Precipitation Reactions

Chemistry ⇒ Chemical Reactions and Equations

Precipitation Reactions starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Precipitation Reactions. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

A chemist adds \mathrm{Na}_2\mathrm{SO}_4 to a solution of \mathrm{CaCl}_2. 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 \mathrm{Ag}^+ ions remaining in solution after mixing 100\,\mathrm{mL} of 0.10\,\mathrm{M} \mathrm{AgNO}_3 with 100\,\mathrm{mL} of 0.10\,\mathrm{M} NaCl, assuming complete precipitation of AgCl.

Calculate the number of moles of \mathrm{BaSO}_4 formed when 100\,\mathrm{mL} of 0.20\,\mathrm{M} \mathrm{BaCl}_2 reacts with excess \mathrm{Na}_2\mathrm{SO}_4.

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 (K_{sp}) in precipitation reactions.

Explain why \mathrm{AgNO}_3 forms a precipitate with NaCl but not with NaNO_3.

Explain why mixing solutions of \mathrm{Na}_2\mathrm{CO}_3 and \mathrm{CaCl}_2 results in a precipitate, but mixing \mathrm{Na}_2\mathrm{CO}_3 and NaCl does not.

Explain why no precipitate forms when solutions of NaNO_3 and KCl are mixed.

If 50.0\,\mathrm{mL} of 0.10\,\mathrm{M} \mathrm{AgNO}_3 is mixed with 50.0\,\mathrm{mL} of 0.10\,\mathrm{M} NaCl, what mass of AgCl will precipitate? (Molar mass of AgCl = 143.32\,\mathrm{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 \mathrm{MgSO}_4(aq) and \mathrm{NaOH}(aq).

Write the net ionic equation for the reaction between aqueous solutions of sodium sulfate and barium nitrate.

A chemist mixes 50.0\,\mathrm{mL} of 0.10\,\mathrm{M} \mathrm{Pb(NO}_3)_2 with 100.0\,\mathrm{mL} of 0.20\,\mathrm{M} \mathrm{Na}_2\mathrm{SO}_4. Calculate the mass of \mathrm{PbSO}_4 that will precipitate. (Molar mass of \mathrm{PbSO}_4 = 303.26\,\mathrm{g/mol})

A solution contains 0.020\,\mathrm{M} \mathrm{Ca}^{2+} and 0.020\,\mathrm{M} \mathrm{Mg}^{2+} ions. When 0.020\,\mathrm{M} \mathrm{Na}_2\mathrm{CO}_3 is added dropwise, which ion will precipitate first? Justify your answer using the solubility product constants: K_{sp}(\mathrm{CaCO}_3) = 4.8 \times 10^{-9}, K_{sp}(\mathrm{MgCO}_3) = 6.8 \times 10^{-6}.

Describe how you would use a precipitation reaction to separate a mixture of \mathrm{Ba}^{2+}, \mathrm{Ca}^{2+}, and \mathrm{Mg}^{2+} ions from an aqueous solution.