Download SOLUBILITY RULES FOR IONIC COMPOUNDS IN WATER

EXTRA HOMEWORK 4A
1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not
necessary.
(a) Silver metal is added to acetic acid.
(b) Zinc metal is added to acetic acid.
(c) Beryllium metal is added to an aqueous solution of nickel (II) nitrate.
(d) Nickel metal is added to an aqueous solution of beryllium nitrate.
(e) Tungsten metal is added to water.
(f) Cesium metal is added to water.
(g) Crystals of iodine are added to an aqueous solution of ammonium bromide.
(h) Liquid bromine is added to an aqueous solution of ammonium iodide.
2. Write a balanced chemical equation for each of the following, each of which results in a reaction
occurring. For reactions occurring in water solution, write the balanced net ionic equation. Indicate
the phase of each reactant and product.
(a) Lithium metal is burned in nitrogen gas.
(b) A ribbon of beryllium metal is added to hydrochloric acid.
(c) Pellets of aluminum metal are added to a solution of copper (II) sulfate.
(d) Pieces of strontium metal are added to water.
(e) Liquid bromine is added to a solution of sodium iodide.
(f) Liquid hexane (C6H14) is burned in air.
(g) Liquid pentanol (C5H12O) is burned in air.
3. For reactions 1(b), 1(c), and 1(e), write the oxidation half reaction, the reduction half reaction, and
show how they add to make the overall net ionic equation
*4. (a) Solid calcium carbide (CaC2) is burned in air.
(b) Copper (II) sulfide is burned in an oxygen atmosphere
*5. Balance the following equation: CxHy + O2  CO2 + H2O
EXTRA HOMEWORK 4B
1. Write a balanced chemical equation for each of the following, each of which results in a reaction
occurring. Indicate the phase of each reactant and product.
(a) An electric current is passed through molten potassium iodide.
(b) Calcium chlorate is heated.
2. Give the oxidation numbers of all atoms in each of the following:
(a) O2
(b) P3-
(c) Hg22+
(d) Ni(NO3)2
(e) OF2
(f) C3H8O
(g) H3PO3
(h) C2O42-
*3. Give the oxidation numbers of all atoms in each of the following:
(a) C6H12O6
(b) KO2
(c) Fe3O4
EXTRA HOMEWORK 4C
1. Based upon the solubility rules, predict whether each of the following ionic compounds would be
soluble or insoluble in water:
(a) potassium chromate
(b) iron (III) acetate
(c) calcium bromide
(d) barium sulfate
(e) aluminum oxalate
(f) sodium phosphate
2. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not
necessary.
(a) Solutions of calcium acetate and ammonium carbonate are mixed.
(b) Solutions of barium nitrate and zinc chloride are mixed.
(c) Solutions of lithium hydroxide and sodium sulfate are mixed.
3. Write the balanced net ionic equation for each of the following, each of which results in a reaction
occurring. Indicate the phase of each reactant and product.
(a) Solutions of mercury (I) nitrate and hydrochloric acid are mixed.
(b) Solutions of sulfuric acid and potassium hydroxide are mixed.
(c) Solutions of lithium carbonate and hydrochloric acid are mixed.
(d) Solutions of potassium bisulfate and lithium hydroxide are mixed.
(continued on next page)
*3. A sample may contain any or all of the following ions: Hg22+, Ba2+ and Mn2+. No precipitate was
formed when an aqueous solution of NaCl or Na2SO4 was added to the sample solution, but a
precipitate formed when an aqueous solution of NaOH was added to the sample. What ion or ions
were present in the sample? Write net ionic equations for the formation of each of the precipitates.
*4. A sample may contain any or all of the following ions: Pb2+, Ca2+ and Cu2+. No precipitate formed
when an aqueous solution of NaCl was added. A white precipitate formed when an aqueous solution
of Na2SO4 was added. The precipitate was filtered off and an aqueous solution of Na2CO3 was added
to the remaining solution, forming a precipitate. What ion or ions were present in the sample? Write
net ionic equations for the formation of each of the precipitates.
