutions can be calculated using the dilution formula of M1V1 = M2V2. The pH of solutions can be determined through litmus paper, pH paper, indicators, or a pH meter. Calculations must be completed and checked by the TA in advance of the experiment.
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The document describes the materials and methods used in a titration lab experiment. Materials included a pH probe, buret, beakers, stir plate, balance, pipette, and NaOH and KHP solutions. The method involved standardizing a NaOH solution by titrating it into KHP and measuring the pH, then using the standardized NaOH to titrate two unknown acids and calculate their identities based on titration curves and pKa values.
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The pH scale measures how acidic or basic a solution is on a scale from 0-14, with 0-7 being acidic and 7-14 being basic/alkaline. The pH is defined as the negative log of the hydrogen ion concentration. A pH of 7 indicates a neutral substance, like water. Examples show how to calculate the pH from given hydrogen ion concentrations using the logarithmic definition of pH.
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The document is a student assignment that includes responses to three questions about process control systems.
In the first question, the student describes a manual process control system to measure and adjust the pH of a campus lake. The control variable is the pH reading, the manipulated variable is adding an acidic solution, and the disturbance is domestic waste in the lake.
The second question asks to automate the control system. The student describes an automatic system with a pH probe connected to a controller that regulates an acid metering pump based on pH readings to neutralize water flowing into a treatment tank before it exits.
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This document describes procedures for potentiometric titration experiments involving aspirin, vinegar, and sodium carbonate samples. Potentiometric titration uses a pH electrode and reference electrode connected to a pH meter to monitor pH changes during titration. For the aspirin experiment, an aspirin tablet is dissolved and titrated with sodium hydroxide while pH is recorded. The vinegar experiment involves titrating a vinegar sample with hydrochloric acid. For sodium carbonate, the sample produces two equivalence points when titrated with hydrochloric acid due to its carbonate ions. Data analysis involves calculating percent composition and errors from the titration curves and derivative plots.
Experimental Methods Det 3
The document describes experimental methods conducted over two days. On day 1, a 0.1M NaOH solution was prepared and used to titrate an acid mixture potentiometrically, recording pH and burette readings at each addition. The NaOH was also standardized by titrating potassium hydrogen phthalate and recording the volume needed to reach the endpoint. On day 2, the pH electrode was recalibrated and the potentiometric titration was repeated with dropwise NaOH additions near the equivalence points. The NaOH was standardized again.
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This document provides information about buffers and how to prepare a buffer solution in the laboratory. It defines a buffer as a solution that can maintain a constant pH level when small amounts of acid or base are added. Buffers are composed of an acid and its conjugate base. The key properties that should match the desired pH are the acid's pKa value and that its conjugate base only differs by one hydrogen ion. The document outlines how to calculate the mass of salt needed using the Henderson-Hasselbalch equation and dilute the acid solution, and describes various methods for measuring the pH of buffer solutions. It also defines buffer capacity and how it can be experimentally determined.
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Buffers maintain pH through small additions of acid or base and are composed of an acid and its conjugate base, with the pKa slightly above the desired pH. Dilutions can be calculated using the dilution formula of M1V1 = M2V2. The pH of solutions can be determined through litmus paper, pH paper, indicators, or a pH meter. Calculations must be completed and checked by the TA in advance of the experiment.
Acid base
The document describes the materials and methods used in a titration lab experiment. Materials included a pH probe, buret, beakers, stir plate, balance, pipette, and NaOH and KHP solutions. The method involved standardizing a NaOH solution by titrating it into KHP and measuring the pH, then using the standardized NaOH to titrate two unknown acids and calculate their identities based on titration curves and pKa values.
Ph part 1
The pH scale measures how acidic or basic a solution is on a scale from 0-14, with 0-7 being acidic and 7-14 being basic/alkaline. The pH is defined as the negative log of the hydrogen ion concentration. A pH of 7 indicates a neutral substance, like water. Examples show how to calculate the pH from given hydrogen ion concentrations using the logarithmic definition of pH.
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The document is a student assignment that includes responses to three questions about process control systems.
