Worksheet #12
Gas Forming Reactions
1. Write the molecular, total and net ionic equations for the reaction of sodium carbonate with
sulfuric acid, and identify the spectator ions
2. When sodium bicarbonate (baking soda) reacts with hydrochloric acid, what products are
formed? Write the molecular, total and net ionic equations for this reaction, and identify the
spectator ions.
3. If ammonium perchlorate reacts with lithium hydroxide, what species will form? Write the
molecular, total and net ionic equations for this reaction, and identify the spectator ions.
4. If sodium sulfite reacts with perchloric acid, what products will form? Write the molecular,
total and net ionic equations for this reaction, and identify the spectator ions.
Reactions in Aqueous Solutions
5. Write an example precipitation reaction, showing exactly what happens in the solution (i.e.
write the net ionic equation).
6. Write an example of an acid/base reaction, showing exactly what happens in solution.
7. Write an example of a gas forming reaction, showing exactly what happens in solution.
Writing Molecular, Total Ionic, and Net Ionic Equations
8. Write the molecular, total and net ionic equations for a mixture of Pb(ClO4)2 and NaCl.
Identify the spectator ions
9. Write the molecular, total and net ionic equations for a mixture of BaCl2 and Na2SO4.
Identify the spectator ions.
10. Write the molecular and net ionic equations for the following aqueous reactions. If no
reaction occurs, write NR.
a) Ba(NO3)2 + K2SO4
b) Mg(NO3)2 + K2SO4
c) CaCl2 + Al(NO3)3
d) NiCl2 + NaBr
e) Na2CO3 + MgBr2.
11. Write the net ionic equation for each of the following. Use the general rules for solubility
(Bauer Table 5.3, p 177).
a) H2SO4(aq) + BaCl2(aq) = ?
b) NaHSO3(aq) + HCl(aq) = NaCl(aq) + SO2(g) + H2O
c) CaO(s) + 2HCl(aq) = CaCl2(aq) + H2O
Worksheet 12
1
12. Which of the following metathesis (double-replacement) reactions will go? Write the
products for any reactions that will occur.
a) KCl(aq) + HNO3(aq) = ?
b) Na2CO3(aq) + H2SO4(aq) = ?
c) AgNO3(aq) + CH3COOH(aq) [acetic acid] = ?
Answers to Worksheet #12
Gas Forming Reactions
1. Molecular: __Na2CO3(aq) + __H2SO4(aq) → __H2O(ℓ) + __CO2(g) + __Na2SO4(aq)
Total Ionic: 2Na+(aq)+CO32-(aq) + 2H+(aq) + SO42-(aq) → H2O(ℓ)+ CO2(g) + 2Na+(aq) + SO42-(aq)
Net Ionic: CO32-(aq) + 2H+(aq) → H2O (ℓ) + CO2(g)
Spectators: Na+ and SO422. Molecular: __NaHCO3(aq) + __HCl(aq) → __H2O(ℓ) + __CO2(g) + __NaCl(aq)
Total Ionic: Na+(aq) +HCO3-(aq) + H+(aq) + Cl-(aq) → H2O(ℓ) + CO2(g) + Na+(aq) + Cl-(aq)
Net Ionic: HCO3-(aq) + H+(aq) → H2O(ℓ) + CO2(g)
Spectators: Na+ and C13. Molecular: __NH4ClO4(aq) + __LiOH(aq) → __LiClO4(aq) + __NH3(g) + __H2O(ℓ)
