Practice Precipitation Reaction in Chemistry

Use these practice problems to test your method after reviewing the concept explanation and worked examples.

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Quick Recap

A type of double displacement reaction in which two aqueous ionic solutions are mixed and the exchange of ions produces at least one insoluble ionic compound (a precipitate) that drops out of solution as a solid.

Mix two clear solutions and a solid appears 'out of nowhere' β€” the ions combine to form a compound that won't dissolve.

Showing a random 20 of 50 problems.

Example 1

medium
Write the net ionic equation for AgNO3(aq)+NaCl(aq)β†’AgCl(s)+NaNO3(aq)\text{AgNO}_3\text{(aq)} + \text{NaCl(aq)} \rightarrow \text{AgCl(s)} + \text{NaNO}_3\text{(aq)}.

Example 2

medium
How many grams of AgCl form when 50.0 mL50.0\,\text{mL} of 0.200 M0.200\,\text{M} AgNO3_3 reacts with excess NaCl? (MAgCl=143.32 g/molM_\text{AgCl} = 143.32\,\text{g/mol}.)

Example 3

easy
Two clear solutions mix and a solid appears. What reaction occurred?

Example 4

challenge
0.10 mol AgNO3 reacts with excess NaCl. Mass of AgCl (M=143.5) precipitate?

Example 5

medium
Predict and balance: AgNO3+Na2CO3β†’AgNO_3 + Na_2CO_3 \rightarrow ? (Ag2CO3Ag_2CO_3 insoluble)

Example 6

easy
How is a precipitate denoted in an equation?

Example 7

easy
Are sodium nitrates ever a precipitate?

Example 8

medium
Does NaCl+KNO3NaCl + KNO_3 form a precipitate? Use solubility rules.

Example 9

medium
Predict whether a precipitate forms when solutions of Pb(NO3)2\text{Pb(NO}_3)_2 and KI\text{KI} are mixed. If so, identify the precipitate and write the balanced equation. Use solubility rules: most iodides are soluble, but PbI2\text{PbI}_2 is insoluble.

Example 10

easy
Symbol used to indicate a precipitate forming in an equation?

Example 11

medium
List the spectator ions when Pb(NO3)2\text{Pb(NO}_3)_2 reacts with KI\text{KI} to give PbI2\text{PbI}_2.

Example 12

medium
Predict and balance: FeCl2+Na2S→FeCl_2 + Na_2S \rightarrow ? (FeS insoluble)

Example 13

challenge
How many mol Na2CO3Na_2CO_3 are needed to fully precipitate 0.30 mol CaCl2CaCl_2 as CaCO3CaCO_3?

Example 14

medium
Using solubility rules (nitrates soluble, most sulfates soluble except Ba/Pb/Ca): does Ba(NO3)2+K2SO4Ba(NO_3)_2 + K_2SO_4 precipitate?

Example 15

challenge
25.0 mL25.0\,\text{mL} of 0.200 M0.200\,\text{M} AgNO3_3 is added to 25.0 mL25.0\,\text{mL} of 0.100 M0.100\,\text{M} Na2_2CrO4_4. Identify the limiting reactant and the mass of Ag2_2CrO4_4 precipitate. (M_\text{Ag}_2\text{CrO}_4 = 331.7\,\text{g/mol}.)

Example 16

medium
Are precipitation reactions reversible at the macroscopic level under typical lab conditions?

Example 17

hard
100.0 mL100.0\,\text{mL} of 0.150 M0.150\,\text{M} Pb(NO3_3)2_2 is mixed with 100.0 mL100.0\,\text{mL} of 0.300 M0.300\,\text{M} NaI. Find the mass of PbI2_2 precipitate. (M_\text{PbI}_2 = 461.0\,\text{g/mol}.)

Example 18

medium
Mixing CuSO4_4(aq) and NaOH(aq) yields a blue precipitate. Identify it and write the molecular equation.

Example 19

easy
Complete: Pb(NO3)2+2KI→Pb(NO_3)_2 + 2KI \rightarrow ? (PbI2 is insoluble)

Example 20

easy
Are most Group 1 (alkali metal) salts soluble in water?
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