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Chapter 17: Problem 108

The most acidic of the following \(0.10 \mathrm{M}\) salt solutions is (a) \(\mathrm{Na}_{2} \mathrm{S} ;\) (b) \(\mathrm{NaHSO}_{4} ;\) (c) \(\mathrm{NaHCO}_{3} ;\) (d) \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\)

Short Answer

Expert verified
The most acidic 0.10 M salt solution among the given solutions is \(\mathrm{NaHSO}_{4}\) because \(\mathrm{HSO}_{4}^{-}\), the anion present in this salt, has the parent acid \(\mathrm{H}_{2}\mathrm{SO}_{4}\), which is the strongest compared to the parent acids of the anions in other salts.

Step by step solution

01

Identify the Anions and Their Parent Acids

Firstly, identify the anions in each salt and their parent acids: In (a) \(\mathrm{Na}_{2} \mathrm{S}\), the anion is \(\mathrm{S}^{^{2-}}\) and the parent acid is \(\mathrm{H}_{2} \mathrm{S}\). In (b) \(\mathrm{NaHSO}_{4}\), the anion is \(\mathrm{HSO}_{4}^-\) and the parent acid is \(\mathrm{H}_{2}\mathrm{SO}_{4}\). In (c) \(\mathrm{NaHCO}_{3}\), the anion is \(\mathrm{HCO}_{3}^-\) and the parent acid is \(\mathrm{H}_{2}\mathrm{CO}_{3}\). In (d) \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\), the anion is \(\mathrm{HPO}_{4}^{^{2-}}\) and the parent acid is \(\mathrm{H}_{2}\mathrm{PO}_{4}\).
02

Determine the Strength of the Parent Acids

Now, the more acidic a solution, the lower its pH value. Therefore, the strength of the parent acid of each anion will determine how acidic the salt solution is: \(\mathrm{H}_{2}\mathrm{S}\) is a weak acid; \(\mathrm{H}_{2}\mathrm{SO}_{4}\) is a strong acid; \(\mathrm{H}_{2}\mathrm{CO}_{3}\) is a weak acid; and \(\mathrm{H}_{2}\mathrm{PO}_{4}\) is a moderate acid.
03

Find the Most Acidic Solution

Since the most acidic solution will be the one whose anion's parent acid is the strongest, and given that \(\mathrm{H}_{2}\mathrm{SO}_{4}\) is the strongest among the identified parent acids, then the solution \(\mathrm{NaHSO}_{4}\), where \(\mathrm{HSO}_{4}^{-}\) is the anion, will be the most acidic.

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Most popular questions from this chapter

Using appropriate equilibrium constants but without doing detailed calculations, determine whether a solution can be simultaneously: (a) \(0.10 \mathrm{M} \mathrm{NH}_{3}\) and \(0.10 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl},\) with \(\mathrm{pH}=6.07\) (b) \(0.10 \mathrm{M} \mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(0.058 \mathrm{M} \mathrm{HI}\) (c) \(0.10 \mathrm{M} \mathrm{KNO}_{2}\) and \(0.25 \mathrm{M} \mathrm{KNO}_{3}\) (d) \(0.050 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) and \(0.65 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) (e) \(0.018 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) and \(0.018 \mathrm{M} \mathrm{NaC}_{6} \mathrm{H}_{5} \mathrm{COO}\) with \(\mathrm{pH}=4.20\) (f) \(0.68 \mathrm{M} \mathrm{KCl}, 0.42 \mathrm{M} \mathrm{KNO}_{3}, 1.2 \mathrm{M} \mathrm{NaCl},\) and \(0.55 \mathrm{M}\) \(\mathrm{NaCH}_{3} \mathrm{COO},\) with \(\mathrm{pH}=6.4\)

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Thymol blue indicator has \(t w o\) pH ranges. It changes color from red to yellow in the pH range from 1.2 to 2.8, and from yellow to blue in the pH range from 8.0 to 9.6. What is the color of the indicator in each of the following situations? (a) The indicator is placed in \(350.0 \mathrm{mL}\) of \(0.205 \mathrm{M} \mathrm{HCl}\) (b) To the solution in part (a) is added \(250.0 \mathrm{mL}\) of \(0.500 \mathrm{M} \mathrm{NaNO}_{2}\) (c) To the solution in part (b) is added \(150.0 \mathrm{mL}\) of \(0.100 \mathrm{M} \mathrm{NaOH}\) (d) To the solution in part (c) is added \(5.00 \mathrm{g} \mathrm{Ba}(\mathrm{OH})_{2}\)

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Consider a solution containing two weak monoprotic acids with dissociation constants \(K_{\mathrm{HA}}\) and \(K_{\mathrm{HB}}\). Find the charge balance equation for this system, and use it to derive an expression that gives the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) as a function of the concentrations of \(\mathrm{HA}\) and HB and the various constants.
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