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Chapter 13: Problem 17

Match the following pH values: \(1,2,5,6,6.5,8,11,11,\) and 13 with the following chemicals (of equal concentration): HBr, NaOH, NaF, NaCN, \(\mathrm{NH}_{4} \mathrm{F}, \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{F}, \mathrm{HF}, \mathrm{HCN},\) and \(\mathrm{NH}_{3} .\) Answer this question without performing calculations.

Short Answer

Expert verified
- HBr - pH 1 - \(\mathrm{HF}\) - pH 2 - \(\mathrm{HCN}\) - pH 5 - \(\mathrm{NH}_{4}\mathrm{F}\) - pH 6 - \(\mathrm{NH}_{3}\) - pH 6.5 - NaF - pH 8 - NaOH - pH 11 - \(\mathrm{CH}_{3}\mathrm{NH}_{3}\) - pH 11 - NaCN - pH 13

Step by step solution

01

Acids

HBr and \(\mathrm{HF}\) are strong acids and \(\mathrm{HCN}\) is a weak acid.
02

Bases

NaOH is a strong base, while \(\mathrm{NH}_{3}\) and \(\mathrm{CH}_{3}\mathrm{NH}_{3}\) are weak bases.
03

Salts

The salts in this exercise are NaF, NaCN, and \(\mathrm{NH}_{4}\mathrm{F}\). 2. Determine acidity or basicity based on pH values and then match each chemical:
04

pH 1 and 2

These pH values are very acidic. Based on the information above, we can match these with our strong acids: HBr and \(\mathrm{HF}\).
05

pH 5 and 6

These pH values are somewhat acidic. This implies that they are weak acids. In this case, we match pH 5 and 6 with the weak acid \(\mathrm{HCN}\) and \(\mathrm{NH}_{4}\mathrm{F}\), which is an acidic salt formed from a weak base and strong acid.
06

pH 6.5

This pH value is close to neutral. We can match this with the weak base \(\mathrm{NH}_{3}\), which has a pH slightly above neutral.
07

pH 8

This pH value is somewhat basic. We can match this with the basic salt NaF, which is formed from a weak acid and a strong base.
08

pH 11

These pH values are very basic. Based on the information above, we can match these with our strong base: NaOH, and the weak base \(\mathrm{CH}_{3}\mathrm{NH}_{3}\).
09

pH 13

This pH value is extremely basic. We can match this with the basic salt NaCN, which is formed from a very weak acid and a strong base. In conclusion: - HBr - pH 1 - \(\mathrm{HF}\) - pH 2 - \(\mathrm{HCN}\) - pH 5 - \(\mathrm{NH}_{4}\mathrm{F}\) - pH 6 - \(\mathrm{NH}_{3}\) - pH 6.5 - NaF - pH 8 - NaOH - pH 11 - \(\mathrm{CH}_{3}\mathrm{NH}_{3}\) - pH 11 - NaCN - pH 13

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Most popular questions from this chapter

Rank the following 0.10 \(M\) solutions in order of increasing pH. a. \(\mathrm{NH}_{3}\) b. KOH c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. KCl e. HCl

For propanoic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}, K_{\mathrm{a}}=1.3 \times 10^{-5}\right),\) determine the concentration of all species present, the \(\mathrm{pH}\), and the percent dissociation of a 0.100-M solution.

Place the species in each of the following groups in order of increasing acid strength. Explain the order you chose for each group. a. \(\mathrm{HIO}_{3}, \mathrm{HBrO}_{3}\) b. \(\mathrm{HNO}_{2}, \mathrm{HNO}_{3}\) c. HOCI, HOI d. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{PO}_{3}\)

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. \(\mathrm{NH}_{3}, \mathrm{HONH}_{2}\)

Calculate the \(\mathrm{pH}\) of a \(0.200-M\) solution of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\). Hint: \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\) is a salt composed of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}\) and \(\mathrm{F}^{-}\) ions. The principal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is $$\begin{aligned} \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(a q)+\mathrm{F}^{-}(a q) & \rightleftharpoons \\ \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(a q) &+\mathrm{HF}(a q) \quad K=8.2 \times 10^{-3}\end{aligned}$$
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