*5. A sample may contain any or all of the following ions: Ag+, Ba2+ and Fe2+. A precipitate formed when
an aqueous solution of KCl was added. The precipitate was filtered off and an aqueous solution of
K2SO4 was added to the remaining solution, but no precipitate was formed. When an aqueous solution
of K2CO3 was added to the remaining solution, a precipitate formed. What ion or ions were present in
the sample? Write net ionic equations for the formation of each of the precipitates.
*6. Write the balanced net ionic equation for following, which results in a reaction occurring. Indicate the
phase of each reactant and product.
(a) A penny coated with copper (II) oxide is added to vinegar, which contains acetic acid.
EXTRA HOMEWORK 4D
1. For each of the following reactions, (1) specific whether it is an oxidation-reduction reaction or not,
and if it is, identify (2) the element oxidized, (3) the element reduced (4) the oxidizing agent, and (5)
the reducing agent:
(a) Ag+ + Cl-  AgCl
(b) NH4+ + OH-  NH3 + H2O
(c) 2ZnS + 3O2  2ZnO + 2SO2
(d) MgCO3  MgO + CO2
2. Predict the products of the following oxidation-reduction reactions, but do not balance:
(a) Acidified solutions of potassium dichromate and sodium iodide are mixed.
(b) Zinc metal is added to an acidified solution of potassium permanganate.
(c) A basic solution of potassium permanganate is mixed with a solution of sodium nitrite.
(d) Concentrated nitric acid is added to a solution of sodium oxalate.
(e) Acidified solutions of iron (II) sulfate and hydrogen peroxide are mixed.
*3. Predict the products of the following oxidation-reduction reactions, but do not balance:
(a) Solutions of iron (III) ions and antimony (III) ions are mixed.
(b) Mercury metal is added to a solution of mercury (II) nitrate.
EXTRA HOMEWORK 4E
1. Write the balanced net ionic equation for each of the following, each of which results in a reaction
occurring. Indicate the phase of each reactant and product.
(a) Solutions of sodium dichromate and nitrous acid are mixed.
(b) Concentrated nitric acid is added to a precipitate of iron (III) sulfide.
(c) Zinc metal is added to a basic solution of potassium permanganate.
(d) A solution of bismuth (III) nitrate is added to an acidified solution of hydrogen peroxide.
*2. Write the balanced net ionic equation for each of the following, each of which results in a reaction
occurring. Indicate the phase of each reactant and product.
(a) Iron filings are added to a solution of iron (III) ions.
(b) Antimony metal is added to a solution of antimony (V) fluoride
EXTRA REACTION HOMEWORK (OPTIONAL)
1. (a) Cesium metal is burned in chlorine gas.
(b) Aluminum metal and powdered sulfur are heated together.
(c) Barium metal is burned in oxygen.
2. (a) Mossy zinc is added to a solution of iron (III) nitrate.
(b) Strips of magnesium metal are added to sulfuric acid.
(c) Chlorine gas is added to a solution of magnesium bromide.
(d) A piece of cesium metal is added to water.
3. (a) Pentane, C5H12, is burned in air
(b) The alcohol in brandy (ethanol, C2H5OH) is ignited.
4. (a) Crystals of bismuth (III) oxide are heated.
(b) Solid cobalt (III) chlorate is heated.
(continued on next page)
5. (a) Solutions of potassium carbonate and magnesium nitrate are mixed.
(b) Solutions of lead (II) nitrate and sodium iodide are mixed.
(c) Solutions of iron (II) chloride and lithium hydroxide are mixed.
(d) Dilute sulfuric acid is added to a solution of strontium bromide.
(e) Hydrogen sulfide gas is bubbled through a solution of copper (II) chloride.
(f) Solutions of hydrofluoric acid and sodium hydroxide are mixed.
(g) Solutions of sodium bicarbonate and hydrofluoric acid are mixed.
(h) Solutions of sodium sulfide and hydrochloric acid are mixed.
6. (a) Solutions of ammonium sulfate and sodium hydroxide are mixed..
(b) Solutions of chlorous acid and ammonia are mixed.
(c) Solutions of potassium hydroxide and sodium bisulfate are mixed.
