Download Basic Chemical Concepts I

Chem 1050
Core Chemical Concepts I
Chemical calculations:
especially basic stoichiometry, limiting reagents, gravimetric
analysis, empirical and molecular formulas
writing balanced equations and predicting products
Chemical reactions:
Important:
The suggested text problems and the additional problems (which are
organized by topic) are intended to be a guide to bring you up to the
required competency for this course. You should do some problems in all
areas indicated and concentrate on topics which you have forgotten or
have not already encountered.
Text: PetrucciCHarwoodCHerring 8th Edition
Chapter 1
Chapter 2
Exercises: 63,67,71
Review Questions: 21
Exercises: 47, 55, 65, 69
Chapter 3
Review Questions: 14-16, 19
Exercises: 49, 51, 53, 55, 61, 65
Chapter 4
Review Questions: 9, 10, 12, 16-24
Exercises: 25, 27, 33, 37, 39, 45, 49, 53, 65, 69
Chapter 5
Review Questions: 5, 7, 9-19, 26
Exercises: 35, 37, 41, 49, 51, 53, 55, 59, 61, 63, 71, 73, 75
Additional problems:
Calculations involving moles, Avogadro's number, density, mass percent.
I
Calculate the mass of 5.58 x 1022 formula units of NaCl.
II.
The density of ice is 0.917 g mL–1 at 0ºC and 101.3 kPa of pressure. Calculate
the volume occupied by 1.000 kg of ice under these conditions.
III.
An aqueous solution is 15.0% NaCl by mass and has a density of 1.15 g mL–1.
(a)
(b)
Calculate the mass in grams of 300.0 mL of this solution.
Calculate the mass of NaCl present in 300.0 mL of this solution.
1
Calculations involving solutions, solution preparation and dilution.
1.
Calculate the molar concentration of the solute in the following solutions:
(a) 12.42 g of HCl dissolved in enough H2O to make 250.0 mL of solution
(b) 3.618 g of Cd(NO3)2 dissolved in enough H2O to make 2.000 L of solution.
2.
Calculate the mass of Kl required to make 50.00 mL of 0.08000 mol L–1 Kl(aq).
3.
Calculate the volume (in mL) of 0.2002 mol L–1 KMnO4(aq) which contains
7.140 g of KMnO4.
4.
How many milliliters of 6.00 mol L–1 HNO3 (aq) are required to make 500.0 mL
of 0.255 mol L–1 HNO3(aq)?
5.
A student wishes to dilute 3.0 mL of 2 mol L–1 NaOH(aq) to a concentration of
0.1 mol L–1. Calculate the final volume of solution required.
6.
A student adds 100.0 mL of 0.800 mol L–1 NaCl(aq) to 400.0 mL of 0.800
mol L–1 KBr(aq). Calculate the molar concentrations of NaCl and KBr in the
combined solution.
Percent composition, empirical and molecular formulas.
7.
Calculate the % by mass of oxygen (to 4 significant figures) in the following
compounds:
(a) K4P2O7
(b) Be(NO3)2·4H2O
8.
Carboranes are a class of compounds composed of carbon, boron and
hydrogen. One carborane is found to contain 32.77% C and 59.00% B by mass.
Determine its empirical formula.
9.
Ethyl butyrate, a compound containing carbon, hydrogen and oxygen is
responsible for the characteristic odor of pineapples. Determine the empirical
formula of ethyl butyrate if combustion of 2.78 g of ethyl butyrate produced 6.32
g CO2 and 2.58 g H2O. Find its molecular formula if its molar mass has been
determined to be 116.2 g molG1.
10.
When a 6.20 g sample of a compound containing only carbon, hydrogen and
sulfur reacted with an excess of Cl2, 16.7 g of HCl and 26.4 g of CCl4 were
obtained. Determine the empirical formula of the compound.
11.
A 6.00 g sample of cobalt metal is completely consumed in a stream of oxygen
producing 8.17 g of compound. Determine the empirical formula of the cobaltoxygen compound formed.
2
Balancing equations.
12.
