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Chapter 4: Problem 57

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
Net ionic equations: a. Ammonium sulfate and barium nitrate: \[ Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) \] b. Lead(II) nitrate and sodium chloride: \[ Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s) \] c. Sodium phosphate and potassium nitrate: No reaction. d. Sodium bromide and rubidium chloride: No reaction. e. Copper(II) chloride and sodium hydroxide: \[ Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s) \]

Step by step solution

01

a. Ammonium sulfate and barium nitrate

1. Write the chemical formulas for the reactants: Ammonium sulfate: \( (NH_4)_2SO_4 \) Barium nitrate: \( Ba(NO_3)_2 \) 2. Exchange anions and write the chemical formulas for the possible products: Ammonium nitrate: \( NH_4NO_3 \) Barium sulfate: \( BaSO_4 \) 3. Check solubility rules: Ammonium nitrate is soluble because all ammonium salts are soluble. Barium sulfate is insoluble because sulfate salts are generally insoluble, with some exceptions (which barium is not a part of). 4. Write the net ionic equation: Since barium sulfate is insoluble, the net ionic equation is: \[ Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) \]
02

b. Lead(II) nitrate and sodium chloride

1. Write the chemical formulas for the reactants: Lead(II) nitrate: \( Pb(NO_3)_2 \) Sodium chloride: \( NaCl \) 2. Exchange anions and write the chemical formulas for the possible products: Lead(II) chloride: \( PbCl_2 \) Sodium nitrate: \( NaNO_3 \) 3. Check solubility rules: Lead(II) chloride is insoluble because chloride salts are generally soluble, but lead(II) is an exception. Sodium nitrate is soluble because all nitrates are soluble. 4. Write the net ionic equation: Since lead(II) chloride is insoluble, the net ionic equation is: \[ Pb^{2+}(aq) + 2Cl^-(aq) \rightarrow PbCl_2(s) \]
03

c. Sodium phosphate and potassium nitrate

1. Write the chemical formulas for the reactants: Sodium phosphate: \( Na_3PO_4 \) Potassium nitrate: \( KNO_3 \) 2. Exchange anions and write the chemical formulas for the possible products: Sodium nitrate: \( NaNO_3 \) Potassium phosphate: \( K_3PO_4 \) 3. Check solubility rules: Both sodium nitrate and potassium phosphate are soluble (all nitrates and sodium and potassium salts are soluble). 4. Since both possible products are soluble, no reaction occurs.
04

d. Sodium bromide and rubidium chloride

1. Write the chemical formulas for the reactants: Sodium bromide: \( NaBr \) Rubidium chloride: \( RbCl \) 2. Exchange anions and write the chemical formulas for the possible products: Sodium chloride: \( NaCl \) Rubidium bromide: \( RbBr \) 3. Check solubility rules: Both sodium chloride and rubidium bromide are soluble (all sodium and rubidium salts are soluble). 4. Since both possible products are soluble, no reaction occurs.
05

e. Copper(II) chloride and sodium hydroxide

1. Write the chemical formulas for the reactants: Copper(II) chloride: \( CuCl_2 \) Sodium hydroxide: \( NaOH \) 2. Exchange anions and write the chemical formulas for the possible products: Copper(II) hydroxide: \( Cu(OH)_2 \) Sodium chloride: \( NaCl \) 3. Check solubility rules: Copper(II) hydroxide is insoluble because hydroxide salts are generally insoluble, except alkali metal and some alkaline earth metal hydroxides. Sodium chloride is soluble because all sodium salts are soluble. 4. Write the net ionic equation: Since copper(II) hydroxide is insoluble, the net ionic equation is: \[ Cu^{2+}(aq) + 2OH^-(aq) \rightarrow Cu(OH)_2(s) \]

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Most popular questions from this chapter

A 230 -mL sample of a \(0.275-M \mathrm{CaCl}_{2}\) solution is left on a hot plate overnight; the following morning, the solution is 1.10\(M .\) What volume of water evaporated from the 0.275\(M \mathrm{CaCl}_{2}\) solution?

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) A 0.205-g sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The BaSO\(_{4}\) that is formed is filtered, dried, and weighed. Its mass is 0.298 g. What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

Citric acid, which can be obtained 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 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ A 10.00-g mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with 156 mL of 3.00 M silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If 78.0 mL of HCl was added, what was the concentration of the HCl?

A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions left in solution.
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