(d) Solutions of nitric acid and ammonia are mixed.
7. (a) An acidified solution of potassium permanganate is mixed with a magnesium bromide solution.
(b) Carbon monoxide gas is bubbled through a concentrated solution of nitric acid.
(c) An alkaline solution of potassium permanganate is added to a solution of sodium oxalate.
(d) An acidified solution of sodium dichromate is added to a solution of magnesium nitrite .
(e) An solution of hydrogen peroxide is added to an acidified solution of tin (II) nitrate.
(e) A water solution of chlorine undergoes autooxidation to hydrochloric acid and hypochlorous acid.
(continued on next page)
8. Write the balanced net ionic equation for each of the following, each of which results in a reaction
occurring. Indicate the phase of each reactant and product.
(a) An acidified solution of hydrogen peroxide is added to a solution of sodium iodide.
(b) Chlorine gas is passed over powdered aluminum.
(c) Solutons of mercury (I) nitrate and potassium sulfate are mixed.
(d) A strip of magnesium metal is added to a solution of silver nitrate.
(e) Solutions of lead (II) nitrate and sodium bromide are mixed.
(f) Silver metal is added to concentrated nitric acid.
(g) A solution of ammonium sulfate is added to a potassium hydroxide solution.
(h) Magnesium metal is burned in nitrogen gas.
(i) Solutions of zinc sulfate and sodium phosphate are mixed.
(j) A solution of potassium dichromate is added to an acidified solution of iron (II) sulfate.
(k) Solutions of lithium hydroxide and sodium bicarbonate are mixed.
(l) Solid barium metal is added to warm water.
(m) A solution of bismuth (III) nitrate is added to a solution of potassium sulfide.
(n) Solutions of ammonia and potassium bisulfate are mixed.
(o) Ethane gas (C2H6) is burned in air.
(p) Solutions of copper (II) sulfate and barium hydroxide are mixed.
(q) An acidified solution of potassium permanganate is mixed with a solution of lead (II) nitrate.
(r) Dilute sulfuric acid is mixed with a solution of strontium acetate.
(s) Liquid bromine is added to a solution of sodium iodide.
(t) Pieces of zinc metal are added to dilute acetic acid.
(u) An alkaline solution of potassium permanganate is mixed with a solution of sodium sulfite.
(v) Solid cobalt (III) chlorate is heated.
(w) Dilute sulfuric acid is added to a solution of lithium bicarbonate.
(x) Nickel (II) sulfide is burned in oxygen gas.
(y) Concentrated nitric acid is added to solid lithium nitride.
(z) Solutions of oxalic acid and sodium hydroxide are mixed.
() Concentrated hydrochloric acid is added to a precipitate of manganese (II) sulfide.
() A water solution of hydrogen peroxide undergoes autooxidation.
EXTRA HOMEWORK 4F
1. Complete the table for each of the following reactions:
(a)
O2 + 2F2  2OF2
0.40
P4 + 6H2  4PH3
(b)
0.60
0.00
initial moles
0.40
0.60
0.00
initial moles
____ ____
____
reacting moles
____
____
____
reacting moles
____ ____
____
final moles
____
____
____
final moles
2. hydrogen molecules and nitrogen molecules, shown in
the reaction chamber to the right, react to form
ammonia. Draw a picture of the chamber after the
reaction.
3. One of the few reactions that takes place between two solids at room temperature is:
Ba(OH)2.8H2O(s) + 2NH4SCN(s)  Ba(SCN)2(s) + 10H2O(l) + 4NH3(g)
If 6.5 g of barium hydroxide octahydrate will be used in the reaction, calculate
(a) the mass of ammonium thiocyanate that must react
(b) the mass of water that will be formed
(c) the mass of ammonia that will be formed
4. An electric furnace produces phosphorus by the following reaction:
Ca3(PO4)2(s) + 5C(s) + 3SiO2(s)  3CaSiO3(s) + 5CO(g) + 2P(l)
(a) Calculate the mass of phosphorus produced from the reaction of 1,500 g calcium phosphate, 250 g
carbon, and 1,100 g silicon dioxide.
