Explanation Calcium hydroxide is a strong base and it completely dissociates in water. This can be represented as follows; Ca(OH) 2 ( a q ) → Ca 2 + ( a q ) + 2 OH − ( a q ) The concentration of calcium hydroxide is assumed as 1.0 mol ⋅ L − 1 . Therefore, 1.0 mol ⋅ L − 1 of Ca(OH) 2 dissociates to give 1.0 mol ⋅ L − 1 of Ca 2+ and 2.0 mol ⋅ L − 1 of OH − . The concentration of OH − is found as 2.0 mol ⋅ L − 1 . The equation for autopyrolysis constant can be given as follows; K W = [ H 3 O + ] [ OH − ] (1) Rearranging the above equation to obtain concentration of hydronium ion as shown below; [ H 3 O + ] = K W [ OH − ] (2) Substituting the value of autopyrolysis constant and concentration of hydroxide ion in equation (2), the concentration of hydronium ion is calculated. [ H 3 O + ] = 1.0 × 10 − 14 mol 2 ⋅ L − 2 2.0 mol ⋅ L − 1 = 0.5 × 10 − 14 mol ⋅ L − 1 = 5.0 × 10 − 15 mol ⋅ L − 1 Hence, the concentration of hydronium ion is 5.0 × 10 − 15 mol ⋅ L − 1 . The pH of the solution can be calculated using the formula of pH as follows: pH = − log [ H 3 O + ] = − log ( 5.0 × 10 − 15 mol ⋅ L − 1 ) = 14

Chemical Principles: The Quest for Insight

7th Edition

ISBN: 9781464183959

Author: Peter Atkins, Loretta Jones, Leroy Laverman

Publisher: W. H. Freeman

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Question

Chapter 6, Problem 6B.2E

Interpretation Introduction

Interpretation:

Difference in the pH value of the two calcium hydroxide solutions has to be given.

Concept Introduction:

Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows;

pH=−log[H3O+]

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Chapter 6, Problem 6B.1E

Chapter 6, Problem 6B.3E

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Chapter 6 Solutions

Chemical Principles: The Quest for Insight

Ch. 6 - Prob. 6A.1AST Ch. 6 - Prob. 6A.1BST Ch. 6 - Prob. 6A.2AST Ch. 6 - Prob. 6A.2BST Ch. 6 - Prob. 6A.3AST Ch. 6 - Prob. 6A.3BST Ch. 6 - Prob. 6A.1E Ch. 6 - Prob. 6A.2E Ch. 6 - Prob. 6A.3E Ch. 6 - Prob. 6A.4E

Knowledge Booster

Difference in the pH value of the two calcium hydroxide solutions has to be given. Concept Introduction: Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows; pH = − log [ H 3 O + ]

Solution Summary: The author explains that the difference in the pH value of two calcium hydroxide solutions is 1.29.

Interpretation:

Difference in the pH value of the two calcium hydroxide solutions has to be given.

Concept Introduction:

Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows;

pH=−log[H3O+]

Want to see the full answer?

Chapter 6 Solutions

Difference in the pH value of the two calcium hydroxide solutions has to be given. Concept Introduction: Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows; pH = − log [ H 3 O + ]

Solution Summary: The author explains that the difference in the pH value of two calcium hydroxide solutions is 1.29.

Interpretation: Difference in the pH value of the two calcium hydroxide solutions has to be given. Concept Introduction: Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows; pH=−log[H3O+]

Want to see the full answer?

Chapter 6 Solutions

Interpretation:

Difference in the pH value of the two calcium hydroxide solutions has to be given.

Concept Introduction:

Negative logarithm of the concentration of hydronium ion is the pH of solution. This can be given in equation form as follows;

pH=−log[H3O+]