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Chapter 15: Problem 202

The molar concentration of concentrated hydrochloric acid is \(12.1 \mathrm{M}\). What are the \(\mathrm{pH}\) and \(\mathrm{OH}^{-}\) ion molar concentration?

Short Answer

Expert verified
The pH of the concentrated hydrochloric acid is about -1.08, and the OH⁻ ion molar concentration is approximately \(8.26 \times 10^{-16} M\).

Step by step solution

01

Understanding the Dissociation of Hydrochloric Acid

Hydrochloric acid is a strong acid, meaning it completely dissociates in water. When it does so, it releases a hydrogen ion (H+) and a chloride ion (Cl-). This can be represented as: HCl → H+ + Cl-. The molar concentration of HCl is given as 12.1 M, implying that the molar concentration of H+ ions will also be 12.1 M.
02

Calculate the pH of the Solution

From step 1, it's known that the concentration of H+ ions is 12.1 M. The pH of a solution is the negative logarithm of the H+ ion concentration: pH = -log[H+]. By substituting [H+] = 12.1 M into the pH equation, one gets the pH of the solution.
03

Calculate the OH- ion Concentration

The water ion product Kw is equal to [H+][OH-] = \(1.0 \times 10^{-14}\) at 25 ºC. In order to find the OH- ion concentration, one can rearrange the water ion product equation to get [OH-] = Kw / [H+]. Substitute [H+] = 12.1 M from Step 1 and Kw = \(1.0 \times 10^{-14}\) into the equation. This will enable the conclusion of the OH- ion molar concentration.

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Most popular questions from this chapter

Are a \(1 \mathrm{M}\) solution of ammonia, \(\mathrm{NH}_{3}\), and a \(1 \mathrm{M}\) solution of lithium hydroxide, I iOH, equally basic, or is one solution more basic than the other? Explain.

An ionic compound with the formula \(\operatorname{NaX}(\mathrm{X}\) is an unknown anion) is dissolved in water, and the resulting solution is basic. Is HX a strong acid or a weak acid? Explain.

Based solely on concentrations, when is an aqueous solution judged to be basic? Give two answers to this question.

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?
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