(b) Which of the reactants is the limiting reagent?
(c) How many grams of each of the nonlimiting reagents remain after the reaction has ended?
*5. Commercial brass is an alloy of zinc and copper. When 5.065 g of brass is treated with hydrochloric,
0.0985 g of hydrogen gas is produced. Calculate the percentage by mass of zinc and copper in brass.
*6. An alloy is made of zinc and aluminum. When 3.476 g of the alloy is treated with hydrochloric acid,
0.2117 g of hydrogen gas is produced. Calculate the percentage by mass of zinc and aluminum in the
alloy.
EXTRA HOMEWORK 4G
1. A stock solution of nitric acid has a concentration of 12.0 M.
(a) To what volume should you dilute 50.0 mL of the stock nitric acid solution to obtain a 1.00 M
nitric acid solution?
(b) If 350. mL of the 1.00 M nitric acid solution is diluted to 4.500 L, what will be the molarity of
new nitric acid solution?
2. What volume of water must be added to 5.00 mL of a 6.00 M hydrochloric acid solution to make a
0.100 M hydrochloric acid solution?
3. A 75.0 mL sample of a 0.250 M hydrochloric acid solution is mixed with a 225.0 mL sample of a
0.0550 M barium hydroxide solution.
(a) Calculate the moles of each of the ions present in the solution before any reaction has occurred.
(b) Calculate the moles of each of the ions present in the solution after any reaction has occurred.
(c) Calculate the molarities of each of the ions present in the solution after any reaction has occurred.
*4. A 15.0 mL sample of a 0.300 M sodium carbonate solution is mixed with a 25.0 mL sample of a
0.200 M silver nitrate solution.
(a) Calculate the moles of each of the ions present in the solution before any reaction has occurred.
(b) Calculate the moles of each of the ions present in the solution after any reaction has occurred.
(c) Calculate the molarities of each of the ions present in the solution after any reaction has occurred.
(d) Calculate the mass of the precipitate formed from the reaction.
EXTRA HOMEWORK 4H
1. Tin (II) ions are oxidized by the permanganate ion in an acidic solution. Calculate the mass of tin (II)
ions that can be oxidized by 21.25 mL of a 0.1575 M permanganate ion solution.
2. A 0.6524 gram sample of oxalic acid dehydrate, H2C2O4.2H2O, is titrated to a phenolphthalein
endpoint with 23.35 mL of a sodium hydroxide solution. Calculate the molarity of the sodium
hydroxide solution.
3. A 0.125 g sample of a triprotic acid takes 15.15 mL of a 0.1050 M potassium hydroxide solution to
reach neutralization. Calculate the molar mass of the acid.
*4. An NaOH solution was standardized against potassium biphthalate, KHC8H4O4, (molar mass 204.22
g/mole). The volume of NaOH solution required to neutralize 1.7794 grams of potassium biphthalate
was 33.85 milliliters. A 0.5240 gram sample of a diprotic acid was dissolved in 25.00 mL of deionized
water. The solution was titrated with 45.22 milliliters of the NaOH solution.
(a) Calculate the molarity of the NaOH solution.
(b) Calculate the molar mass of the diprotic acid.
(c) The diprotic acid was found to be 2.24% hydrogen, 26.68% carbon, and 71.08% oxygen by mass.
Determine the molecular formula of the acid
EXTRA HOMEWORK 4I
1. Calculate the percent composition by mass of each element in C4H6O.
2. Calculate the number of phosphorus atoms present in 5.00 g of calcium phosphate.
3. A metal oxide with the formula M3O4 is 72.4% metal by mass. Calculate the molar mass of the metal.
*4. Hemoglobin, the protein that transports oxygen in mammals, is 0.342% iron by mass, and each
hemoglobin molecule contains four iron atoms. Calculate the molar mass of hemoglobin.
EXTRA HOMEWORK 4J
1. A compound contains only carbon and hydrogen. Combustion of the hydrocarbon produces 4.237
grams of carbon dioxide and 1.952 grams of water. If the molar mass of the compound is 120  10
g/mol, determine its empirical and molecular formulas.
