Chapter 4

Write two sets of equations (both molecular and total ionic) with different reactants that have the same net ionic equation as the following equation: $$ \mathrm{Ba}\left(\mathrm{NO}_{0}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{BaCO}_{3}(s)+2 \mathrm{NaNO}_{3}(a q) $$

Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations: (a) \(\mathrm{CaCl}_{2}(a q)+\mathrm{Cs}_{3} \mathrm{PO}_{4}(a q) \longrightarrow\) (b) \(\mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{ZnSO}_{4}(a q) \longrightarrow\)

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium nitrate \(+\) copper(II) sulfate (b) Ammonium bromide + silver nitrate

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Potassium carbonate + barium hydroxide (b) Aluminum nitrate \(+\) sodium phosphate

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations. (a) Potassium chloride + iron(III) nitrate (b) Ammonium sulfate + barium chloride

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium sulfide + nickel(II) sulfate (b) Lead(II) nitrate + potassium bromide

If \(38.5 \mathrm{~mL}\) of lead(II) nitrate solution reacts completely with excess sodium iodide solution to yield \(0.628 \mathrm{~g}\) of precipitate, what is the molarity of lead(II) ion in the original solution?

How many grams of barium sulfate form when \(35.0 \mathrm{~mL}\) of \(0.160 \mathrm{M}\) barium chloride reacts with \(58.0 \mathrm{~mL}\) of \(0.065 \mathrm{M}\) sodium sulfate?

How many grams of iron(III) sulfide form when \(62.0 \mathrm{~mL}\) of \(0.135 \mathrm{M}\) iron(III) chloride reacts with \(45.0 \mathrm{~mL}\) of \(0.285 \mathrm{M}\) calcium sulfide?

The mass percent of \(\mathrm{Cl}^{-}\) in a seawater sample is determined by titrating \(25.00 \mathrm{~mL}\) of seawater with \(\mathrm{AgNO}_{3}\) solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free \(\mathrm{Ag}^{+}\) ion is present in solution after all the \(\mathrm{Cl}^{-}\) has reacted. If \(53.63 \mathrm{~mL}\) of \(0.2970 \mathrm{M} \mathrm{AgNO}_{3}\) is required to reach the end point, what is the mass percent of \(\mathrm{Cl}^{-}\) in the seawater \((d\) of seawater \(=1.024 \mathrm{~g} / \mathrm{mL}) ?\)