In the first question, the student describes a manual process control system to measure and adjust the pH of a campus lake. The control variable is the pH reading, the manipulated variable is adding an acidic solution, and the disturbance is domestic waste in the lake.
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This document describes procedures for potentiometric titration experiments involving aspirin, vinegar, and sodium carbonate samples. Potentiometric titration uses a pH electrode and reference electrode connected to a pH meter to monitor pH changes during titration. For the aspirin experiment, an aspirin tablet is dissolved and titrated with sodium hydroxide while pH is recorded. The vinegar experiment involves titrating a vinegar sample with hydrochloric acid. For sodium carbonate, the sample produces two equivalence points when titrated with hydrochloric acid due to its carbonate ions. Data analysis involves calculating percent composition and errors from the titration curves and derivative plots.
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This document provides instructions for students to complete pre-lab calculations to design a buffer solution for a chemistry lab experiment. It specifies that students must determine the acid/salt pair to use based on an assigned pH value between 1 and 8. It then outlines the calculations needed to determine the amounts of acid and salt to measure out, including molar concentrations and masses, using the dilution equation and Henderson-Hasselbalch formula. Students are reminded to show their work and have their calculations verified before starting the experiment.
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BUFFER.ppt
The document describes how to prepare an acetate buffer using two methods: 1) Titration of acetic acid with sodium hydroxide and 2) Using the Henderson-Hasselbalch equation. For the titration method, acetic acid is titrated with sodium hydroxide and the pH is monitored to determine the pKa. For the Henderson-Hasselbalch method, the desired pH, pKa, and concentrations are used to calculate the ratios of acetic acid and sodium acetate needed to make a 0.1M buffer at pH 4.86. The solutions are then mixed and the final pH is checked to ensure it is as desired.
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This document provides instructions and background information for an experiment on calculating reaction rates. It includes:
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- An explanation that increasing the concentration of sodium thiosulfate increases the rate of reaction because there are more particles closer together, leading to more collisions.
- Instructions to complete three out of five experimental methods and record results by sketching graphs.
- Background definitions of "rate of reaction" and how to calculate the rate.
- A sample experiment measuring carbon dioxide production from the reaction of calcium carbonate and hydrochloric acid over time.
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This document outlines an experiment to determine how temperature affects the rate of reaction between sodium thiosulfate and hydrochloric acid. It describes the independent variable as the temperature of the hydrochloric acid ranging from 0°C to 80°C. The dependent variable is the time for a cross drawn on paper to become invisible when placed behind a test tube containing the reaction. The method involves timing how long it takes for the cross to disappear at each temperature, with results recorded in a table. The conclusion states that higher temperatures led to faster reaction times, supporting the particle collision theory that increasing temperature causes particles to move faster and collide more frequently.
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This document provides instructions for students to complete pre-lab calculations to design a buffer solution for a chemistry lab experiment. It specifies that students must determine the acid/salt pair to use based on an assigned pH value between 1 and 8. It then outlines the calculations needed to determine the amounts of acid and salt to measure out, including molar concentrations and masses, using the dilution equation and Henderson-Hasselbalch formula. Students are reminded to show their work and have their calculations verified before starting the experiment.
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This experiment involves preparing two buffer solutions using acetic acid and sodium acetate and measuring the pH of the buffers as strong acid and base are added. Students will prepare a buffer by mixing acetic acid and sodium acetate, and another by partially neutralizing acetic acid with sodium hydroxide. They will then measure the pH of the buffers as hydrochloric acid and sodium hydroxide are added. Students will also measure the pH of water and a diluted buffer solution with acid and base additions for comparison. The goal is to observe how buffers resist changes in pH when acids or bases are added compared to water.
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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
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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
Measurement of Hydrogen Ion Concentration (pH)
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Introduction According to the definition of Arrhenius.pdf
1) The document describes the process and results of titrating a strong acid (HCl) and weak acid (acetic acid) with a base (NaOH) to determine the concentration of the base and equilibrium constant of acetic acid.
2) pH values were recorded during each titration and graphs were plotted from which the concentration of NaOH was calculated to be 0.108 M and the equilibrium constant of acetic acid was calculated to be 1.028 x 10-5 units.
