Explanation Explanation To determine : The volume of water added in HA to change the pH from 4.000 to 5 .000 . The concentration of [ H 3 O + ] at pH = 4.000 is 1 . 0 × 10 − 4 M _ . Given Initial volume of HA is 50 .0 mL . The initial pH value of HA at 50 .0 mL is 4 .000 . The final pH value of HA after addition of water is 5 .000 . Formula The pH value is calculated using the formula, pH = − log 10 [ H 3 O + ] (1) Where, [ H 3 O + ] is concentration of hydronium ions. Substitute the initial pH value of HA in the above equation. pH = − log 10 [ H 3 O + ] 4 .000 = − log 10 [ H 3 O + ] [ H 3 O + ] = 1 . 0 × 10 − 4 M _ The concentration of HA at pH = 4.000 is 0 . 0 1 0 1 M _ . The concentration of [ H 3 O + ] is 1 .0 × 10 − 4 M . The value of K a is 1 .0 × 10 − 6 . It is assumed that the initial concentration of HA is x . Make the ICE table for the dissociation reaction of HA . HA( a q ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + A − ( a q ) Initial: x 0 0 Change: − 10 − 4 10 − 4 10 − 4 Equilibrium: x − 10 − 4 10 − 4 10 − 4 The equilibrium constant for the given reaction is, K a = [ H 3 O + ] [ A − ] [ HA ] Substitute the equilibrium concentration values in the above expression. K a = [ H 3 O + ] [ A − ] [ HA ] 1 .0 × 10 − 6 = ( 10 − 4 ) 2 ( x − 10 − 4 ) x = 0.0101 Thus, initial concentration of HA at pH = 4.000 is 0 . 0 1 0 1 M _ . The concentration of [ H 3 O + ] at pH = 5.000 is 1 . 0 × 10 − 5 M . Given Initial volume of HA is 50 .0 mL . The initial pH value of HA at 50 .0 mL is 4 .000 . The final pH value of HA after addition of water is 5 .000 . Substitute the pH value of HA in equation (1). pH = − log 10 [ H 3 O + ] 5

Bundle: Chemistry: An Atoms First Approach, 2nd, Loose-Leaf + OWLv2, 4 terms (24 months) Printed Access Card

2nd Edition

ISBN: 9781305717633

Author: Steven S. Zumdahl, Susan A. Zumdahl

Publisher: Cengage Learning

See similar textbooks

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibri…

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Videos

Question

Chapter 13, Problem 173CP

Interpretation Introduction

Interpretation: The volume of a weak acid HA , its acid dissociation constant and pH value is given. The volume of water added in HA to change the pH from 4.000 to 5.000 is to be calculated.

Concept introduction: The measure of concentration of hydrogen ions is known as pH .

The process of reduction of concentration of a solute in a solution is known as dilution.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 13, Problem 172CP

Chapter 13, Problem 174CP

Students have asked these similar questions

The equilibrium constant for an acid is called the acid ionization constant (Ka). If acetic acid (weak acid, HC2H3O2) is placed into water, it ionizes to H+ and C2H3O2- with a Ka of 1.82 x 10-5. Determine the pH of the solution when 20.0 g HC2H3O2 (s) is added to water, with a final volume of 1000. mL?

The ka of an unknown acid, HYO₂, is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1 M solution of HYO₂?

How many grams of sodium fluoride (NaF) need to be dissolved in 130 mL of a 1.56 M hydrofluoric acid (HF, Ka = 6.8 × 10−4) solution, so that the pH of the solution is 3.42? Report your answer to THREE significant figures.

Chapter 13 Solutions

Bundle: Chemistry: An Atoms First Approach, 2nd, Loose-Leaf + OWLv2, 4 terms (24 months) Printed Access Card

Ch. 13 - Define each of the following: a. Arrhenius acid b....Ch. 13 - Define or illustrate the meaning of the following...Ch. 13 - Prob. 3RQ Ch. 13 - How is acid strength related to the value of Ka?...Ch. 13 - Two strategies are followed when solving for the...Ch. 13 - Prob. 6RQ Ch. 13 - Prob. 7RQ Ch. 13 - For conjugate acidbase pairs, how are Ka and Kb...Ch. 13 - What is a salt? List some anions that behave as...Ch. 13 - For oxyacids, how does acid strength depend on a....

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Solution Summary: The author calculates the volume of a weak acid HA, its acid dissociation constant, and its value using the formula.

Concept explainers

Videos

Want to see the full answer?

Chapter 13 Solutions