Explanation The equilibrium reaction is given below. H 3 B O 3 ( a q ) + H 2 O ( l ) ⇌ H 2 B O 3 − ( a q ) + H 3 O + ( a q ) The acid ionization constant can be written as given below. K a = [ H 2 B O 3 − ] [ H 3 O + ] [ H 3 B O 3 ] A table can be set up as shown below. H 3 B O 3 ( a q ) H 3 O + ( a q ) H 2 B O 3 − ( a q ) I n i t i a l c o n c . ( M ) 0.10 1.0 × 10 − 7 0 C h a n g e i n c o n c . ( M ) − x + x + x E q u i l i b r i u m c o n c . ( M ) 0.10 − x x x The concentration of H 3 O + comes from its autoionization that is 1

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Publisher: Cengage Learning

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Chapter 14, Problem 65QRT

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The pH of a 0.10 M solution of boric acid has to be calculated.

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Chapter 14, Problem 64QRT

Chapter 14, Problem 66QRT

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Chapter 14 Solutions

Chemistry: The Molecular Science

Ch. 14.1 - Identify each molecule or ion as a Brnsted-Lowry...Ch. 14.1 - Using Le Chatelier’s Principle Use Le Chatelier’s...Ch. 14.1 - Prob. 14.3E Ch. 14.1 - Complete the table. Ch. 14.1 - Prob. 14.4E Ch. 14.1 - Prob. 14.5E Ch. 14.2 - Prob. 14.6CE Ch. 14.2 - Prob. 14.7E Ch. 14.3 - Prob. 14.2PSP Ch. 14.3 - Prob. 14.3PSP

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The p H of a 0.10 M solution of boric acid has to be calculated.

Solution Summary: The author calculates the pH of a 0.10M solution of boric acid water. The equilibrium reaction is given below.

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Interpretation:

The pH of a 0.10 M solution of boric acid has to be calculated.

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Chapter 14 Solutions

The p H of a 0.10 M solution of boric acid has to be calculated.

Solution Summary: The author calculates the pH of a 0.10M solution of boric acid water. The equilibrium reaction is given below.

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Interpretation: The pH of a 0.10 M solution of boric acid has to be calculated.

Want to see the full answer?

Chapter 14 Solutions

Interpretation:

The pH of a 0.10 M solution of boric acid has to be calculated.