   # A 2.50 g sample of a solid that could be Ba(OH) 2 or Sr(OH) 2 was dissolved in enough water to make 1.00L of solution. If the pH of the solution is 12.61, what is the identity of the solid? ### 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, Problem 85GQ
Textbook Problem
148 views

## A 2.50 g sample of a solid that could be Ba(OH)2 or Sr(OH)2 was dissolved in enough water to make 1.00L of solution. If the pH of the solution is 12.61, what is the identity of the solid?

Interpretation Introduction

Interpretation:

The identity of the solid has to be determined when the 2.50 g sample of a solid that could be Ba(OH)2 or Sr(OH)2 was dissolved in enough water to make 1.00L of solution. If the pH of the solution is 12.61.

Concept introduction:

The concentration of compound can be calculated by using the following formula.

Concentration = Mass of given compoundMolar mass of given compound × 1Volume in Litres

### Explanation of Solution

Let’s calculate the hydroxide ion concentration by using pH value.

Given pH =12.61

pH  =  - log[H3O+]12.61 =-log[H3O+][H3O+]=10-12.61[H3O+]=2.455×10-13MAt 250CKW=[H3O+][OH-]=1.0×10-141.0×10-14=(2.45×10-13)[OH-][OH-]=4.1×10-2M

Therefore, hydroxide ion concentration is 4.1×10-2M

Assumed the solid to be Ba(OH)2

The dissociation of Ba(OH)2 is as follows.

Ba(OH)2Ba2++2OH-

Let’s calculate the concentration of Ba(OH)2

Given mass of solid = 2.50g

Molar mass of Ba(OH)2=171.327g/mol

Volume = 1L

Concentration of Ba(OH)2=Mass of Ba(OH)2Molar mass of Ba(OH)2×1V2

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