   Chapter 14, Problem 171CP

Chapter
Section
Textbook Problem

# Calculate the pH of a 1.0 × 10−7-M solution of NaOH in water.

Interpretation Introduction

Interpretation: The concentration of NaOH solution in water is given. By using this value, the pH value of NaOH in water is to be calculated.

Concept introduction: The pH value is the measure of H+ ions. The pH is calculated using the formula,

pH=log10[H+]

Explanation

Explanation

To determine: The pH value of NaOH solution in water.

The concentration of H+ ion is 6.18×108M_ .

Given

The concentration of OH from NaOH is 1.0×107M .

The pH can be calculated by considering the relationship between the molarities of three principle ion solution Na+,H2O and OH .

The autoionization of water involves formation of hydroxide ion and H+ ion due to transfer of a proton from one water molecule to another.

The reaction of ionization of water is,

H2O(l)H+(aq)+OH(aq)

It is assumed that the change in concentration of [H+] is x .

Make the ICE table for the above reaction.

H2O(l)H+(aq)OH(aq)Initial:01.0×107Chang:xxEquilibrium:x1.0×107+x

The ion product constant for water is given as,

Kw=[H+][OH]

Where,

• Kw is ion product constant of water (1

### 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

#### Find more solutions based on key concepts 