Explanation a) 0.12 M in HCl Given information: As HCl is a strong acid, it gets completely dissociated when dissolved in water to form an aqueous solution. The reaction is, HCl ( a q ) + H 2 O ( l ) → H 3 O + ( a q ) + Cl − ( a q ) Since, there is complete dissociation of the acid, the hydronium ion concentration is equal to the quantity of acid dissolved. Thus, [ H 3 O + ] = 0.12 M Now, substitute this value in equation (1) to calculate the pH of the solution as: pH = − log [ 0 .12 ] = 0.92 The pH of the solution is 0.92 . b) 2.4 M in HNO 3 As HNO 3 is a strong acid, it gets completely dissociated when dissolved in water to form an aqueous solution. The reaction is, HNO 3 ( a q ) + H 2 O ( l ) → H 3 O + ( a q ) + NO 3 - ( a q ) Since, there is complete dissociation of the acid, the hydronium ion concentration is equal to the quantity of acid dissolved

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Author: Burdge

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Chapter 16, Problem 38QP

Interpretation Introduction

Interpretation:

The pH values of aqueous solutions are to be determined, when the concentrations of acids are given.

Concept introduction:

A strong acid is an electrolyte that completely dissociates, when dissolved in water, to produce hydronium ions and its conjugate base.

BOH(aq)→B+(aq)+OH−(aq)

pH is the measure of acidity of a solution and it depends on the concentration of hydronium ions and the temperature of the solution.

The formula to calculate the pH is:

pH=−log[H3O+] …… (1)

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Chapter 16, Problem 37QP

Chapter 16, Problem 39QP

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Chapter 16 Solutions

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Solution Summary: The author explains that the pH values of aqueous solutions are determined when the concentrations of acids are given.

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