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Chapter 14: Problem 22

Which of the following conditions indicate an acidic solution at $25^{\circ} \mathrm{C} ?$ a. \(\mathrm{pH}=3.04\) b. \(\left[\mathrm{H}^{+}\right]>1.0 \times 10^{-7} \mathrm{M}\) c. \(\mathrm{pOH}=4.51\) d. \(\left[\mathrm{OH}^{-}\right]=3.21 \times 10^{-12} \mathrm{M}\)

Short Answer

Expert verified
Conditions (a), (b), and (d) indicate an acidic solution at \(25^{\circ} \mathrm{C}\). Condition (a) has pH = 3.04 which is less than 7. Condition (b) has [\(\mathrm{H}^{+}\)] > \(1.0 \times 10^{-7} \mathrm{M}\), higher than pure water. Condition (d) has [\(\mathrm{OH}^{-}\)] = \(3.21 \times 10^{-12} \mathrm{M}\), lesser than the concentration in pure water, indicating a higher concentration of \(\mathrm{H}^{+}\) ions.

Step by step solution

01

Analyzing the first condition (pH = 3.04)

As an acidic solution has a pH less than 7, we can see that the given pH = 3.04 is lesser than 7, which indicates an acidic solution. So, condition (a) is true.
02

Analyzing the second condition ([\(\mathrm{H}^{+}\)] > \(1.0 \times 10^{-7} \mathrm{M}\))

In pure water at \(25^{\circ}\mathrm{C}\), the concentration of \(\mathrm{H}^{+}\) ions is \(1.0 \times 10^{-7} \mathrm{M}\). Since an acidic solution has a higher concentration of \(\mathrm{H}^{+}\) ions than pure water, this condition indicates an acidic solution. So, condition (b) is true.
03

Analyzing the third condition (pOH = 4.51)

An acidic solution is characterized by a pOH greater than 7. The given pOH = 4.51, which is less than 7. This condition does not indicate an acidic solution. So, condition (c) is false.
04

Analyzing the fourth condition ([\(\mathrm{OH}^{-}\)] = \(3.21 \times 10^{-12} \mathrm{M}\))

An acidic solution is characterized by a higher concentration of \(\mathrm{H}^{+}\) ions than \(\mathrm{OH}^{-}\) ions. In pure water at \(25^{\circ}\mathrm{C}\), the concentration of \(\mathrm{OH}^{-}\) ions is also \(1.0 \times 10^{-7} \mathrm{M}\). Since the given \(\mathrm{OH}^{-}\) concentration is \(3.21 \times 10^{-12} \mathrm{M}\) which is lesser than the concentration in pure water, this condition indicates an acidic solution as the concentration of \(\mathrm{H}^{+}\) ions must be higher. So, condition (d) is true. Answer: Conditions (a), (b), and (d) indicate an acidic solution at \(25^{\circ}\mathrm{C}.\)

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Most popular questions from this chapter

A \(0.100-\mathrm{g}\) sample of the weak acid \(\mathrm{HA}\) (molar mass \(=\) 100.0 \(\mathrm{g} / \mathrm{mol} )\) is dissolved in 500.0 \(\mathrm{g}\) water. The freezing point of the resulting solution is \(-0.0056^{\circ} \mathrm{C}\) . Calculate the value of \(K_{\mathrm{a}}\) for this acid. Assume molality equals molarity in this solution.

The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: $$ \mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) $$ Acids formed during normal cellular respiration react with the \(\mathrm{HCO}_{3}^{-}\) to form carbonic acid, which is in equilibrium with \(\mathrm{CO}_{2}(a q)\) and \(\mathrm{H}_{2} \mathrm{O}(l) .\) During vigorous exercise, a person's \(\mathrm{H}_{2} \mathrm{CO}_{3}\) blood levels were $26.3 \mathrm{mM},\( whereas his \)\mathrm{CO}_{2}\( levels were 1.63 \)\mathrm{mM}$ . On resting, the \(\mathrm{H}_{2} \mathrm{CO}_{3}\) levels declined to 24.9 \(\mathrm{m} M\) . What was the \(\mathrm{CO}_{2}\) blood level at rest?

A typical sample of vinegar has a pH of \(3.0 .\) Assuming that vinegar is only an aqueous solution of acetic acid \(\left(K_{\mathrm{a}}=1.8 \times\right.\) \(10^{-5}\) ), calculate the concentration of acetic acid in vinegar.

Quinine $\left(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{2}\right)$ is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, $\mathrm{p} K_{\mathrm{b}_{1}}=5.1\( and \)\mathrm{p} K_{\mathrm{b}_{2}}=9.7\left(\mathrm{p} K_{\mathrm{b}}=-\log K_{\mathrm{b}}\right) .$ Only 1 g quinine will dissolve in 1900.0 \(\mathrm{mL}\) of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction $\mathrm{Q}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{QH}^{+}+\mathrm{OH}^{-}$ described by \(\mathrm{p} K_{\mathrm{b}_{1}},\) where \(\mathrm{Q}=\) quinine.

Using your results from Exercise \(133,\) place the species in each of the following groups in order of increasing base strength. a. \(\mathrm{OH}^{-}, \mathrm{SH}^{-}, \mathrm{SeH}^{-}\) b. \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\) c. \(\mathrm{NH}_{3}, \mathrm{HONH}_{2}\)
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