3) Precautions must be taken when handling chemicals and disposing of wastes to avoid skin burns and ensure accurate results.
06 microscale titration_fa06
The document discusses acid-base titration, including the analyte, standard, neutralization reaction, equivalence point, and procedure. It explains that an acid-base titration involves titrating an acid with a base until the moles of H+ equal the moles of OH-. It also discusses using a pH sensor and indicator to determine the equivalence point, and using stoichiometry to calculate unknown concentrations from experimental data.
lolghj.ppt
This document provides an overview of buffer solutions for A-level chemistry students. It defines a buffer solution as "solutions which resist changes in pH when small quantities of acid or alkali are added." It explains that acidic buffer solutions are made from a weak acid and its salt, while alkaline buffers use a weak base and its salt. Common uses of buffer solutions include regulating pH in biological systems and household/cosmetic products. The document also provides details on the action of buffer solutions, ideal concentrations, calculating pH, and salt hydrolysis reactions.
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This document provides an introduction to acid-base chemistry concepts including the definitions of acids and bases according to Arrhenius and Bronsted-Lowry, and the differences between strong and weak acids. It describes acid-base titration procedures for a strong acid (HCl) and weak acid (acetic acid) against a strong base (NaOH). Graphs of pH versus volume of base added are presented and used to calculate the concentration of NaOH and the equilibrium constant for acetic acid. Precautions for safe chemical handling are also outlined.
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.
Bio 1121 unit 2 written assignmentdirectionsaccurately meas
This document provides instructions and questions for an assignment on preparing and working with phosphate buffered saline (PBS) solutions. Students are asked to calculate molecular masses and molar concentrations of compounds used to make a 10x concentrate of PBS, then use this to prepare a 1x working solution. They are also asked questions about laboratory techniques like weighing chemicals, measuring volumes, and adjusting pH.
Similar to Calculations for chemistry_is_p_hun_ (20)
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
Introduction According to the definition of Arrhenius.pdf
Introduction According to the definition of Arrhenius.pdf
Scanned with CamScanner1 STANDARIZATION OF A B.docx
Scanned with CamScanner1 STANDARIZATION OF A B.docx
Bio 1121 unit 2 written assignmentdirectionsaccurately meas
Bio 1121 unit 2 written assignmentdirectionsaccurately meas
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This document outlines academic offenses and plagiarism policies for chemistry labs at the University of Kentucky. It defines plagiarism as using another's words or ideas without proper attribution. Examples of academic offenses include changing lab data, copying from others' work, sharing unauthorized materials during exams, and falsifying absences. Students must write lab reports individually and are prohibited from sharing work. Penalties for offenses include failing grades and academic misconduct records. The department takes all offenses seriously and will penalize any involved students according to university rules.
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Calculations for chemistry_is_p_hun_
- 1. Calculations for Chemistry is pHun!
- 2. Reminders Complete these calculations before you come to lab. You will not be able to start the experiment until you have completed the correct calculations and your TA has verified your buffer system. Show all work so your TA can help you find your mistake.
- 3. Preparation Access the PreLab assignment on Chem21labs.com. There you will find your assigned pH. Value is between 1 and 8 pH values are given in increments of 0.5 (i.e. 1.0, 1.5, 2.0, etc)
- 4. Preparation Go to “Blackboard”, “Experiments” and find the table of available acids and salts. Determine which acid/salt pair you should use to make a buffer with your assigned pH. The pH should be within ± 1 of the pKa value of the acid. Find the concentration of the acid that will be available.
- 5. Calculations Use the dilution equation to determine the volume of your acid needed to prepare 100 mL of a 0.100 M solution M 1V1 = M 2V2
- 6. Calculations Calculate the molar mass of the salt Your salt should contain the conjugate base of your acid Include hydrates (water molecules) when calculating the molar mass
- 7. Calculations Use the Henderson-Hasselbalch formula to calculate the concentration of your conjugate base The concentration of acid should be 0.100 M [conjugate base] pH = pK a + log [acid]
- 8. Calculations Use the concentration of base, the volume (100 mL) and the molar mass to calculate the mass of salt needed to prepare your buffer.