Table of contents

17. Acid and Base Equilibrium

pH of Strong Acids and Bases

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

What is the pH of a neutral solution at a temperature where Kw = 1.8 × 10^-14?

7.1

6.8

7.0

6.9

Verified step by step guidance

Understand that the pH of a neutral solution is determined by the concentration of hydrogen ions [H⁺] and hydroxide ions [OH⁻] being equal.

Recall that the ion product of water (Kw) is the product of the concentrations of [H⁺] and [OH⁻], given by the equation:

K w = [H

⁺][OH^-].

Given that Kw = 1.8 × 10^-14, set up the equation for a neutral solution where [H⁺] = [OH⁻], so

[H

⁺]^2 = 1.8 imes 10^{-14}.

Solve for [H⁺] by taking the square root of both sides:

[H

⁺] = ext{sqrt}(1.8 imes 10^{-14}).

Calculate the pH using the formula:

pH = -	ext{log}_{10}([H

⁺]).

Master pH of Strong Acids and Bases with a bite sized video explanation from Jules

Problem sets built by lead tutors

Expert video explanations