Please answer all questions. INSTRUCTIONS: Solve the following problems. Show all pertinent calculations. If computing forthe final answer requires more than one step, express initial decimals of numerical values in twodecimal places. Final answers will also be expressed in two decimal places and enclose them ina box.1. What is the pH of a 0.500 M solution of acetic acid? Ka = 1.77x10-52. What is the pH of a solution that contains: 0.333 benzoic acid and 0.252 M sodiumbenzoate? The pk of benzoic acid is 4.20.3. What is the pH of a solution that contains: 0.050 M trimethylamine and 0.066 Mtrimethylamine hydrochloride? The pk of trimethylamine is also 4.20.4. What is the pH of a solution of pyruvic acid that contains [ CH3C-COO2 ] = 0.435 Mand [CH3COCOOH] = 0.260 M. Ka = 3.16x10-3

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INSTRUCTIONS: Solve the following problems. Show all pertinent calculations. If computing for the final answer requires more than one step, express initial decimals of numerical values in two decimal places. Final answers will also be expressed in two decimal places and enclose them in a box. 1. What is the pH of a 0.500 M solution of acetic acid? Ka = 1.77x10-5

INSTRUCTIONS: Solve the following problems. Show all pertinent calculations. If computing for the final answer requires more than one step, express initial decimals of numerical values in two decimal places. Final answers will also be expressed in two decimal places and enclose them in a box. 1. What is the pH of a 0.500 M solution of acetic acid? Ka = 1.77x10-5

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 26QAP: Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution...

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Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?
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Differentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?
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Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?