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Chapter 17: Problem 64

For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS, \((\mathbf{b}) \mathrm{Pbl}_{2,}(\mathbf{c}) \mathrm{AuCl}_{3},(\mathbf{d}) \mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) (e) CuBr.

Short Answer

Expert verified
Reacting MnS with Strong Acid: \(MnS + 2H^+ \rightarrow Mn^{2+} + H_2S\)

Step by step solution

01

Reacting MnS with Strong Acid

\(MnS + 2H^+ \rightarrow Mn^{2+} + H_2S\) In the case of PbI₂, the net ionic equation is not formed because HI is a strong acid and will not react with H⁺ ions. In the case of AuCl₃, the net ionic equation is not formed because Cl⁻ ion is not reacting with H⁺ ions. In the case of Hg₂C₂O₄, the anions don't react with H⁺, so no net ionic equation is formed. In the case of CuBr, the net ionic equation is not formed because HBr is a strong acid that cannot react with H⁺ ions. So, the only net ionic equation in this exercise is for MnS reacting with a strong acid to form Mn²⁺ and H₂S.

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Most popular questions from this chapter

(a) Calculate the percent ionization of 0.125\(M\) lactic acid \(\left(K_{a}=1.4 \times 10^{-4}\right) .(\) b) Calculate the percent ionization of 0.125\(M\) lactic acid in a solution containing 0.0075\(M\) sodium lactate.

Suggest how the cations in each of the following solution mixtures can be separated: (a) \(\mathrm{Na}^{+}\) and \(\mathrm{Cd}^{2+},(\mathbf{b}) \mathrm{Cu}^{2+}\) and \(\mathrm{Mg}^{2+},(\mathbf{c}) \mathrm{Pb}^{2+}\) and \(\mathrm{Al}^{3+},(\mathbf{d}) \mathrm{Ag}^{+}\) and \(\mathrm{Hg}^{2+}\) .

A solution contains three anions with the following concentrations: \(0.20 M \mathrm{CrO}_{4}^{2-}, 0.10 M \mathrm{CO}_{3}^{2-}\) , a n d 0.010\(M \mathrm{Cl}^{-} .\) If a dilute AgNO \(_{3}\) solution is slowly added to the solution, what is the first compound to precipitate: \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\left(K_{s p}=1.2 \times 10^{-12}\right), \mathrm{Ag}_{2} \mathrm{CO}_{3}\left(K_{s p}=8.1 \times 10^{-12}\right)\) or \(\mathrm{AgCl}\left(K_{s p}=1.8 \times 10^{-10}\right) ?\)

Baking soda (sodium bicarbonate, \(\mathrm{NaHCO}_{3}\)) reacts with acids in foods to form carbonic acid (\(\mathrm{H}_{2} \mathrm{CO}_{3}\)), which in turn decomposes to water and carbon dioxide gas. In a cake batter, the \(\mathrm{CO}_{2}(g)\) forms bubbles and causes the cake to rise. (a) A rule of thumb in baking is that 1\(/ 2\) teaspoon of baking soda is neutralized by one cup of sour milk. The acid component in sour milk is lactic acid, \(\mathrm{CH}_{3} \mathrm{CH (\mathrm{OH}) \)\mathrm{COOH}\( .Write the chemical equation for this neutralization reaction. (b) The density of baking soda is 2.16 \)\mathrm{g} / \mathrm{cm}^{3} .\( Calculate the concentration of lactic acid in one cup of sour milk(assuming the rule of thumb applies), in units of mol/L. (One cup \)=236.6 \mathrm{mL}=48\( teaspoons). (c) If 1/2 teaspoon of baking soda is indeed completely neutralized by the lactic acid in sour milk, calculate the volume of carbon dioxide gas that would be produced at 1 atm pressure, in an oven set to \)350^{\circ} \mathrm{F}$ .

(a) \(\mathrm{A} .0 .1044\) -g sample of an unknown monoprotic acid requires 22.10 \(\mathrm{mL}\) of 0.0500 \(\mathrm{MNaOH}\) to reach the end point. What is the molar mass of the unknown? (b) As the acid is titrated, the pH of the solution after the addition of 11.05 \(\mathrm{mL}\) of the base is \(4.89 .\) What is the \(K_{a}\) for the acid? (c) Using Appendix D, suggest the identity of the acid.
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