Precipitation Reactions
Chemistry ⇒ Chemical Reactions and Equations
Precipitation Reactions starts at 10 and continues till grade 12.
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See sample questions for grade 12
A chemist adds Na2SO4 to a solution of CaCl2. Will a precipitate form? If yes, name it.
A student mixes solutions of potassium iodide and lead(II) nitrate. What is the color of the precipitate formed?
Calculate the concentration of Ag+ ions remaining in solution after mixing 100 mL of 0.10 M AgNO3 with 100 mL of 0.10 M NaCl, assuming complete precipitation of AgCl.
Calculate the number of moles of BaSO4 formed when 100 mL of 0.20 M BaCl2 reacts with excess Na2SO4.
Describe how you would experimentally confirm the formation of a precipitate in a reaction.
Describe the difference between a complete ionic equation and a net ionic equation in precipitation reactions.
Describe the steps to predict whether a precipitate will form when two aqueous solutions are mixed.
Explain the role of solubility product (Ksp) in precipitation reactions.
Explain why AgNO3 forms a precipitate with NaCl but not with NaNO3.
Explain why mixing solutions of Na2CO3 and CaCl2 results in a precipitate, but mixing Na2CO3 and NaCl does not.
Explain why no precipitate forms when solutions of NaNO3 and KCl are mixed.
If 50.0 mL of 0.10 M AgNO3 is mixed with 50.0 mL of 0.10 M NaCl, what mass of AgCl will precipitate? (Molar mass of AgCl = 143.32 g/mol)
State the general rule for the solubility of sulfates in water.
Which of the following best explains why precipitation reactions are important in water treatment processes?
Write the balanced chemical equation for the precipitation reaction between barium chloride and sodium sulfate.
Write the ionic equation for the reaction between MgSO4(aq) and NaOH(aq).
Write the net ionic equation for the reaction between aqueous solutions of sodium sulfate and barium nitrate.
A chemist mixes 50.0 mL of 0.10 M Pb(NO3)2 with 100.0 mL of 0.20 M Na2SO4. Calculate the mass of PbSO4 that will precipitate. (Molar mass of PbSO4 = 303.26 g/mol)
A solution contains 0.020 M Ca2+ and 0.020 M Mg2+ ions. When 0.020 M Na2CO3 is added dropwise, which ion will precipitate first? Justify your answer using the solubility product constants: Ksp(CaCO3) = 4.8 × 10−9, Ksp(MgCO3) = 6.8 × 10−6.
Describe how you would use a precipitation reaction to separate a mixture of Ba2+, Ca2+, and Mg2+ ions from an aqueous solution.