2. A compound contains only carbon, hydrogen, and oxygen. Combustion of 0.750 grams of the
compound produces 1.118 grams of carbon dioxide and 0.343 grams of water. If the molar mass of the
compound is 120  10 g/mol, determine its empirical and molecular formulas.
3. Elemental analysis of an unknown pure substance indicates that the percent composition by mass is
36.93% carbon, 4.65% hydrogen, and 58.42% fluorine. A solution that is prepared by dissolving 2.477
grams of the substance in 25.00 grams of benzene, C6H6, has a freezing point of 1.60ºC. (The normal
freezing point of benzene is 5.50ºC and the molal freezing point constant, Kf, for benzene is 5.12
Cº/m.)
(a) Determine the empirical formula of the substance.
(b) Calculate the molar mass of the substance
(c) Determine the molecular formula of the substance
*4. A compound contains only carbon, hydrogen, and oxygen. Combustion of 0.257 grams of the
compound produces 0.665 grams of carbon dioxide and 0.136 grams of water. In another experiment,
4.73 grams of the compound is dissolved in 26.90 grams of ethyl ether, and the boiling point of the
solution was found to be 37.1ºC.
(a) Determine the empirical formula of the compound.
(b) Determine the molar mass of the compound.
(c) Determine the molecular formula of the compound.
*5. Water is added to 4.267 grams of uranium (VI) fluoride. The only products are 3.70 grams of a solid
containing only uranium, oxygen, and fluorine and 0.970 grams of a gas. The gas is 95.0% fluorine by
mass and the remainder is hydrogen.
(a) Determine the empirical formula of the gas.
(b) Determine the fraction of fluorine from the original compound that ended up in the solid and the
fraction of fluorine from the original compound that ended up in the gas after the reaction.
(c) Determine the empirical formula of the solid product.
(d) Write a balanced equation for the reaction between uranium (VI) fluoride and water. Assume the
empirical formula of the gas is the true molecular formula.
EXTRA 4A ANSWERS
1. (a) no
(b) yes
(c) yes
(d) no
(f) no
(g) yes
(h) no
(i) yes
2. (a) 6Li (s) + N2 (g)  2Li3N (s)
(b) Be (s) + 2H+ (aq)  Be2+ (aq) + H2 (g)
(c) 2Al (s) + 3Cu2+ (aq)  2Al3+ (aq) + 3Cu (s)
(d) Sr (s) + 2H2O (l)  Sr(OH)2 (s) + H2 (g)
