Solubility Rules and Double replacement reactions Practice Worksheet

Name: ______period: ______
Read the solubility rules (provided or in text) and use to predict the compound that will precipitate out (be insoluble). As you get better you will need to use more skills (balancing and predicting compounds). Use phase notation to indicate theprecipitate (remember, precipitates are insoluble and designated (s) for solid). The soluble ones are (aq) for aqueous. CIRCLE the insoluble product; the one that turns into a solid precipitate.
Example: Silver(I) nitrate + cobalt (II) chloride  Silver(I) chloride + cobalt(II) nitrate

Writing chemical formulas gets: AgNO3 + CoCl2 AgCl + Co(NO3)2

Balanced with Phases: 2AgNO3(aq) + CoCl2(aq) 2AgCl(s) + Co(NO3)2(aq)

1.1 FeCl2(aq) +1 K2S(aq) 2 KCl + 1 FeS (circle the insoluble product)

  1. 1 ZnSO4(aq) +1 SrCl2(aq) 1 ZnCl2 + 1 SrSO4 (circle the insoluble product)
  1. (finish balancing and circle the insoluble product)

___ AlCl3(aq) + ____ Na2CO3(aq)__6__ NaCl(aq) + ___ Al2(CO3)3(s)

  1. (balance and circle the insoluble product; look it up)

___ Na3PO4(aq) + ___ AgNO3(aq) ____ NaNO3 + ___ Ag3PO4

  1. (fill in the missing compounds; determine which product doesn’t dissolve(precipitates out as a solid))

Sodium hydroxide + copper(II) sulfate → Sodium sulfate + copper(II) hydroxide

2 ______(aq) +1 CuSO4(aq) 1 ______( ) + 1 Cu(OH)2( )

6.(Turn the names into compounds and finish balancing)

Sodium chloride + silver(I) nitrate → sodium nitrate + silver (I) chloride

1 ______(aq) + 1 ______(aq) 1 NaNO3(aq) + ______(s)

(do it all for the rest; like your final test)

  1. Manganese (II) sulfate + ammonium sulfide →
  1. Sodium phosphate + silver nitrate →
  1. Cobalt (II) nitrate + sodium hydroxide →
  1. Nickel(II) chloride + sodium sulfide →
  1. Ammonium carbonate + barium hydroxide →

ANSWERS:

Final Answer - Balanced with Phases: the precipitates are circled as well

1.Iron (II) chloride + potassium sulfide →

1 FeCl2(aq) +1 K2S(aq) 2 KCl(aq) + 1 FeS(s)

2.Zinc(II) sulfate + strontium chloride →

1 ZnSO4(aq) +1 SrCl2(aq) 1 ZnCl2(aq) + 1 SrSO4(s)

3.Aluminum chloride + sodium carbonate →

2 AlCl3(aq)+3 Na2CO3(aq) 6 NaCl(aq) + 1 Al2(CO3)3(s)

4.Ammonium sulfate + barium chloride →

1 (NH4)2SO4(aq) +1 BaCl(aq) 2 NH4Cl(aq) + 1 BaSO4(s)

5.Sodium hydroxide + copper(II) sulfate →

2 NaOH(aq) +1 CuSO4(aq) 1 Na2SO4(aq) + 1 Cu(OH)2(s)

6.Sodium chloride + silver(I) nitrate →

1 NaCl(aq) +1 AgNO3(aq) 1 NaNO3(aq) + 1 AgCl(s)

7.Manganese (II) sulfate + ammonium sulfide →

1 MnSO4(aq) +1 (NH4)2S(aq) 1 (NH4)2SO4(aq) + 1 MnS(s)

8.Sodium phosphate + silver nitrate →

1 Na3PO4(aq) + 3 AgNO3(aq) 3 NaNO3(aq) + 1 Ag3PO4(s)

9.Cobalt (II) nitrate + sodium hydroxide →

1 Co(NO3)2(aq) + 2 NaOH(aq) 2 NaNO3(aq) + 1 Co(OH)2(s) will look blue & jelly like

10.Nickel(II) chloride + sodium sulfide →

1 NiCl2(aq) + 1 Na2S(aq) 2 NaCl(aq) + 1 NiS(s)

11.Ammonium carbonate + barium hydroxide →

1 (NH4)2CO3(aq) + 1 Ba(OH)2(aq) 2 NH4OH(aq) + 1 Ba(OH)2(s)

Remember rules are a great place to start but there are some exceptions to the rules.

Solubility Rules

  1. All compounds containing alkali metal cations and the ammonium ion are soluble.
  2. All compounds containing NO3-1, ClO4-1, ClO3-1, and C2H3O2-1 anions are soluble.
  3. All chlorides, bromides, and iodides are soluble except those containing Ag1+, Pb2+, or Hg2+.
  4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
  5. All hydroxides are insoluble except compounds of the alkali metals, Ca2+,Sr2+,and Ba2+.
  6. All compounds containing PO4-3, S-2, CO3-2, and SO3-2 are insoluble except those that also contain alkali metals or NH41+.

The above are general rules of solubility that it is advantageous to memorize (especially for the AP chemistry test

They can be restated as:

Solubility Rules (restated)

  1. All compounds containing alkali metal cations and the ammonium ion are soluble.(1st column and ammonium, NH41+ )
  2. All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.(nitrates, perchlorates, chlorates and acetates are soluble)
  3. All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+.(halides (halogen family) except silver, lead and mercury are soluble)
  4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.(most SO4- compounds are soluble except for mercury, lead and the heavy alkaline earth elements)
  5. All hydroxides are insoluble except compounds of the alkali metals, Ca2+,Sr2+,and Ba2+.(OH- compounds insoluble except for 1st and 2ns columns (Be and Mg don’t dissolve as well)
  6. All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble except those that also contain alkali metals or NH4+.( phosphates, carbonates, sulfites and sulfides are insoluble except the column 1 and Ammonium compounds)