1) Evaluate the solubility of the following ionic substances.

1. NaOH c. MgCO3 e. Ag2SO4
2. PbCl2 d. K3PO4 f. CaSO4

Dr. Blackburn

g. Ba3(PO4)2

h. (NH4)2CO3

1. 2) Predict the products that can form if the following aqueous reagents are mixed. This includes making sure the chemical formulas are charged balanced. Evaluate the solubility of the products and include the correct phase designations after the chemical formulas.
   1. KCl (aq) + Pb(NO2)2 (aq) à
   2. Na2SO4 (aq) + CaCl2 (aq) à
   3. MgSO4 (aq) + Na3PO4 (aq) à
   4. Na2S (aq) + CaCl2 (aq) à
2. 3) Write the complete ionic equation for the following molecular equations.
   1. MgCl2(aq) + 2AgNO3(aq) →2AgCl(s) + Mg(NO3)2(aq)
   2. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
   3. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq)
3. 4) Write the net ionic equation for the following reactions.
   1. Na+(aq) + Cl ̄(aq) + Ag+(aq) + NO3 ̄(aq) —> AgCl(s) + Na+(aq) + NO3 ̄(aq)
   2. 6Na+ (aq)+2PO43- (aq)+3Ca2+ (aq)+6Cl- (aq)–>6Na+ (aq)+6Cl- (aq)+Ca3(PO4)2 (s)
   3. 6NH4+ (aq)+3CO32- (aq)+2Al3+(aq)+6NO3-(aq)–>6NH4+ (aq)+6NO3- (aq)+Al2(CO3)3 (s)
   4. 2Na+ (aq)+2OH- (aq)+2H+ (aq)+SO42- (aq)–>2Na+ (aq)+SO42- (aq)+2H2O(l)

5) Use the following choices to classify each reaction given below (more than one choice may apply).

1. oxidation-reduction
2. neutralization (acid-base)
3. precipitation

d. double displacement e. single displacement f. combustion

g. synthesis
h. decomposition

C3H8 (g) + O2(g) à CO2 (g ) + H2O(g) Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) Zr(s) + O2(g) → ZrO2(s)
6Na(s) + N2(g) → 2Na3N(s)

2Hg(l) + O2(g) → 2HgO(s) Ca(s) + H2(g) → CaH2(s) 8Fe(s)+S8(s)→8FeS(s) 2 KCl(s) → 2 K(s) + Cl2(g)

1. ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s)
2. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq)
3. HC2H3O2(aq) + CsOH(aq) → H2O(l) + CsC2H3O2(aq)
4. HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3(aq)
5. H2SO4(aq) + Ba(OH)2(aq) → 2H2O(l) + BaSO4(s)
6. 2HCl(aq) + Pb(OH)2(aq) → PbCl2(s) + 2H2O(l)
7. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
8. 2AgNO3(aq) + Zn(s) → 2Ag(s) + Zn(NO3)2(aq)

ix. x. xi. xii. xiii. xiv. xv. xvi.

6) Identify whether the following reactions are molecular equations, complete ionic equations, or net ionic equations.

1. Cu2+(aq) + 2NO3-(aq) + 2Na+(aq) + 2OH-(aq) →Cu(OH)2(s) + 2Na+(aq) + 2NO3-(aq)
2. Ba2+(aq) + SO42-(aq) →BaSO4 (s)
3. HNO3(aq) + KOH(aq) →KNO3(aq) +H2O(l)
4. Ba2+(aq) + 2OH-(aq) + 2H+(aq) + 2Cl-(aq) →2H2O(l) + Ba2+(aq) + 2Cl-(aq)

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