INTRODUCTION TO CHEMISTRY-ACCESS
5th Edition
ISBN: 9781260518542
Author: BAUER
Publisher: MCG
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Chapter 13, Problem 137QP
Interpretation Introduction
Interpretation:
The acid which produces a buffer solution when it is mixed with sodium salt is to be identified.
Concept Introduction
There are two types of buffer solutions that exist that are, acidic and basic buffer. Acidic buffer is produced when weak acid is mixed with sodium or potassium salt of weak acid. Basic buffer is produced when weak base such as ammonia or ammonium hydroxide is mixed with ammonium chloride salt.
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INTRODUCTION TO CHEMISTRY-ACCESS
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.arrow_forwardExplain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.arrow_forwardIdentify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forward
- Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.arrow_forwardExplain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.arrow_forwardConsider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forward
- Calculate the pH of these buffers.arrow_forwardIdentify each pair that could form a buffer. (a) HCl and CH3COOH (b) NaH2PO4 and Na2HPO4 (c) H2CO3 and NaHCO3arrow_forwardWhat is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.arrow_forward
- A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the most likely value for the buffer solution pH after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?arrow_forwardConsider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0arrow_forwardWhat is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.arrow_forward
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