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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

The unknown acid \(\mathrm{H}_{2} \mathrm{X}\) can be neutralized completely by \(\mathrm{OH}^{-}\) according to the following (unbalanced) equation: $$ \mathrm{H}_{2} \mathrm{X}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{X}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ The ion formed as a product, \(\mathrm{X}^{2-},\) was shown to have 36 total electrons. What is element X? Propose a name for \(\mathrm{H}_{2} \mathrm{X}\). To completely neutralize a sample of \(\mathrm{H}_{2} \mathrm{X}, 35.6 \mathrm{~mL}\) of \(0.175 \mathrm{M}\) \(\mathrm{OH}^{-}\) solution was required. What was the mass of the \(\mathrm{H}_{2} \mathrm{X}\) sample used?

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

Hydrochloric acid (75.0 mL of 0.250 \(M\) ) is added to 225.0 mL of 0.0550 \(M\) Ba(OH) \(_{2}\) solution. What is the concentration of the excess \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions left in this solution?

Citric acid, which can he ohtained from lemon juice, has the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\). A 0.250 -g sample of citric acid dissolved in \(25.0 \mathrm{mL}\) of water requires \(37.2 \mathrm{mL}\) of \(0.105 \mathrm{M}\) NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

A stock solution containing \(\mathrm{Mn}^{2+}\) ions was prepared by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution \(A, 50.00 \mathrm{mL}\) of stock solution was diluted to \(1000.0 \mathrm{mL}\) For solution \(B, 10.00 \mathrm{mL}\) of solution \(A\) was diluted to \(250.0 \mathrm{mL}\). For solution \(C, 10.00 \mathrm{mL}\) of solution \(B\) was diluted to \(500.0 \mathrm{mL}\). Calculate the concentrations of the stock solution and solutions \(A, B,\) and \(C .\)
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