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Chapter 17: Problem 62

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

Short Answer

Expert verified
Net ionic equations for the reaction of slightly soluble salts with acid are as follows: a) \(MnS (s) + 2H^{+} (aq) \rightarrow Mn^{2+} (aq) + H_{2}S(g)\) b) \(PbF_{2} (s) + 2H^{+} (aq) \rightarrow Pb^{2+} (aq) + 2HF (g)\) c) \(AuCl_{3} (s) + 3H^{+} (aq) \rightarrow Au^{3+} (aq) + 3HCl (g)\) d) \(Hg_{2}C_{2}O_{4} (s) + 2H^{+} (aq) \rightarrow Hg^{2+} (aq) + 2H_{2}C_{2}O_{4} (aq)\) e) \(CuBr (s) + H^{+} (aq) \rightarrow Cu^{2+} (aq) + HBr (g)\)

Step by step solution

01

Write the balanced molecular equation

MnS (s) + 2H+ (aq) → Mn2+ (aq) + H2S(g)
02

Break the compounds into their respective ions

MnS (s) → Mn2+ (aq) + S2- (aq) 2H+ (aq) → 2H+ (aq) Mn2+ (aq) + H2S(g) → Mn2+ (aq) + H2S(g)
03

Write the net ionic equation

MnS (s) + 2H+ (aq) → Mn2+ (aq) + H2S(g) #b) \(\mathrm{PbF}_{2}\) with Acid#
04

Write the balanced molecular equation

\(\mathrm{PbF}_{2}\) (s) + 2H+ (aq) → Pb2+ (aq) + 2HF (g)
05

Break the compounds into their respective ions

\(\mathrm{PbF}_{2}\) (s) → Pb2+ (aq) + 2F- (aq) 2H+ (aq) → 2H+ (aq) Pb2+ (aq) + 2HF (g) → Pb2+ (aq) + 2HF (g)
06

Write the net ionic equation

\(\mathrm{PbF}_{2}\) (s) + 2H+ (aq) → Pb2+ (aq) + 2HF (g) #c) \(\mathrm{AuCl}_{3}\) with Acid#
07

Write the balanced molecular equation

\(\mathrm{AuCl}_{3}\) (s) + 3H+ (aq) → Au3+ (aq) + 3HCl (g)
08

Break the compounds into their respective ions

\(\mathrm{AuCl}_{3}\) (s) → Au3+ (aq) + 3Cl- (aq) 3H+ (aq) → 3H+ (aq) Au3+ (aq) + 3HCl (g) → Au3+ (aq) + 3HCl (g)
09

Write the net ionic equation

\(\mathrm{AuCl}_{3}\) (s) + 3H+ (aq) → Au3+ (aq) + 3HCl (g) #d) \(\mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) with Acid#
10

Write the balanced molecular equation

\(\mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (s) + 2H+ (aq) → Hg2+ (aq) + 2H2C2O4 (aq)
11

Break the compounds into their respective ions

\(\mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (s) → Hg2+ (aq) + 2C2O42- (aq) 2H+ (aq) → 2H+ (aq) Hg2+ (aq) + 2H2C2O4 (aq) → Hg2+ (aq) + 2H2C2O4 (aq)
12

Write the net ionic equation

\(\mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (s) + 2H+ (aq) → Hg2+ (aq) + 2H2C2O4 (aq) #e) CuBr with Acid#
13

Write the balanced molecular equation

CuBr (s) + H+ (aq) → Cu2+ (aq) + HBr (g)
14

Break the compounds into their respective ions

CuBr (s) → Cu2+ (aq) + Br- (aq) H+ (aq) → H+ (aq) Cu2+ (aq) + HBr (g) → Cu2+ (aq) + HBr (g)
15

Write the net ionic equation

CuBr (s) + H+ (aq) → Cu2+ (aq) + HBr (g)

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Most popular questions from this chapter

A biochemist needs \(750 \mathrm{~mL}\) of an acetic acid-sodium acetate buffer with \(\mathrm{pH}\) 4.50. Solid sodium acetate \(\left(\mathrm{CH}_{3} \mathrm{COONa}\right)\) and glacial acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) are available. Glacial acetic acid is \(99 \% \mathrm{CH}_{3} \mathrm{COOH}\) by mass and has a density of \(1.05 \mathrm{~g} / \mathrm{mL}\). If the buffer is to be \(0.15 \mathrm{M}\) in \(\mathrm{CH}_{3} \mathrm{COOH}\), how many grams of \(\mathrm{CH}_{3} \mathrm{COONa}\) and how many milliliters of glacial acetic acid must be used?

A 20.0-mL sample of \(0.200 \mathrm{M}\) HBr solution is titrated with \(0.200 \mathrm{M} \mathrm{NaOH}\) solution. Calculate the \(\mathrm{pH}\) of the solution after the following volumes of base have been added: (a) \(15.0 \mathrm{~mL}\) (b) \(19.9 \mathrm{~mL}\) (c) \(20.0 \mathrm{~mL},\) (d) \(20.1 \mathrm{~mL},\) (e) \(35.0 \mathrm{~mL}\)

A solution contains \(2.0 \times 10^{-4} \mathrm{MAg}^{+}\) and \(1.5 \times 10^{-3} \mathrm{M}\) \(\mathrm{Pb}^{2+}\). If NaI is added, will AgI \(\left(K_{s p}=8.3 \times 10^{-17}\right)\) or \(\mathrm{PbI}_{2}\) \(\left(K_{s p}=7.9 \times 10^{-9}\right)\) precipitate first? Specify the concentration of \(1^{-}\) needed to begin precipitation.

How many milliliters of \(0.0850 \mathrm{M} \mathrm{NaOH}\) are required to titrate each of the following solutions to the equivalence point: (a) \(40.0 \mathrm{~mL}\) of \(0.0900 \mathrm{M} \mathrm{HNO}_{3}\), (b) \(35.0 \mathrm{~mL}\) of \(0.0850 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{COOH},\) (c) \(50.0 \mathrm{~mL}\) of a solution that contains \(1.85 \mathrm{~g}\) of HCl per liter?

A 20.0 -mL sample of \(0.150 \mathrm{M} \mathrm{KOH}\) is titrated with \(0.125 \mathrm{M}\) \(\mathrm{HClO}_{4}\) solution. Calculate the \(\mathrm{pH}\) after the following volumes of acid have been added: (a) \(20.0 \mathrm{~mL},\) (b) \(23.0 \mathrm{~mL},\) (c) \(24.0 \mathrm{~mL}\), (d) \(25.0 \mathrm{~mL},(\mathrm{e}) 30.0 \mathrm{~mL}\).
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