Total Ionic: NH4+(aq)+ClO4-(aq) +Li+(aq)+OH-(aq) → Li+(aq)+ClO4-(aq)+NH3(g)+H2O(ℓ)
Net Ionic: NH4+(aq) + OH- (aq) → NH3(g) + H2O(ℓ)
Spectators: ClO4- and Li+
4. Molecular: __Na2SO3(aq) + 2HClO4(aq) → 2NaClO4(aq) + SO2(g) + H2O(ℓ)
Total Ionic: 2Na+(aq)+ SO32-(aq) + 2H+(aq) + 2ClO4-(aq) → 2Na+(aq) + 2ClO4-(aq) + SO2(g)+H2O(ℓ)
Net Ionic: SO32-(aq) + 2H+(aq) → SO2(g) + H2O(ℓ)
Spectators: Na+ and ClO4Reactions in Aqueous Solutions
5. Molecular: __AgNO3(aq) + __NaCl(aq) → __AgCl(s) + __NaNO3(aq)
Net Ionic: Ag+(aq) + Cl-(aq) → AgCl(s)
6. Molecular: __HCl(aq) + __NaOH(aq) → __NaCl(aq) + __H2O(ℓ)
Net Ionic: H+(aq) + OH-(aq) → H2O(ℓ)
7. Molecular: __Na2O3(aq) + __H2SO4(aq) → __H2O(ℓ) + __CO2 + Na2SO4(aq)
Net Ionic: CO32-(aq) + 2H+(aq) → H2O(ℓ) + CO2(g)
Molecular, Total Ionic, and Net Ionic Equations
Molecular equations are balanced equations that show all soluble aqueous ionic substances as
un-dissociated compounds. Remember to balance the equation and use phase labels. Total ionic
equations show all soluble aqueous ionic substances as dissociated into ions. Remember to
balance the equation, use phase labels, and state the charges of all ions. Only dissociate
Worksheet 12
2
substances that are (aq). Do not dissociate (s), (ℓ), or (g). Net ionic equations only show the ions
that react to form a precipitate. Remember to balance the equation, use phase labels, and state
the charges of all ions. A reaction only occurs if a precipitate is made. A spectator ion is an ion
that is present as part of a reagent solution that does not take part in the reaction.
8. Molecular: _Pb(ClO4)2(aq) + 2NaCl(aq) → 2NaClO4(aq) + _PbCl2(s)
Total Ionic: Pb2+ (aq) + 2ClO4-(aq) + 2Na+ (aq) + 2Cl-(aq) → 2Na+(aq) + 2ClO4-(aq) + PbCl2(s)
Net Ionic: Pb2+(aq) + 2Cl-(aq) → PbCl2(s)
Spectators: ClO4- and Na+
9. Molecular: _BaCl2(aq) + Na2SO4(aq) → 2NaCl(aq) + _BaSO4(s)
Total Ionic: Ba2+(aq) + 2Cl- (aq) + 2Na+ (aq) + SO42- (aq) → 2Na+ (aq) + 2Cl- (aq) + BaSO4(s)
Net Ionic: Ba2+(aq) + SO42-(aq) → BaSO4(s)
Spectators: Cl- and Na+
10. a) Molecular: _Ba(NO3)2(aq) + _K2SO4(aq) → 2KNO3(aq) + _BaSO4(s)
Total Ionic: Ba2+(aq) + 2NO3- (aq) + 2K+(aq) + SO42-(aq) → 2K+ (aq) + 2NO3-(aq) + BaSO4(s)
Net Ionic: Ba2+(aq) + SO42-(aq) → BaSO4(s)
Spectators: NO3- and K+
b) Mg(NO3)2(aq) + K2SO4(aq) → NR
c) CaCl2(aq) + Al(NO3)3(aq) → NR
d) NiCl2(aq) + NaBr(aq) → NR
e) Molecular: _Na2CO3(aq) + _MgBr2(aq) → 2NaBr(aq) + _MgCO3(s)
Total Ionic: 2Na+ (aq) + CO32-(aq) + Mg2+(aq) + 2Br -(aq) → 2Na+(aq) + 2Br -(aq) + MgCO3(s)
Net Ionic: Mg2+(aq) + CO32-(aq) → MgCO3(s)
Spectators: Na+ and Br 11.
(a)
(b)
(c)
SO42- + Ba2+ = BaSO4(s)
HSO3- + H+ = H2O + SO2(g)
CaO + 2H+ = Ca2+ + H2O
12.
(a)
(b)
(c)
Will not go
Will go [CO2(g) and H2O formed]
Will go [CH3COOAg(s) formed
Worksheet 12
3