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Chapter 4: Problem 52

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. chromium(III) chloride and sodium hydroxide b. silver nitrate and ammonium carbonate c. copper(II) sulfate and mercury(I) nitrate d. strontium nitrate and potassium iodide

Short Answer

Expert verified
a. \(Cr^{3+}(aq) + 3OH^-(aq) \rightarrow Cr(OH)_3(s)\) b. \(2Ag^+(aq) + CO_3^{2-}(aq) \rightarrow 2AgCO_3(s)\) c. \(SO_4^{2-}(aq) + Hg_2^{2+}(aq) \rightarrow Hg_2SO_4(s)\) d. \(Sr^{2+}(aq) + 2I^-(aq) \rightarrow SrI_2(s)\)

Step by step solution

01

Write the balanced molecular equation

CrCl3(aq) + 3NaOH(aq) -> Cr(OH)3(s) + 3NaCl(aq)
02

Break each reactant and product into ions

CrCl3 (aq) -> Cr3+ (aq) + 3Cl- (aq) NaOH (aq) -> Na+ (aq) + OH- (aq) Cr(OH)3 (s) -> Cr(OH)3 (s) NaCl (aq) -> Na+ (aq) + Cl- (aq)
03

Write the complete ionic equation

Cr3+(aq) + 3Cl-(aq) + 3Na+(aq) + 3OH-(aq) -> Cr(OH)3(s) + 3Na+(aq) + 3Cl-(aq)
04

Write the net ionic equation

Cr3+(aq) + 3OH-(aq) -> Cr(OH)3(s) b. silver nitrate and ammonium carbonate
05

Write the balanced molecular equation

2AgNO3(aq) + (NH4)2CO3(aq) -> 2Ag2CO3(s) + 2NH4NO3(aq)
06

Break each reactant and product into ions

AgNO3 (aq) -> Ag+ (aq) + NO3- (aq) (NH4)2CO3 (aq) -> 2NH4+ (aq) + CO3^2- (aq) Ag2CO3 (s) -> Ag2CO3 (s) NH4NO3 (aq) -> NH4+ (aq) + NO3- (aq)
07

Write the complete ionic equation

2Ag+(aq) + 2NO3-(aq) + 2NH4+(aq) + CO3^2-(aq) -> 2AgCO3(s) + 2NH4+(aq) + 2NO3-(aq)
08

Write the net ionic equation

2Ag+(aq) + CO3^2-(aq) -> 2AgCO3(s) c. copper(II) sulfate and mercury(I) nitrate
09

Write the balanced molecular equation

CuSO4(aq) + 2HgNO3(aq) -> Cu(NO3)2(aq) + Hg2SO4(s)
10

Break each reactant and product into ions

CuSO4 (aq) -> Cu2+ (aq) + SO4^2- (aq) HgNO3 (aq) -> Hg2^2+ (aq) + 2NO3- (aq) Cu(NO3)2 (aq) -> Cu2+ (aq) + 2NO3- (aq) Hg2SO4 (s) -> Hg2SO4 (s)
11

Write the complete ionic equation

Cu^2+(aq) + SO4^2-(aq) + Hg2^2+(aq) + 2NO3-(aq) -> Cu^2+(aq) + 2NO3-(aq) + Hg2SO4(s)
12

Write the net ionic equation

SO4^2-(aq) + Hg2^2+(aq) -> Hg2SO4(s) d. strontium nitrate and potassium iodide
13

Write the balanced molecular equation

Sr(NO3)2(aq) + 2KI(aq) -> SrI2(s) + 2KNO3(aq)
14

Break each reactant and product into ions

Sr(NO3)2 (aq) -> Sr2+ (aq) + 2NO3- (aq) KI (aq) -> K+ (aq) + I- (aq) SrI2 (s) -> SrI2 (s) KNO3 (aq) -> K+ (aq) + NO3- (aq)
15

Write the complete ionic equation

Sr2+(aq) + 2NO3-(aq) + 2K+(aq) + 2I-(aq) -> SrI2(s) + 2K+(aq) + 2NO3-(aq)
16

Write the net ionic equation

Sr2+(aq) + 2I-(aq) -> SrI2(s)

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Most popular questions from this chapter

A 0.500-L sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution was analyzed by taking a \(100.0-\mathrm{mL}\) aliquot and adding \(50.0 \mathrm{~mL}\) of \(0.213 M \mathrm{NaOH}\). After the reaction occurred, an excess of \(\mathrm{OH}^{-}\) ions remained in the solution. The excess base required \(13.21 \mathrm{~mL}\) of \(0.103 \mathrm{M} \mathrm{HCl}\) for neutralization. Calculate the molarity of the original sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Sulfuric acid has two acidic hydrogens.

A \(100.0-\mathrm{mL}\) aliquot of \(0.200 M\) aqueous potassium hydroxide is mixed with \(100.0 \mathrm{~mL}\) of \(0.200 M\) aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.

What mass of solid \(\mathrm{AgBr}\) is produced when \(100.0 \mathrm{~mL}\) of \(0.150 \mathrm{M}\) \(\mathrm{AgNO}_{3}\) is added to \(20.0 \mathrm{~mL}\) of \(1.00 M \mathrm{NaBr} ?\)

Describe how you would prepare \(2.00 \mathrm{~L}\) of each of the following solutions. a. \(0.250 \mathrm{M} \mathrm{NaOH}\) from solid \(\mathrm{NaOH}\) b. \(0.250 \mathrm{M} \mathrm{NaOH}\) from \(1.00 \mathrm{M} \mathrm{NaOH}\) stock solution c. \(0.100 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr} \mathrm{O}_{4}\) from solid \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) d. \(0.100 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr} \mathrm{O}_{4}\) from \(1.75 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) stock solution

The vanadium in a sample of ore is converted to \(\mathrm{VO}^{2+}\). The VO \(^{2+}\) ion is subsequently titrated with \(\mathrm{MnO}_{4}^{-}\) in acidic solution to form \(\mathrm{V}(\mathrm{OH})_{4}{ }^{+}\) and manganese(II) ion. The unbalanced titration reaction is \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{VO}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) $$ \mathrm{V}(\mathrm{OH})_{4}^{+}(a q)+\mathrm{Mn}^{2+}(a q)+\mathrm{H}^{+}(a q) $$ To titrate the solution, \(26.45 \mathrm{~mL}\) of \(0.02250 \mathrm{M} \mathrm{MnO}_{4}^{-}\) was required. If the mass percent of vanadium in the ore was \(58.1 \%\), what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.
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