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Chapter 4: Problem 51

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. \( Pb^{2+}(aq) + 2 Cl^-(aq) \rightarrow PbCl_2(s) \) c. No net ionic equation, as all ions are spectator ions. d. No net ionic equation, as all ions are spectator ions. e. \( Cu^{2+}(aq) + 2 OH^-(aq) \rightarrow Cu(OH)_2(s) \)

Step by step solution

01

a. Ammonium sulfate and barium nitrate

Step 1: Write the balanced molecular equation \( (NH_4)_2 SO_4(aq) + Ba(NO_3)_2(aq) \rightarrow 2 NH_4NO_3(aq) + BaSO_4(s) \) Step 2: Write the complete ionic equation \( 2 NH_4^+(aq) + SO_4^{2-}(aq) + Ba^{2+}(aq) + 2 NO_3^-(aq) \rightarrow 2 NH_4^+(aq) + 2 NO_3^-(aq) + BaSO_4(s) \) Step 3: Write the net ionic equation (cancel out spectator ions) \( SO_4^{2-}(aq) + Ba^{2+}(aq) \rightarrow BaSO_4(s) \)
02

b. Lead(II) nitrate and sodium chloride

Step 1: Write the balanced molecular equation \( Pb(NO_3)_2(aq) + 2 NaCl(aq) \rightarrow 2 NaNO_3(aq) + PbCl_2(s) \) Step 2: Write the complete ionic equation \( Pb^{2+}(aq) + 2 NO_3^-(aq) + 2 Na^+(aq) + 2 Cl^-(aq) \rightarrow 2 Na^+(aq) + 2 NO_3^-(aq) + PbCl_2(s) \) Step 3: Write the net ionic equation (cancel out spectator ions) \( Pb^{2+}(aq) + 2 Cl^-(aq) \rightarrow PbCl_2(s) \)
03

c. Sodium phosphate and potassium nitrate

Step 1: Write the balanced molecular equation \( Na_3PO_4(aq) + 3 KNO_3(aq) \rightarrow 3 NaNO_3(aq) + K_3PO_4(aq) \) Step 2: Write the complete ionic equation \( 3 Na^+(aq) + PO_4^{3-}(aq) + 3 K^+(aq) + 3 NO_3^-(aq) \rightarrow 3 Na^+(aq) + 3 NO_3^-(aq) + 3 K^+(aq) + PO_4^{3-}(aq) \) Step 3: Write the net ionic equation (cancel out spectator ions) There is no net ionic equation, as all ions are spectator ions.
04

d. Sodium bromide and rubidium chloride

Step 1: Write the balanced molecular equation \( NaBr(aq) + RbCl(aq) \rightarrow NaCl(aq) + RbBr(aq) \) Step 2: Write the complete ionic equation \( Na^+(aq) + Br^-(aq) + Rb^+(aq) + Cl^-(aq) \rightarrow Na^+(aq) + Cl^-(aq) + Rb^+(aq) + Br^-(aq) \) Step 3: Write the net ionic equation (cancel out spectator ions) There is no net ionic equation, as all ions are spectator ions.
05

e. Copper(II) chloride and sodium hydroxide

Step 1: Write the balanced molecular equation \( CuCl_2(aq) + 2 NaOH(aq) \rightarrow 2 NaCl(aq) + Cu(OH)_2(s) \) Step 2: Write the complete ionic equation \( Cu^{2+}(aq) + 2 Cl^-(aq) + 2 Na^+(aq) + 2 OH^-(aq) \rightarrow 2 Na^+(aq) + 2 Cl^-(aq) + Cu(OH)_2(s) \) Step 3: Write the net ionic equation (cancel out spectator ions) \( Cu^{2+}(aq) + 2 OH^-(aq) \rightarrow Cu(OH)_2(s) \)

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Most popular questions from this chapter

Acetylsalicylic acid is the active ingredient in aspirin. It took \(35.17 \mathrm{~mL}\) of \(0.5065 M\) sodium hydroxide to react completely with \(3.210 \mathrm{~g}\) of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

What volume of each of the following bases will react completely with \(25.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\) ? a. \(0.100 \mathrm{M} \mathrm{NaOH}\) b. \(0.0500 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\) c. \(0.250 \mathrm{M} \mathrm{KOH}\)

The zinc in a \(1.343-g\) sample of a foot powder was precipitated as \(\mathrm{ZnNH}_{4} \mathrm{PO}_{4} .\) Strong heating of the precipitate yielded \(0.4089 \mathrm{~g} \mathrm{Zn}_{2} \mathrm{P}_{2} \mathrm{O}_{7} .\) Calculate the mass percent of zinc in the sample of foot powder.

Three students were asked to find the identity of the metal in a particular sulfate salt. They dissolved a \(0.1472-\mathrm{g}\) sample of the salt in water and treated it with excess barium chloride, resulting in the precipitation of barium sulfate. After the precipitate had been filtered and dried, it weighed \(0.2327 \mathrm{~g}\). Each student analyzed the data independently and came to different conclusions. Pat decided that the metal was titanium. Chris thought it was sodium. Randy reported that it was gallium. What formula did each student assign to the sulfate salt? Look for information on the sulfates of gallium, sodium, and titanium in this text and reference books such as the \(C R C\) Handbook of Chemistry and Physics. What further tests would you suggest to determine which student is most likely correct?

What mass of silver chloride can be prepared by the reaction of \(100.0 \mathrm{~mL}\) of \(0.20 \mathrm{M}\) silver nitrate with \(100.0 \mathrm{~mL}\) of \(0.15 \mathrm{M}\) calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.
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