   # If the pH of a solution containing the strong base Sr(OH) 2 is 10.46 at 25°C, what is the concentration of Sr(OH) 2 ? (a) 3.5 × 10 −11 M (b) 2.9 × 10 −4 M (c) 6.9 × 10 −4 M (d) 1.4 × 10 −4 M ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 16.2, Problem 3RC
Textbook Problem
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## If the pH of a solution containing the strong base Sr(OH)2 is 10.46 at 25°C, what is the concentration of Sr(OH)2? (a) 3.5 × 10−11 M (b) 2.9 × 10−4 M (c) 6.9 × 10−4 M (d) 1.4 × 10−4 M

Interpretation Introduction

Interpretation:

The Sr(OH)2 pH rang was given in the satement at 250C, than Sr(OH)2 concentration should calculated at same temprature.

Concept introduction:

A strong acid completely dissociates into its constituent ions in aqueous solution, as a result, the concentration of its ion is same as the initial concentration of that strong acid.

For example, strong acid dissociates as follows in water,

HA(aq)+H2O(l)H3O+(aq)+A(aq)

[H3O+]=[A]=[HA]

The pH of a solution is basically the measure of the molar concentration of the H+ or H3O+ ion in the solution. More the concentration of H+ or H3O+ ion in the solution, lesser will be the pH value and more acidic will be the solution.

The expression for pH is given as,

pH=log[H3O+]

The concentration of OH ions is calculated by using the ionic product of water.

Kw=[H3O+][OH]

The value of Kw is 1.0×1014 .

If pH<7 then, the solution is acidic in nature.

If pH<7 then, the solution is basic in nature.

If pH<7 then, the solution is neutral in nature.

### Explanation of Solution

The Sr(OH)2 concentration has calculated below.

Given

The pH range of Sr(OH)2 10.46 at 250C

pOH=14.00pHGivenpHrange10.46at250CpOH=14.0010.46pOH=3.54pOH=log[OH][OH]=103.54=2.88×104MTheequationrespestingthedessociationSr(OH)

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