(e) Br2 (l) + 2I- (aq)  2Br- (aq) + I2 (s)
(f) 2C6H14 (l) + 19O2 (g)  12CO2 (g) + 14H2O (g)
(g) 2C5H12O (l) + 15O2 (g)  10CO2 (g) + 12H2O (g)
3. (b)
Be (s) → Be2+ (aq) + 2e2H (aq) + 2e- → H2 (g)
____________________________________
+
Be (s) + 2H+ (aq)  Be2+ (aq) + H2 (g)
(c)
2Al (s) → 2Al3+ (aq) + 6e3Cu (aq) + 6e- → 3Cu (s)
________________________________________
2+
2Al (s) + 3Cu2+ (aq)  2Al3+ (aq) + 3Cu (s)
(e)
2I- (aq) → I2 (s) + 2eBr2 (l) + 2e- → 2Br- (aq)
____________________________________
Br2 (l) + 2I- (aq)  2Br- (aq) + I2 (s)
*4. (a) 2CaC2 (s) + 5O2 (g)  2CaO (s) + 4CO2 (g)
(b) 2CuS (s) + 3O2 (g)  2CuO (s) + 2SO2 (g)
*5. CxHy + (2x + y/2)O2  xCO2 + (y/2)H2O
EXTRA 4B ANSWERS
1. (a) 2KI (l)  2K (s) + I2 (s)
(b) Ca(ClO3)2 (s)  CaCl2 (s) + 3O2 (g)
(d) Cs2CO3 (s)  Cs2O (s) + CO2 (g)
(c) 2KOH (s)  K2O (s) + H2O (g)
2. (a) O = 0
(b) P = -3
(c) Hg = +1
(d) Ni = +2, N = +5, O = -2
(e) O = +2, F = -1
(f) C = -2, H = +1, O = -2
(g) H = +1, P = +3, O = -2
(h) C = +3, O = -2
*3. (a) C = 0, H = +1, O = -2
(b) K = +1, O = -½
(c) Fe = +22/3 ,O = -2
EXTRA 4C ANSWERS
1. (a) soluble
(b) soluble
(c) soluble
(d) insoluble
(e) insoluble
(f) soluble
2. (a) yes
(b) no
(c) no
+
3. (a) Hg22 (aq) + 2Cl- (aq)  Hg2Cl2 (s)
(b) H+ (aq) + OH- (aq)  H2O (l)
(c) CO32- (aq) + 2H+ (aq)  H2O (l) + CO2 (g)
(d) HSO4- (aq) + OH- (aq)  SO42- (aq) + H2O (l)
*3. Mn2+
Mn2+ (aq) + 2OH- (aq)  Mn(OH)2 (s)
*4. Ca2+
Ca2+ (aq) + SO42- (aq)  CaSO4 (s)
Cu2+
*5. Ag+
Fe2+
Cu2+ (aq) + CO32- (aq)  CuCO3 (s)
Ag+ (aq) + Cl- (aq)  AgCl (s)
Fe2+ (aq) + CO32- (aq)  FeCO3 (s)
*6. (a) CuO (s) + 2HC2H3O2 (aq)  Cu2+ (aq) + 2C2H3O2- (aq) + H2O (l)
EXTRA 4D ANSWERS
1. (a) not oxidation-reduction
(b) not oxidation-reduction
(c) oxidation-reduction
oxidized: S
reduced: O
oxidizing agent: O2
reducing agent: ZnS
(d) not oxidation-reduction
2. (a) Cr2O72- (aq) + I- (aq)  Cr3+ (aq) + I2 (s)
(b) MnO4- (aq) + Zn (s)  Mn2+ (aq) + Zn2+ (aq)
(c) MnO4- (aq) + NO2- (aq)  MnO2 (s) + NO3- (aq)
(d) NO3- (aq) + C2O42- (aq)  NO2 (g) + CO2 (g)
(e) Fe2+ (aq) + H2O2 (aq)  Fe3+ (aq) + H2O (l)
*3. (a) Fe3+ (aq) + Sb3+ (aq)  Fe2+ (aq) + Sb5+ (aq)
(b) Hg (s) +
Hg2+
(aq)  Hg2
2+
(aq)
(unbalanced)
(unbalanced)
EXTRA 4E ANSWERS
