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Chapter 14: Problem 20

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

Short Answer

Expert verified
Conditions a (\(\mathrm{pH}=3.04\)), b (\(\left[\mathrm{H}^{+}\right]>1.0 \times 10^{-7} M\)), and d (\(\left[\mathrm{OH}^{-}\right]=3.21 \times 10^{-12} M\)) indicate an acidic solution at 25掳C, while condition c (\(\mathrm{pOH}=4.51\)) does not.

Step by step solution

01

Check Condition a

For condition a, the given pH is 3.04. As pH < 7, it fulfills the criteria for an acidic solution and indicates an acidic environment.
02

Check Condition b

For condition b, the given H+ ion concentration is greater than 1.0 脳 10鈦烩伔 M. As the concentration of H+ ions is greater than 10鈦烩伔 M, it matches the criteria for an acidic solution and indicates an acidic environment.
03

Check Condition c

For condition c, the given pOH is 4.51. To determine if this condition indicates an acidic solution, we need to calculate the corresponding pH from the pOH using the relationship: pH + pOH = 14 at 25掳C. So the pH = 14 - pOH = 14 - 4.51 = 9.49. As the pH value is greater than 7, this condition does not indicate an acidic solution.
04

Check Condition d

For condition d, the given OH鈦� ion concentration is 3.21 脳 10鈦宦孤� M. To determine if this condition indicates an acidic solution, we need to calculate the corresponding pH. We will first find the pOH using the relationship: pOH = -log[OH鈦籡. Then, we will determine the pH using the relationship: pH + pOH = 14 at 25掳C. pOH = -log(3.21 脳 10鈦宦孤�) = 11.49 pH = 14 - 11.49 = 2.51 As the pH value is less than 7, this condition indicates an acidic environment. To summarize: Conditions a, b, and d indicate an acidic solution at 25掳C, while condition c does not.

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Most popular questions from this chapter

Is an aqueous solution of \(\mathrm{NaHSO}_{4}\) acidic, basic, or neutral? What reaction occurs with water? Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of \(\mathrm{NaHSO}_{4}\).

Calculate the \(\mathrm{pH}\) and \(\left[\mathrm{S}^{2-}\right]\) in a \(0.10 \mathrm{M} \mathrm{H}_{2} \mathrm{~S}\) solution. Assume \(K_{\mathrm{a}_{1}}=1.0 \times 10^{-7} ; K_{\mathrm{a}_{2}}=1.0 \times 10^{-19}\)

How would you prepare \(1600 \mathrm{~mL}\) of a \(\mathrm{pH}=1.50\) solution using concentrated \((12 M) \mathrm{HCl} ?\)

Arrange the following \(0.10 M\) solutions in order of most acidic to most basic. \(\mathrm{KOH}, \quad \mathrm{KNO}_{3}, \quad \mathrm{KCN}, \quad \mathrm{NH}_{4} \mathrm{Cl}, \mathrm{HCl}\).

A sample containing \(0.0500 \mathrm{~mol} \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) is dissolved in enough water to make \(1.00 \mathrm{~L}\) of solution. This solution contains hydrated \(\mathrm{SO}_{4}{ }^{2-}\) and \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}{ }^{3+}\) ions. The latter behaves as an acid: $$\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}^{2+}(a q)+\mathrm{H}^{+}(a q)$$ a. Calculate the expected osmotic pressure of this solution at \(25^{\circ} \mathrm{C}\) if the above dissociation is negligible. b. The actual osmotic pressure of the solution is \(6.73\) atm at \(25^{\circ} \mathrm{C}\). Calculate \(K_{\mathrm{a}}\) for the dissociation reaction of \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\). (To do this calculation, you must assume that none of the ions goes through the semipermeable membrane. Actually, this is not a great assumption for the tiny \(\mathrm{H}^{+}\) ion.)
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