Chapter 16.2, Problem 16.1CYU

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

What are the hydronium ion and hydroxide ion concentrations in 4.0 × 10−3 M HCI(aq) at 25 °C? (Recall that because HCl is a strong acid, it is 100% ionized in water.)

Interpretation Introduction

Interpretation:

The hydronium ion and hydroxide ion concentration in 4×103MHCl(aq) at 25°C has to be calculated.

Concept introduction:

In pure water, equilibrium exists between water and the hydronium and hydroxide ions.

2H2O(l)H3O+(aq)+OH(aq)

The Equilibrium constant (Kw) expression for auto ionization of pure water is:

Kw=[H3O+][OH]                                                                                                   (1)

The value of equilibrium constant is temperature dependent. The ionization constant for pure water is:

Kw=1×1014 at 25°C.

Explanation

HCl is a strong acid. It is 100â€‰% dissociated into ions in water. The H+ ion concentration is same as the initial concentration of HCl. The H+ ion concentration is calculated below.

Given:

The concentration of HCl in aqueous solution is 4Ã—10âˆ’3â€‰M.

The ionization of HCl in water is given below:

â€‚Â HCl(aq)â‡ŒH+(aq)+OHâˆ’(aq)

The initial concentration of H+ ion is 4Ã—10âˆ’3â€‰M. The concentration of H+ ion produced by autoionization of water is 1Ã—10âˆ’7â€‰M. If x is equal to the concentration of hydronium ion produced by autoionization of water. The total concentration of hydronium ion in aqueous solution is (0

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