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Chapter 15: Problem 78

Predict whether the following solutions are acidic, basic, or nearly neutral: (a) \(\mathrm{NaBr}\), (b) \(\mathrm{K}_{2} \mathrm{SO}_{3}\) (c) \(\mathrm{NH}_{4} \mathrm{NO}_{2}\), (d) \(\operatorname{Cr}\left(\mathrm{NO}_{3}\right)_{3}\).

Short Answer

Expert verified
(a) NaBr forms a neutral solution. (b) K2SO3 forms a basic solution. (c) NH4NO2 forms an acidic solution. (d) Cr(NO3)3 forms an acidic solution.

Step by step solution

01

Analyze NaBr

Sodium bromide, NaBr, is the salt of a strong base (NaOH) and a strong acid (HBr), therefore the solution of NaBr is neutral.
02

Analyze K2SO3

Potassium Sulfite, K2SO3, is the salt of a strong base (KOH) and a weak acid (H2SO3). This means the solution will be basic.
03

Analyze NH4NO2

Ammonium nitrite, NH4NO2, is derived from a weak base (NH3) and a strong acid (HNO2). Hence, the solution will be acidic.
04

Analyze Cr(NO3) 3

Chromium(III) nitrate, Cr(NO3)3, is the salt of a weak base (Cr(OH)3) and a strong acid (HNO3). Hence the solution will be acidic.

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Most popular questions from this chapter

Fill in the word acidic, basic, or neutral for the following solutions: (a) \(\mathrm{pOH}>7 ;\) solution is (b) \(\mathrm{pOH}=7 ;\) solution is (c) \(\mathrm{pOH}<7\); solution is

When chlorine reacts with water, the resulting solution is weakly acidic and reacts with AgNO \(_{3}\) to give a white precipitate. Write balanced equations to represent these reactions. Explain why manufacturers of household bleaches add bases such as \(\mathrm{NaOH}\) to their products to increase their effectiveness.

A certain salt, MX (containing the \(\mathrm{M}^{+}\) and \(\mathrm{X}^{-}\) ions), is dissolved in water, and the \(\mathrm{pH}\) of the resulting solution is \(7.0 .\) Can you say anything about the strengths of the acid and the base from which the salt is derived?

Compare the strengths of the following pairs of acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SeO}_{4}\), (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\).

To which of the following would the addition of an equal volume of \(0.60 \mathrm{M} \mathrm{NaOH}\) lead to a solution having a lower pH: (a) water, (b) \(0.30 \mathrm{M}\) HCl, (c) \(0.70 M \mathrm{KOH}\) (d) \(0.40 M \mathrm{NaNO}_{3} ?\)
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