KNPE 153 Study Guide - Final Guide: Equivalence Point, Sodium Hydroxide

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22 Feb 2021

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[insert a brief statement of your purpose here. You may reference the lab instructions or text book pages for details] [insert a very brief overview of your procedure here. You may use a reference to the details in the lab. Instructions to avoid rewriting the whole thing here. ] Questions: calculate the number of moles of naoh used at the equivalence point that you used. [insert your answer here: determine the number of moles of the diprotic acid, h2x. [insert your answer here: calculate the molecular weight of the diprotic acid in g/mol using the mass of diprotic acid that you measured in the first step of the procedure. [insert your answer here: from the list of five diprotic acids, identify the unknown diprotic acid that you used. [insert your answer here: determine the percent error for the molecular weight value you calculated in step 30.

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CHM 1360 Spring 2021 Name __________________________

Lab 1 Buffers Worksheet

Type your answers to the following questions. Make sure to use complete sentences. For images that need to be hand drawn, take a digital picture of your image and insert it into your worksheet.

(0.5 point) Insert your lab notebook image of the pH plot from your preparation of the acetate buffer.
(1.5 point) Draw the Lewis structures for acetic acid (CH₃COOH) and acetate (CH₃COO^-). On each structure, label the carboxylic acid or carboxylate functional group. Also, label the acidic hydrogen (if it has one).
(2 points) In the first experiment, you prepared a buffer by combining solutions of acetic acid and sodium acetate.
1. (1 point) Write the chemical equation for the equilibrium of acetic acid and acetate in water. Include the states of the reactants.
2. (1 point) Write a net ionic equation that shows how this buffer neutralizes added acid (HCl).
3. (1 point) Write a net ionic equation that shows how this buffer neutralizes added base (NaOH).
In the second part of Experiment 1, you added water to the buffer solution which diluted it by a factor of two.
1. (1 point) Write the chemical equation for the equilibrium of acetic acid and acetate in water. Include the states of the reactants.
2. (0.5 point) Did the pH of the solution change? Briefly explain your observation.
3. (0.5 point) Which buffer solution would have a greater buffer capacity, your acetate buffer before the extra water was added, or the buffer solution that had been diluted? Explain.
4. (0.5 point) For your diluted acetate buffer, if you then added 50 mL of 0.50 M H₂SO₄ to the solution how would you expect the pH to change? Explain your answer.

(1 point) Which of the following could be added to a solution of monobasic dihydrogen phosphate (KH₂PO₄) to produce a buffer? Briefly explain your answer(s).

Dibasic monohydrogen phosphate hydrochloric acid sodium chloride

A) hydrochloric acid only
B) sodium chloride only
C) Dibasic monohydrogen phosphate (K₂HPO₄) only
D) Dibasic monohydrogen phosphate (K₂HPO₄) and sodium chloride

(a) (1 point) The average human contains 5.0 liters of blood having a pH of 7.35. Calculate the number of moles of H₃O⁺ at 25 ^o (Report the correct number of SigFigs in your final answers).

(b) (1 point) If a person’s blood pH falls to 7.25, how many more moles of H₃O⁺ are present at 25 ^oC?

(a) (0.5 point) Write a chemical equation to summarize what was happening in the phenol red solution in the flask in Experiment 2.

(b) (0.5 point) Does exhaling CO₂ help raise or lower the pH of the blood? Explain, using the equation you wrote for part (a).

(1 point) At pH 3.0, the amino acid glycine has the structure shown here. Draw the structure of this molecule at pH 12.0.

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KNPE 153 Study Guide - Final Guide: Equivalence Point, Sodium Hydroxide

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