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Chapter 4: Problem 58

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. Net Ionic Equation: \(Cr^{3+}{(aq)} + 3OH^{-}{(aq)} \rightarrow Cr(OH)_3{(s)}\) b. Net Ionic Equation: \(2Ag^{+}{(aq)}+ CO_3^{2-}{(aq)} \rightarrow 2Ag_2CO_3{(s)}\) c. Net Ionic Equation: \(Hg^{2+}{(aq)} + SO_4^{2-}{(aq)} \rightarrow HgSO_4{(s)}\) d. Net Ionic Equation: \(Sr^{2+}{(aq)} + 2I^{-}{(aq)} \rightarrow SrI_2{(s)}\)

Step by step solution

01

Balanced Molecular Equation

\(CrCl_3{(aq)} + 3NaOH{(aq)} \rightarrow Cr(OH)_3{(s)} + 3NaCl{(aq)}\)
02

Balanced Complete Ionic Equation

\(Cr^{3+}{(aq)} + 3Cl^-{(aq)} + 3Na^{+}{(aq)} + 3OH^{-}{(aq)} \rightarrow Cr(OH)_3{(s)} + 3Na^{+}{(aq)} + 3Cl^-{(aq)}\)
03

Net Ionic Equation

\(Cr^{3+}{(aq)} + 3OH^{-}{(aq)} \rightarrow Cr(OH)_3{(s)}\) b. silver nitrate and ammonium carbonate
04

Balanced Molecular Equation

\(2AgNO_3{(aq)} + (NH_4)_2CO_3{(aq)} \rightarrow 2Ag_2CO_3{(s)} + 2NH_4NO_3{(aq)}\)
05

Balanced Complete Ionic Equation

\(2Ag^{+}{(aq)} + 2NO_3^-{(aq)} + 2NH_4^{+}{(aq)} + CO_3^{2-}{(aq)} \rightarrow 2Ag_2CO_3{(s)} + 2NH_4^{+}{(aq)} + 2NO_3^-{(aq)}\)
06

Net Ionic Equation

\(2Ag^{+}{(aq)}+ CO_3^{2-}{(aq)} \rightarrow 2Ag_2CO_3{(s)}\) c. copper(II) sulfate and mercury(I) nitrate
07

Balanced Molecular Equation

\(CuSO_4{(aq)} + HgNO_3{(aq)} \rightarrow Cu(NO_3)_2{(aq)} + HgSO_4{(s)}\)
08

Balanced Complete Ionic Equation

\(Cu^{2+}{(aq)} + SO_4^{2-}{(aq)} + Hg^{2+}{(aq)} + NO_3^-{(aq)} \rightarrow Cu^{2+}{(aq)} + 2NO_3^-{(aq)} + HgSO_4{(s)}\)
09

Net Ionic Equation

\(Hg^{2+}{(aq)} + SO_4^{2-}{(aq)} \rightarrow HgSO_4{(s)}\) d. strontium nitrate and potassium iodide
10

Balanced Molecular Equation

\(Sr(NO_3)_2{(aq)} + 2KI{(aq)} \rightarrow SrI_2{(s)} + 2KNO_3{(aq)}\)
11

Balanced Complete Ionic Equation

\(Sr^{2+}{(aq)} + 2NO_3^-{(aq)} + 2K^{+}{(aq)} + 2I^{-}{(aq)} \rightarrow SrI_2{(s)} + 2K^{+}{(aq)} + 2NO_3^-{(aq)}\)
12

Net Ionic Equation

\(Sr^{2+}{(aq)} + 2I^{-}{(aq)} \rightarrow SrI_2{(s)}\)

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Most popular questions from this chapter

Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.0200 mole of sodium phosphate in 10.0 mL of solution b. 0.300 mole of barium nitrate in 600.0 mL of solution c. 1.00 g of potassium chloride in 0.500 L of solution d. 132 g of ammonium sulfate in 1.50 L of solution

It took \(25.06 \pm 0.05 \mathrm{mL}\) of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 83). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass

Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: $$\mathrm{IO}_{3}^{-}(a q)+\mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{3}^{-}(a q)$$ Triodide ion concentration is determined by titration with a sodium thiosulfate \(\left(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\right)\) solution. The products are iodide ion and tetrathionate ion \(\left(\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\right)\) a. Balance the equation for the reaction of \(\mathrm{IO}_{3}^{-}\) with \(\mathrm{I}^{-}\) ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HCl required to convert all of the 1 \(\mathrm{O}_{3}^{-}\) ions to \(\mathrm{I}_{3}^{-}\) ions? c. Write and balance the equation for the reaction of \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) with \(\mathrm{I}_{3}-\) in acidic solution. d. A 25.00 -mL sample of a 0.0100\(M\) solution of \(\mathrm{KIO}_{3}\) is reacted with an excess of \(\mathrm{KL}\) . It requires 32.04 \(\mathrm{mL}\) of \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution to titrate the \(\mathrm{I}_{3}^{-}\) ions present. What is the molarity of the \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution? e. How would you prepare 500.0 \(\mathrm{mL}\) of the KIO\(_{3}\)solution in part d using solid \(\mathrm{KIO}_{3} ?\)

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide
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