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Chapter 6: Problem 53

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

Short Answer

Expert verified
a. \(SO_4^{2-}(aq) + Ba^{2+}(aq) \rightarrow BaSO_4(s)\) b. \(Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\) c. No reaction occurs. d. No reaction occurs. e. \(Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s)\)

Step by step solution

01

Write the balanced molecular equation

For the reaction between ammonium sulfate \((NH_4)_2SO_4\), and barium nitrate \((Ba(NO_3)_2)\): \[(NH_4)_2SO_4 (aq) + Ba(NO_3)_2(aq) \rightarrow 2NH_4NO_3(aq) + BaSO_4(s)\]
02

Write the balanced total ionic equation

Split all strong electrolytes into ions: \[2NH_4^+(aq) + SO_4^{2-}(aq) + Ba^{2+}(aq) + 2NO_3^-(aq) \rightarrow 2NH_4^+(aq) + 2NO_3^-(aq) + BaSO_4(s)\]
03

Write the net ionic equation

Remove the spectator ions (2NH4+ and 2NO3-): \[SO_4^{2-}(aq) + Ba^{2+}(aq) \rightarrow BaSO_4(s)\] b. Lead(II) nitrate and sodium chloride
04

Write the balanced molecular equation

For the reaction between lead(II) nitrate \((Pb(NO_3)_2)\) and sodium chloride \((NaCl)\): \[Pb(NO_3)_2(aq) + 2NaCl(aq) \rightarrow 2NaNO_3(aq) + PbCl_2(s)\]
05

Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Pb^{2+}(aq) + 2NO_3^-(aq) + 2Na^+(aq) + 2Cl^-(aq) \rightarrow 2Na^+(aq) + 2NO_3^-(aq) + PbCl_2(s)\]
06

Write the net ionic equation

Remove the spectator ions (2Na+ and 2NO3-): \[Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s)\] c. Sodium phosphate and potassium nitrate
07

Write the balanced molecular equation

For the reaction between sodium phosphate \((Na_3PO_4)\) and potassium nitrate \((KNO_3)\): \[Na_3PO_4(aq) + 3KNO_3(aq) \rightarrow 3NaNO_3(aq) + K_3PO_4(aq)\]
08

Write the balanced total ionic equation

Split all strong electrolytes into ions: \[3Na^+(aq) + PO_4^{3-}(aq) + 3K^+(aq) + 3NO_3^-(aq) \rightarrow 3Na^+(aq) + 3NO_3^-(aq) + 3K^+(aq) + PO_4^{3-}(aq)\]
09

Write the net ionic equation

All ions are spectator ions, so no reaction occurs. d. Sodium bromide and rubidium chloride
10

Write the balanced molecular equation

For the reaction between sodium bromide \((NaBr)\) and rubidium chloride \((RbCl)\): \[NaBr(aq) + RbCl(aq) \rightarrow NaCl(aq) + RbBr(aq)\]
11

Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Na^+(aq) + Br^-(aq) + Rb^+(aq) + Cl^-(aq) \rightarrow Na^+(aq) + Cl^-(aq) + Rb^+(aq) + Br^-(aq)\]
12

Write the net ionic equation

All ions are spectator ions, so no reaction occurs. e. Copper(II) chloride and sodium hydroxide
13

Write the balanced molecular equation

For the reaction between copper(II) chloride \((CuCl_2)\) and sodium hydroxide \((NaOH)\): \[CuCl_2(aq) + 2NaOH(aq) \rightarrow 2NaCl(aq) + Cu(OH)_2(s)\]
14

Write the balanced total ionic equation

Split all strong electrolytes into ions: \[Cu^{2+}(aq) + 2Cl^-(aq) + 2Na^+(aq) + 2OH^-(aq) \rightarrow 2Na^+(aq) + 2Cl^-(aq) + Cu(OH)_2(s)\]
15

Write the net ionic equation

Remove the spectator ions (2Na+ and 2Cl-): \[Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s)\]

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Most popular questions from this chapter

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

A 100.0-mL aliquot of 0.200 \(M\) aqueous potassium hydroxide is mixed with \(100.0 \mathrm{mL}\) of \(0.200 \mathrm{M}\) 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.

How would you prepare 1.00 L of a \(0.50-M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 \mathrm{M})\) sulfuric acid b. HCl from "concentrated" (12 M) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO_ from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

A 30.0 -mL. sample of an unknown strong base is neutralized after the addition of \(12.0 \mathrm{mL}\) of a \(0.150 \mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is 0.0300 \(M,\) give some possible identities for the unknown base.

A solution is prepared by dissolving 0.6706 g oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make \(100.0 \mathrm{mL}\) of solution. \(\mathrm{A}\) \(10.00-\mathrm{mL}\) aliquot (portion) of this solution is then diluted to a final volume of \(250.0 \mathrm{mL}\). What is the final molarity of the oxalic acid solution?
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