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Chapter 16: Problem 21

The pOH of a solution is \(9.40 .\) Calculate the hydrogen ion concentration of the solution.

Short Answer

Expert verified
The concentration of hydrogen ions (\([H^+]\)) in the solution is \(10^{-4.6}\) M.

Step by step solution

01

Calculate the Hydroxide Ion Concentration

pOH is calculated by the formula, pOH = \( -\log[OH^-] \). Therefore, the hydroxide ion concentration can be calculated by rearranging this formula as, \([OH^-] = 10^{-pOH}\). Given that the pOH of the solution is 9.40, the concentration of OH- ions becomes \([OH^-] = 10^{-9.40}\).
02

Calculate the Hydrogen Ion Concentration

Next, the hydrogen ion concentration can be calculated using the ion product of water (\(K_w\)), which is given as \(K_w = [H+][OH^-]\). By substituting our calculated \([OH^-]\) into this formula, the hydrogen ion concentration can be found: \([H+] = \frac{K_w}{[OH^-]}\) = \(\frac{1.0 \times 10^{-14}}{10^{-9.40}}\).

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Most popular questions from this chapter

To which of the following would the addition of an equal volume of \(0.60 \mathrm{M} \mathrm{NaOH}\) lead to a solution having a lower \(\mathrm{pH} ?\) (a) water, (b) \(0.30 \mathrm{M} \mathrm{HCl}\), (c) \(0.70 \mathrm{M} \mathrm{KOH}\) (d) \(0.40 \mathrm{M} \mathrm{NaNO}_{3}\).

What are the concentrations of \(\mathrm{HSO}_{4}^{-}, \mathrm{SO}_{4}^{2-},\) and \(\mathrm{H}^{+}\) in a \(0.20 \mathrm{M} \mathrm{KHSO}_{4}\) solution? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid: \(K_{\mathrm{a}}\) for \(\left.\mathrm{HSO}_{4}^{-}=1.3 \times 10^{-2} .\right)\)

What are the Lewis definitions of an acid and a base? In what way are they more general than the Bronsted definitions?

A certain salt, MX (containing the \(\mathrm{M}^{+}\) and \(\mathrm{X}^{-}\) ions), is dissolved in water, and the \(\mathrm{pH}\) of the resulting solution is 7.0. Can you say anything about the strengths of the acid and the base from which the salt is derived?

Calculate the hydrogen ion concentration for solutions (a) 2.42 with these \(\mathrm{pH}\) values: (b) 11.21 (c) 6.96 , (d) 15.00 .
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