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Chapter 15: Problem 63

What is the hydroxide ion concentration in a solution of \(\mathrm{pH} 8.72 ?\)

Short Answer

Expert verified
The hydroxide ion concentration in a solution of pH 8.72 is approximately \(5.24 \times 10^{-6} M\).

Step by step solution

01

Convert pH to pOH

Using the relationship \(pH + pOH = 14\), the pOH can be calculated as \(pOH = 14 - pH\). Substituting the given pH value of 8.72, we find: \(pOH = 14 - 8.72 = 5.28\).
02

Calculate hydroxide ion concentration

The pOH represents the negative logarithm (base 10) of the hydroxide ion concentration. Therefore, to find the hydroxide ion concentration, the inverse of the logarithm function, known as the exponentiation function, is used. The hydroxide ion concentration will be \(10^{-pOH}\). Substituting the calculated pOH value, the hydroxide ion concentration becomes: \(10^{-5.28}\).

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Most popular questions from this chapter

Find the \(\mathrm{pH}\) of a solution prepared by dissolving 0.65 \(\mathrm{mol}\) of the strong base \(\mathrm{NaOH}\) in 1.0 \(\mathrm{L}\) of water.

Why does an indicator need to be a weak acid or a weak base?

If 35.40 \(\mathrm{mL}\) of 1.000 \(\mathrm{M} \mathrm{HCl}\) is neutralized by 67.30 mL of NaOH, what is the molarity of the NaOH solution?

Describe two methods of measuring pH, and explain the advantages and disadvantages of each method.

Place the following acids in order of increasing strength: \begin{equation} \begin{array}{l}{\text { a. valeric acid, } K_{a}=1.5 \times 10^{-5}} \\\ {\text { b. glutaric acid, } K_{a}=3.4 \times 10^{-4}} \\ {\text { c. hypoobromous acid, } K_{a}=2.5 \times 10^{-9}} \\ {\text { d. acetylsalicylic acid (aspirin), }} \\ {K_{a}=3.3 \times 10^{-4}}\end{array} \end{equation}
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