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Chapter 15: Problem 130

An aqueous solution has an OH concentration of \(1.0 \times 10^{-11} \mathrm{M}\). What is the \(\mathrm{H}_{3} \mathrm{O}\) concentration? Is this solution acidic or basic? Justify your answer

Short Answer

Expert verified
The H3O⁺ concentration is \(1.0 \times 10^{-3} M\), and the solution is acidic.

Step by step solution

01

Understand what is given

The OH⁻ concentration of the aqueous solution is given as \(1.0 \times 10^{-11} M\).
02

Apply the water ion product formula

The water ion product formula, \(K_w = [H_3O^+][OH^-]\), where \(K_w\) represents the ion product constant for water and has a value of \(1.0 \times 10^{-14}\) at 25°C, can be used to find the H3O⁺ concentration if the OH⁻ concentration is known.
03

Calculate the H3O⁺ concentration

To find the H3O⁺ concentration, we need to rearrange the water ion product formula and replace \(K_w\) with the given value: \[H_3O^+ =\frac{K_w}{OH^-}\] Plug in the values, \(K_w= 1.0 \times 10^{-14} \) and \(OH^- = 1.0 \times 10^{-11} M\): \(H_3O^+ =\frac{1.0 \times 10^{-14}}{1.0 \times 10^{-11}}\) \(H_3O^+ = 1.0 \times 10^{-3} M\)
04

Determine whether the solution is acidic or basic

To determine whether the solution is acidic or basic, we need to compare the H3O⁺ concentration with the neutral value. For a neutral solution, \(H_3O^+ = OH^-\), and the typical value is \(1.0 \times 10^{-7} M\). 1. If \(H_3O^+ > 1.0 \times 10^{-7} M\), the solution is acidic. 2. If \(H_3O^+ < 1.0 \times 10^{-7} M\), the solution is basic.
05

Justify the answer

In our case, the H3O⁺ concentration is \(1.0 \times 10^{-3} M\). As this value is greater than \(1.0 \times 10^{-7} M\), the solution is acidic. Final answer: The H3O⁺ concentration is \(1.0 \times 10^{-3} M\), and the solution is acidic.

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Most popular questions from this chapter

Knowing that aniline (Problem \(15.158\) ) is a weak base, is its conjugate acid a weak acid or a strong acid?

The pH of a solution is 8 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the OH concentration? (c) Is this solution acidic or basic?

Perchloric acid, \(\mathrm{HClO}_{4}\), is a strong acid. (a) Write the chemical equation for the reaction between perchloric acid and water. (b) List all species present in an aqueous solution of perchloric acid in order of concentration, highest to lowest. (c) Calculate the concentration of all species (except \(\mathrm{H}_{2} \mathrm{O}\) ) present in a \(0.100 \mathrm{M} \mathrm{HClO}_{4}\) solution. (d) What is the \(\mathrm{pH}\) of this solution?

Can a weak acid and its conjugate base ever have the same charge? Explain.

What is the \(\mathrm{OH}^{-}\) concentration of a solution that has a pH of \(9.66\) ? Is this solution acidic or basic?
See all solutions

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