   Chapter 14, Problem 170CP

Chapter
Section
Textbook Problem

# The pH of 1.0 × 10−8 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering the relationship between the molarities of the three principal ions in the solution (H+, Cl−, and OH−). These molarities can be calculated from algebraic equations that can be derived from the considerations given below.a. The solution is electrically neutral.b. The hydrochloric acid can be assumed to be 100% ionized.c. The product of the molarities of the hydronium ions and the hydroxide ions must equal Kw.Calculate the pH of a 1.0 × 10−8-M HCl solution.

Interpretation Introduction

Interpretation: The concentration of hydrochloric acid and the method to calculate the molarities of three principal ions is given. The pH value of HCl 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 HCl solution.

The concentration of H+ ion is 1.1×107M_ .

Given

The concentration of HCl is 1.0×108M .

It is given that pH can be calculated by considering the relationship between the molarities of three principle ion solution H+,Cl 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 ionization product of autoionization of water is,

Kw=[H+][OH]

Where,

• Kw is ion product constant.

In the given solution, the amount of HCl will be equal to amount of H+ ion (1.0×107) in water. Therefore, concentration of H+ ion is,

(1

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