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Solubility Rules

CSCOPE Unit 10 Lesson 03 Day 1

Rule / Soluble Compounds Contain / Common Exceptions
1 / C2H3O2, CH3COO / None
2 / NH4+ / None
3 / NO3 / None
4 / CN / None
5 / ClO / None
6 / ClO2 / None
7 / ClO3 / None
8 / ClO4 / None
9 / Br / compounds of Ag+, Pb2+, and Hg22+
10 / Cl / compounds of Ag+, Pb2+, and Hg22+
11 / I / compounds of Ag+, Pb2+, and Hg22+
12 / SO42 / compounds of Sr2+, Ba2+, Pb2+, and Hg22+
Rule / Insoluble Compounds Contain / Common Exceptions
13 / CO32 / Compounds of NH4+ and the alkali metal cations
14 / PO43 / Compounds of NH4+ and the alkali metal cations
15 / CrO42 / Compounds of NH4+ and the alkali metal cations
16 / Cr2O72 / Compounds of NH4+ and the alkali metal cations
17 / OH / Compounds of NH4+ and the alkali metal cations,
Ca2+, Sr2+, and Ba2+
18 / S2 / Compounds of NH4+, and the alkali metal cations, Ca2+, Sr2+, and Ba2+

Vocabulary

(s) / indicates that the substance is a solid, used for precipitates
(aq) / indicates that the substance is dissolved in water
Double replacement reaction / the reactants are two compounds and the products are two compounds, two ionic compounds react by exchanging cations to form two new compounds, usually takes place in aqueous solution
Insoluble / a substance that will not dissolve
Precipitate / an insoluble substance that forms in, and separates from, a solution
Soluble / a substance that will dissolve

Students mixed solutions of six different ionic compounds and recorded their observations in the table below.

  • “ppt” in a box in the table means that a precipitate formed – one of the new compounds formed in the double replacement reaction was not soluble in water.
  • A blank white box means that no precipitates formed – both of the new compounds formed in the double replacement reaction were soluble in water.

NaOH / MgSO4 / AgNO3 / NaCl / Ba(NO3)2 / Na2CO3
NaOH
MgSO4 / ppt
AgNO3 / ppt
NaCl / ppt
Ba(NO3)2 / ppt
Na2CO3 / ppt / ppt / ppt

Each of these reactions is a double replacement reaction. For each reaction, write the correct products and balance the equation. Then give the rule number that tells whether or not each compound is soluble. If the product is soluble, then write “(aq)” after the formula. If the product is not soluble (it is a precipitate), then write “(s)” after the formula.

Example
Na2S / + / Pb(NO3)2 /  / 2 NaNO3 (aq) / + / PbS (s)
Rule # / 18 / 3 / 3 / 18
01.
NaOH / + / MgSO4 /  / +
Rule #
02.
NaOH / + / AgNO3 /  / +
Rule #
03.
NaOH / + / NaCl /  / +
Rule #
04.
NaOH / + / Ba(NO3)2 /  / +
Rule #
05.
NaOH / + / Na2CO3 /  / +
Rule #
06.
MgSO4 / + / AgNO3 /  / +
Rule #
07.
MgSO4 / + / NaCl /  / +
Rule #
08.
MgSO4 / + / Ba(NO3)2 /  / +
Rule #
09.
MgSO4 / + / Na2CO3 /  / +
Rule #
10.
AgNO3 / + / NaCl /  / +
Rule #
11.
AgNO3 / + / Ba(NO3)2 /  / +
Rule #
12.
AgNO3 / + / Na2CO3 /  / +
Rule #
13.
NaCl / + / Ba(NO3)2 /  / +
Rule #
14.
NaCl / + / Na2CO3 /  / +
Rule #
15.
Ba(NO3)2 / + / Na2CO3 /  / +
Rule #

CSCOPE Unit 10 Lesson 03 Day 1