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Chapter 16: Problem 84

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) \(\mathrm{AlCl}_{3}\), (b) \(\mathrm{NaBr}\), (c) \(\mathrm{NaClO},(\mathrm{d})\) \(\left[\mathrm{CH}_{3} \mathrm{NH}_{3}\right] \mathrm{NO}_{3},(\mathrm{e}) \mathrm{Na}_{2} \mathrm{SO}_{3}\)

Short Answer

Expert verified
The aqueous solutions of the given substances have the following pH nature: (a) \(\mathrm{AlCl}_{3}\) - acidic, (b) \(\mathrm{NaBr}\) - neutral, (c) \(\mathrm{NaClO}\) - basic, (d) \(\left[\mathrm{CH}_{3} \mathrm{NH}_{3}\right] \mathrm{NO}_{3}\) - acidic, and (e) \(\mathrm{Na}_{2} \mathrm{SO}_{3}\) - basic.

Step by step solution

01

Analyzing AlCl3

When \(\mathrm{AlCl}_{3}\) is dissolved in water, it forms \(\mathrm{Al}^{3+}\) and \(\mathrm{Cl}^{-}\) ions. The \(\mathrm{Al}^{3+}\) ion can undergo hydrolysis to generate \(\mathrm{H}^{+}\) ions in the solution, which makes the solution acidic. Thus, an aqueous solution of \(\mathrm{AlCl}_{3}\) is acidic. #b)
02

Analyzing NaBr

When \(\mathrm{NaBr}\) is dissolved in water, it forms \(\mathrm{Na}^{+}\) and \(\mathrm{Br}^{-}\) ions. Neither of these ions undergoes hydrolysis in water, so no \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions are produced. As a result, an aqueous solution of \(\mathrm{NaBr}\) is neutral. #c)
03

Analyzing NaClO

When \(\mathrm{NaClO}\) is dissolved in water, it forms \(\mathrm{Na}^{+}\) and \(\mathrm{ClO}^{-}\) ions. The \(\mathrm{ClO}^{-}\) ion can react with water to generate \(\mathrm{OH}^{-}\) ions, making the solution basic. Thus, an aqueous solution of \(\mathrm{NaClO}\) is basic. #d)
04

Analyzing [CH3NH3]NO3

When \(\left[\mathrm{CH}_{3} \mathrm{NH}_{3}\right] \mathrm{NO}_{3}\) is dissolved in water, it forms \(\mathrm{CH}_{3}\mathrm{NH}_{3}^+\) and \(\mathrm{NO}_{3}^-\) ions. The \(\mathrm{CH}_{3}\mathrm{NH}_{3}^{+}\) ion can release \(\mathrm{H}^{+}\) ions in the solution, making the solution acidic. Therefore, an aqueous solution of \(\left[\mathrm{CH}_{3} \mathrm{NH}_{3}\right] \mathrm{NO}_{3}\) is acidic. #e)
05

Analyzing Na2SO3

When \(\mathrm{Na}_{2} \mathrm{SO}_{3}\) is dissolved in water, it forms \(\mathrm{Na}^{+}\) and \(\mathrm{SO}_{3}^{2-}\) ions. The \(\mathrm{SO}_{3}^{2-}\) ion can undergo hydrolysis to generate \(\mathrm{OH}^{-}\) ions, making the solution basic. Thus, an aqueous solution of \(\mathrm{Na}_{2} \mathrm{SO}_{3}\) is basic.

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Most popular questions from this chapter

The odor of fish is due primarily to amines, especially methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\). Fish is often served with a wedge of lemon, which contains citric acid. The amine and the acid react forming a product with no odor, thereby making the lessthan-fresh fish more appetizing. Using data from Appendix \(D\), calculate the equilibrium constant for the reaction of citric acid with methylamine, if only the first proton of the citric acid \(\left(K_{a 1}\right)\) is important in the neutralization reaction.

Determine the \(\mathrm{pH}\) of each of the following solutions \(\left(K_{a}\right.\) and \(K_{b}\) values are given in Appendix \(D\) ): (a) \(0.095 M\) hypochlorous acid, (b) \(0.0085 \mathrm{M}\) hydrazine, (c) \(0.165 \mathrm{M}\) hydroxylamine.

A \(0.100 M\) solution of bromoacetic acid \(\left(\mathrm{BrCH}_{2} \mathrm{COOH}\right)\) is \(13.2 \%\) ionized. Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{BrCH}_{2} \mathrm{COO}^{-}\right],\left[\mathrm{BrCH}_{2} \mathrm{COOH}\right]\) and \(K_{a}\) for bromoacetic acid.

Lactic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\right)\) has one acidic hydrogen. A \(0.10 \mathrm{M}\) solution of lactic acid has a \(\mathrm{pH}\) of \(2.44 .\) Calculate \(K_{a}\)

(a) Give the conjugate base of the following Bronsted-Lowry acids: (i) \(\mathrm{HCOOH},\) (ii) \(\mathrm{HPO}_{4}^{2-}\). (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{SO}_{4}^{2-}\), (ii) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\)
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