1. (a) 5H+ (aq) + Cr2O72- (aq) + 3HNO2 (aq)  2Cr3+ (aq) + 3NO3- (aq) + 4H2O (l)
(b) 96H+ (aq) + 48NO3- (aq) + 8Fe2S3 (s)  3S8 (s) + 48NO2 (g) + 16Fe3+ (aq) + 48H2O (l)
(c) 4H2O (l) + 2MnO4- (aq) + 3Zn (s)  2MnO2 (s) + 3Zn(OH)2 (s) + 2OH- (aq)
(d) 2H+ (aq) + Bi3+ (aq) + H2O2 (aq)  Bi5+ (aq) + 2H2O (l)
*2. (a) Fe (s) + 2Fe3+ (aq)  3Fe2+ (aq)
(b) 2Sb (s) + 3Sb5+ (aq)  5Sb3+ (aq)
EXTRA REACTION ANSWERS
1. (a) 2Cs (s) + Cl2 (g)  2CsCl (s)
(b) 16Al (s) + 3S8 (s)  8Al2S3 (s)
(c) 2Ba (s) + O2 (g)  2BaO (s)
2. (a) 3Zn (s) + 2Fe3+ (aq)  3Zn2+ (aq) + 2Fe (s)
(b) Mg (s) + 2H+ (aq)  Mg2+ (aq) + H2 (g)
(c) Cl2 (g) + 2Br- (aq)  2Cl- (aq) + Br2 (l)
(d) 2Cs (s) + 2H2O (l)  2Cs+ (aq) + 2OH- (aq) + H2 (g)
3. (a) C5H12 (s) + 8O2 (g)  5CO2 (g) + 6H2O (g)
(b) C2H5OH (aq) + 3O2 (g)  2CO2 (g) + 3H2O (g)
4. (a) 2Bi2O3 (s)  4Bi (s) + 3O2 (g)
(b) 2Co(ClO3)3 (s)  2CoCl3 (s) + 9O2 (g)
5. (a) CO32- (aq) + Mg2+ (aq)  MgCO3 (s)
(b) Pb2+ (aq) + 2I- (aq)  PbI2 (s)
(c) Fe2+ (aq) + 2OH- (aq)  Fe(OH)2 (s)
(d) SO42- (aq) + Sr2+ (aq)  SrSO4 (s)
(e) H2S (g) + Cu2+ (aq)  2H+ (aq) + CuS (s)
(f) HF (aq) + OH- (aq)  F- (aq) + H2O (l)
(g) HCO3- (aq) + HF (aq)  F- (aq) + H2O (l) + CO2 (g)
(h) S2- (aq) + 2H+ (aq)  H2S (g)
6. (a) NH4+ (aq) + OH- (aq)  NH3 (g) + H2O (l)
(b) HClO2 (aq) + NH3 (aq)  NH4+ (aq) + ClO2- (aq)
(c) OH- (aq) + HSO4- (aq) +  H2O (l) + SO42- (aq)
(d) H+ (aq) + NH3 (aq) +  NH4+ (aq)
(continued on next page)
7. (a) 16H+ (aq) + 2MnO4- (aq) + 10Br- (aq)  2Mn2+ (aq) + 5Br2 (l) + 8H2O (l)
(d) CO (g) + 2H+ (aq) + 2NO3- (aq)  CO2 (g) + 2NO2 (g) + H2O (l)
(c) 4H2O (l) + 2MnO4- (aq) + 3C2O42- (aq)  2MnO2 (s) + 6CO2 (g) + 8OH- (aq)
(d) 8H+ (aq) + Cr2O72- (aq) + 3NO2- (aq)  2Cr3+ (aq) + 3NO3- (aq) + 4H2O (l)
(e) 2H+ (aq) + Sn2+ (aq) + H2O2 (aq)  Sn4+ (aq) + 2H2O (l)
(f) Cl2 (aq) + H2O (l)  Cl- (aq) + HClO (aq) + H+ (aq)
8. (a) 2H+ (aq) + H2O2 (aq) + 2I- (aq)  2H2O (l) + I2 (s)
(b) 3Cl2 (g) + 2Al (s)  2AlCl3 (s)
(c) Hg22+ (aq) + SO42- (aq)  Hg2SO4 (s)
(d) Mg (s) + 2Ag+ (aq)  Mg2+ (aq) + 2Ag (s)
(e) Pb2+ (aq) + 2Br- (aq)  PbBr2 (s)
(f) Ag (s) + 2H+ (aq) + NO3- (aq)  Ag+ (aq) + NO2 (g) + H2O (l)
(g) NH4+ (aq) + OH- (aq)  NH3 (g) + H2O (l)
(h) 3Mg (s) + N2 (g)  Mg3N2 (s)
(i) 3Zn2+ (aq) + 2PO43- (aq)  Zn3(PO4)2 (s)
(j) 14H+ (aq) + Cr2O72- (aq) + 6Fe2+ (aq)  2Cr3+ (aq) + 6Fe3+ (aq) + 7H2O (l)