Balance the following equations by inspection (pp 108 - 110 in text):
(a)
CuO(s) + NH3(aq) → Cu(s) + H2O(l) + N2(g)
(b)
C4H6O2(s) + O2(g) → CO2(g) + H2O(l)
(c)
CaS(aq) + Bi(NO3)3(aq) → Ca(NO3)2(aq) + Bi2S3(s)
(d)
La2O3(s) + H2O(l) → La(OH)3(s)
(e)
Ca(OH)2(aq) + HBr(aq) → CaBr2(aq) + H2O(l)
(f)
Zn(BrO3)2(s) → ZnO(s) + Br2(l) + O2(g)
(g)
C3H5NO(s) + O2(g) → CO2(g) + H2O(g)+ NO2(g)
(h)
P4O6(s) + H2O(l) → H3PO3(aq)
(i)
Ag+(aq) + Al(s) → Ag(s) + Al3+ (aq)
Basic stoichiometry problems.
13.
14.
Given the following equation for the combustion of ammonia with oxygen at high
temperatures: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
(a)
If 75.4 g of ammonia are consumed, calculate the minimum mass of oxygen
required and the maximum masses of NO and H2 that can be formed.
(b)
If 338 g of H2O are formed, calculate the maximum mass of NO formed and
the minimum masses of ammonia and oxygen which must be consumed.
Given the following equation representing the reaction of copper(II)oxide with
ammonia:
3 CuO(s) + 2NH3(g) → 3 Cu(s) + N2(g)+ 3 H2O(g)
Determine the percentage yield of copper metal if 48.34 g of copper are collected
from the reaction of 9.44 g of ammonia with an excess of copper(II)oxide.
15.
Given: 2 AgNO3(aq) + Na2S(aq) → Ag2S(s) + 2NaNO3(aq)
Calculate the mass of Ag2S(s) formed when 35.0 mL of 0.200 mol L–1 AgNO3(aq)
are treated with an excess of sodium sulfide solution.
3
Limiting reagent problems.
16.
Potassium nitrate, KNO3, sometimes called saltpeter, is an important fertiliser.
One process for its manufacture is the following reaction, carried out at elevated
temperatures:
3 KCl(s) + 4 HNO3(l) → Cl2(g) + NOCl(g) + 2 H2O(g) + 3 KNO3(s)
(a)
Determine the limiting reagent when 101.0 g of both reactants are mixed.
Justify your answer.
(b)
Assuming the limiting reagent is totally consumed, calculate the mass of
the excess reagent which remains unreacted.
(c)
Calculate the maximum mass of KNO3 that can be formed.
Given: 3 Cu(s) + 8 HNO3(l) → 3 Cu(NO3)2(aq) + 8 H2O(l) + 2 NO(g)
17.
18.
(a)
If 8.41 g of Cu(s) are added to 150.0 mL of 2.00 mol L–1 HNO3(aq),
calculate the maximum amount in grams of NO(g) that can be formed.
(b)
If 2.04 g of NO(g) are actually collected, calculate the % yield of NO(g).
Manganese can be isolated from MnO2 by the thermite reaction, in which the
oxide reacts with aluminum metal forming Mn and A12O3 and liberating a large
amount of heat. A mixture of 227g of MnO2 and 73.4g of Al is allowed to react to
completion. Calculate the actual yield of Mn if the % yield of the reaction is 75.0
%.
3 MnO2(s) + 4 Al(s) → 3 Mn(s) + 2 Al2O3(s)
Gravimetric analysis.
19.
20.
A 4.270 g sample of an unknown metal bromide XBr3 was dissolved in water and
treated with excess AgNO3. If 8.140 g of AgBr were recovered,
(a)
Calculate the number of moles of AgBr formed.
(b)
Calculate the number of moles of XBr3 reacted.
(c)
Calculate the molar mass of XBr3.
(d)
Calculate the molar mass of element X.
(e)
Identify element X.
A 3.500 g sample of a compound of cobalt and iodine was dissolved in water
and treated with excess AgNO3 solution producing 5.255 g of Agl precipitate.
