Explanation The addition of ammonium iodide to water results into an acidic solution. The reaction is given below. N H 4 + ( a q ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + N H 3 ( a q ) The acid ionization constant for the above equation can be written as given below. K a = [ H 3 O + ] [ N H 3 ] [ N H 4 + ] The concentration of H 3 O + can be calculated from the p H as given below. p H = − log [ H 3 O + ] ⇒ [ H 3 O + ] = 10 − p H = 10 − 5.50 = 3.2 × 10 − 6 . A table can be set up as given below. N H 4 + ( a q ) H 3 O + ( a q ) N H 3 ( a q ) I n i t i a l c o n c . ( M ) − 1.0 × 10 − 7 0 C h a n g e i n c o n c . ( M ) − 3.2 × 10 − 6 + 3.2 × 10 − 6 + 3

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ISBN: 9781285199047

Author: John W. Moore, Conrad L. Stanitski

Publisher: Cengage Learning

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Chapter 14, Problem 99QRT

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The concentration of ammonium iodide of aqueous ammonium iodide solution having pH of 5.50 has to be calculated.

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Chapter 14, Problem 98QRT

Chapter 14, Problem 100QRT

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The concentration of ammonium iodide of aqueous ammonium iodide solution having p H of 5.50 has to be calculated.

Solution Summary: The author explains how the concentration of ammonium iodide in aqueous solution with pH of 5.50 can be calculated.

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Interpretation:

The concentration of ammonium iodide of aqueous ammonium iodide solution having pH of 5.50 has to be calculated.

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Chapter 14 Solutions

The concentration of ammonium iodide of aqueous ammonium iodide solution having p H of 5.50 has to be calculated.

Solution Summary: The author explains how the concentration of ammonium iodide in aqueous solution with pH of 5.50 can be calculated.

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Interpretation: The concentration of ammonium iodide of aqueous ammonium iodide solution having pH of 5.50 has to be calculated.

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Chapter 14 Solutions

Interpretation:

The concentration of ammonium iodide of aqueous ammonium iodide solution having pH of 5.50 has to be calculated.