Chapter 14, Problem 104E

### Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

Chapter
Section

### Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

# Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution having a pH of 10.00 (Kb = 1.1 × 10–8).

Interpretation Introduction

Interpretation: The mass of HONH2 has to be calculated.

Concept Introduction:

The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

Explanation

To determine: The mass of HONH2 required to dissolve in enough water to make 250.0mL of the solution having a pH of 10.00 .

The given pH value is 10.00 .

The sum, pH+pOH=14

Substitute the value of pH in the above expression.

pOH+10.00=14pOH=4.0_

The pOH value is 4.0_ .

The pOH of a solution is calculated by the formula,

pOH=log[OH]

Rearrange the above expression to calculate the value of [OH] .

[OH]=10pOH

Substitute the calculated value of pH in the above expression.

[OH]=104.0=1.0×10-4M_

The [OH] is 1.0×10-4M_ .

The [OH] for the weak bases is calculated by the formula

[OH]=Kb×C

Where,

C is the concentration of the weak base involved.

Substitute the value of [OH] and Kb for HONH2 in the above expression.

[1×104]=(1.1×108)2×CC=(0.0001)21.1×108=0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started