(k) OH- (aq) + HCO3- (aq)  H2O (l) + CO32- (aq)
(l) Ba (s) + 2H2O (l)  Ba(OH)2 (s) + H2 (g)
(m) 2Bi3+ (aq) + 3S2- (aq)  Bi2S3 (s)
(n) NH3 (aq) + HSO4- (aq)  NH4+ (aq) + SO42- (aq)
(o) 2C2H6 (g) + 7O2 (g)  4CO2 (g) + 6H2O (g)
(p) Cu2+ (aq) + SO42- (aq) + Ba2+ (aq) + 2OH- (aq)  Cu(OH)2 (s) + BaSO4 (s)
(q) 16H+ (aq) + 2MnO4- (aq) + 5Pb2+ (aq)  2Mn2+ (aq) + 5Pb4+ (aq) + 8H2O (l)
(r) 2H+ (aq) SO42- (aq) + Sr2+ (aq) + 2C2H3O2- (aq)  2HC2H3O2 (aq) + SrSO4 (s)
(s) Br2 (l) + 2I- (aq)  2Br- (aq) + I2 (s)
(t) Zn (s) + 2HC2H3O2 (aq)  Zn2+ (aq) + 2C2H3O2- (aq) + H2 (g)
(u) H2O (l) + 2MnO4- (aq) + 3SO32- (aq)  2MnO2 (s) + 3SO42- (aq) + 2OH- (aq)
(v) 2Co(ClO3)3 (s)  2CoCl3 (s) + 9O2 (g)
(w) H+ (aq) + HCO3- (aq)  H2O (l) + CO2 (g)
(x) 2NiS (s) + 3O2 (g)  2NiO (s) + 2SO2 (g)
(y) 12H+ (aq) + 6NO3- (aq) + 2Li3N (s)  N2 (g) + 6NO2 (g) + 6Li+ (aq) + 6H2O (l)
(z) H2C2O4 (aq) + 2OH- (aq)  C2O42- (aq) + 2H2O (l)
() 2H+ (aq) + MnS (s)  H2S (g) + Mn2+ (aq)
() 2H2O2 (aq)  2H2O (l) + O2 (g)
EXTRA 4F ANSWERS
O2 + 2F2  2OF2
1. (a)
0.40
0.60
0.00
-0.30
-0.60
+0.60
0.10
0.00
0.60
P4 + 6H2  4PH3
(b)
initial moles
reacting moles
0.40
0.60
0.00
-0.10
-0.60
+0.40
0.30
0.00
0.40
final moles
2.
3. (a) 3.1 g NH4SCN
(b) 3.7 g H2O
(c) 1.4 g NH3
4. (a) 2.6 x 102 g P
(b) C
(c) 2.1 x 102 g Ca3(PO4)2, 3.5 x 102 g SiO2
*5. 63.0% Zn, 37.0% Cu
*6. 63.0% Zn, 37.0% Al
EXTRA 4G ANSWERS
1. (a) 600. mL
(b) 0.0778 M
2. 295 mL
3. (a) 0.0188 mol H+, 0.0188 mol Cl-, 0.0124 mol Ba2+, 0.0248 mol OH(b) 0.0188 mol Cl-, 0.0124 mol Ba2+, 0.0060 mol OH(c) 0.0625 M Cl-, 0.0413 M Ba2+, 0.020 M OH*4. (a) 0.00900 mol Na+, 0.00450 mol CO32-, 0.00500 mol Ag+, 0.00500 mol NO3(b) 0.00900 mol Na+, 0.00200 mol CO32-, 0.00500 mol NO3(c) 0.225 M Na+, 0.0500 M CO32-, 0.125 M NO3(d) 0.689 g
initial moles
reacting moles
final moles
EXTRA 4H ANSWERS
1. 0.9932 g Sn2+
2. 0.4432 M NaOH
3. 236 g/mol
*4. (a) 0.2574 M NaOH
(b) 90.04 g/mol
(c) H2C2O4
EXTRA 4I ANSWERS
1. 68.53% C, 8.64% H, 22.82% O
2. 1.94 x 1022 atoms P
3. 56.0 g/mol
*4. 65,300 g/mol
EXTRA 4J ANSWERS
1. C8H18
2. C4H6O4
3. (a) C2H3F2
(b) 130. g/mol
(c) C4H6F4
*4. (a) C4H4O
(b) 140 g/mol
(c) C8H8O2
*5. (a) HF
(b) 33.2% in the solid, 66.8% in the gas
(c) UO2F2
(d) UF6 + 2H2O  4HF + UO2F2