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Chapter 14: Problem 167

Consider \(0.25 M\) solutions of the following salts: \(\mathrm{NaCl}\), \(\mathrm{RbOCl}, \mathrm{KI}, \mathrm{Ba}\left(\mathrm{ClO}_{4}\right)_{2}\), and \(\mathrm{NH}_{4} \mathrm{NO}_{3} .\) For each salt, indicate whether the solution is acidic, basic, or neutral.

Short Answer

Expert verified
In conclusion, the solutions of the given salts have the following properties: \(\mathrm{NaCl}\) (neutral), \(\mathrm{RbOCl}\) (basic), \(\mathrm{KI}\) (neutral), \(\mathrm{Ba}(\mathrm{ClO}_{4})_{2}\) (neutral), and \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) (acidic). This is based on whether each salt dissociates into strong or weak acids and bases in the solution.

Step by step solution

01

1. Analyze NaCl

NaCl is formed from the strong acid HCl and the strong base NaOH. When NaCl dissociates in water, it forms Na+ and Cl- ions. Since both the acid and base are strong, the solution will be neutral.
02

2. Analyze RbOCl

RbOCl is formed from the strong base RbOH and the weak acid HOCl. When RbOCl dissociates in water, it forms Rb+ and OCl- ions. Since the base is strong and the acid is weak, the solution will be basic.
03

3. Analyze KI

KI is formed from the strong acid HI and the strong base KOH. When KI dissociates in water, it forms K+ and I- ions. Since both the acid and base are strong, the solution will be neutral.
04

4. Analyze Ba(ClO4)2

Ba(ClO4)2 is formed from the strong acid HClO4 and the strong base Ba(OH)2. When Ba(ClO4)2 dissociates in water, it forms Ba2+ and 2 ClO4- ions. Since both the acid and base are strong, the solution will be neutral.
05

5. Analyze NH4NO3

NH4NO3 is formed from the weak base NH3 and the strong acid HNO3. When NH4NO3 dissociates in water, it forms NH4+ and NO3- ions. Since the base is weak and the acid is strong, the solution will be acidic. In conclusion, the solutions of NaCl, KI and Ba(ClO4)2 are neutral, the solution of RbOCl is basic and the solution of NH4NO3 is acidic.

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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 \(0.10-M\) solution of \(\mathrm{NaHSO}_{4}\).

Calculate the \(\mathrm{pH}\) of an aqueous solution containing \(1.0 \mathrm{X}\) \(10^{-2} M \mathrm{HCl}, 1.0 \times 10^{-2} M \mathrm{H}_{2} \mathrm{SO}_{4}\), and \(1.0 \times 10^{-2} M \mathrm{HCN}\).

Will \(0.10 M\) solutions of the following salts be acidic, basic, of neutral? See Appendix 5 for \(K_{\mathrm{a}}\) values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate

Making use of the assumptions we ordinarily make in calculating the \(\mathrm{pH}\) of an aqueous solution of a weak acid, calculate the \(\mathrm{pH}\) of a \(1.0 \times 10^{-6}-M\) solution of hypobromous acid (HBrO, \(K_{\mathrm{a}}=2 \times 10^{-9}\) ). What is wrong with your answer? Why is it wrong? Without trying to solve the problem, explain what has to be included to solve the problem correctly.

Trichloroacetic acid \(\left(\mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}\right)\) is a corrosive acid that is used to precipitate proteins. The \(\mathrm{pH}\) of a \(0.050-M\) solution of trichloroacetic acid is the same as the \(\mathrm{pH}\) of a \(0.040-\mathrm{M} \mathrm{HClO}_{4}\) solution. Calculate \(K_{\mathrm{a}}\) for trichloroacetic acid.
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