Determine the empirical formula of the compound.
4
21.
A 2.714 g sample of the hydrated salt, CuSO4·XH2O was dissolved in water and
treated with excess Ba(NO3)2 solution producing 2.537 g of BaSO4 precipitate.
Determine the value of X in the formula CuSO4·XH2O.
Acid/base neutralization stoichiometry problems.
22.
A 20.17 mL aliquot of 0.3036 mol L–1 NaOH(aq) completely neutralizes 25.00 mL
of H2SO4(aq). Calculate the molar concentration of the H2SO4(aq). Hint: Write
a balanced equation for the reaction.
23.
Vitamin C, ascorbic acid, H2C6H6O6, (a weak diprotic acid), can be taken orally in
tablet form where it is the main ingredient. A vitamin C tablet with a mass of
0.4902 g is dissolved in sufficient deionized H2O and neutralized by 20.14 mL of
0.2742 mol L–1 NaOH(aq). The neutralization reaction can be represented as
follows:
H2C6H6O6(aq) + 2 NaOH(aq) → Na2C6H6O6(aq) + 2 H2O(l)
24.
(a)
Calculate the mass of pure ascorbic acid which reacted.
(b)
Calculate the % by mass of ascorbic acid (i.e. % purity) in the vitamin C
tablet.
The active ingredient in common aspirin is acetylsalicylic acid (ASA), a weak
monoprotic acid with the formula HC9H7O4. The aspirin contains ASA and an
non!medicinal binder. A 0.8621g tablet is dissolved in sufficient deionized H2O
and then neutralized by 32.05 mL of 0.07070 mol L–1 Ba(OH)2(aq) according to
the following equation:
2 HC9H7O4 (aq) + Ba(OH)2(aq) → Ba(C9H7O4)2(aq) + 2 H2O(l)
Calculate the mass percent of acetylsalicylic acid in the tablet.
25.
Calculate the volume in milliliters of 0.3450 mol L–1 KOH(aq) required for the
complete neutralization of 38.55 mL of 0.1275 mol L–1 H3PO4(aq). Hint: Write a
balanced equation for the reaction.
Strong electrolytes.
26.
A 2.56 g sample of Na2SO4·10H2O is dissolved in enough water to make 250.0
mL of solution. Calculate the molar concentrations of Na+(aq) and SO42– (aq) in
the solution.
27.
A solution is made by dissolving 0.800 g of NaCl and 1.60 g of CaCl2 in enough
water to make 100.0 mL of solution. Calculate the molar concentration of
chloride ion (Cl–) in the solution.
28.
A 10.00 mL volume of 0.160 M Al2(SO4)3(aq) is mixed with a 15.00 mL volume of
5
0.320 M Na2SO4(aq). Determine the concentration of all three ions in the final
solution.
Miscellaneous problems.
29.
A 10.00 mL aliquot of vinegar (density = 1.02 g mLG1) is diluted to 100.0 mL with
deionized water in a volumetric flask. A 25.00 mL sample of the diluted vinegar
requires 9.10 mL of 0.2218 M NaOH(aq) to reach a pink phenolphthalein end
point. Calculate the mass % of acetic acid, HC2H3O2, in the undiluted vinegar.
30.
An iron carbonyl, Fe3(CO)X, is 33.26% Fe by mass. Determine the value of x for
in the formula.
31.
An ionic compound, KBrOx, where x is unknown, is analysed and found to
contain 52.92% bromine by mass. Determine the value of x and name the
compound.
32.
A compound of metal M and oxygen has the empirical formula M3O4 and is
72.36% M by mass. Calculate the molar mass of metal M and hence determine
its identity.
33.
If 34.2 g of Ca(NO3)2·4H2O is dissolved in water and reacted with excess
Na3PO4(aq), what mass of Ca3(PO4)2 will be produced given the following net
ionic equation?
3 Ca2+ (aq) + 2 PO43-(aq) → Ca3(PO4)2(s)
34.
Potassium dichromate can be prepared by reacting chromium(III)chloride
hexahydrate with hydrogen peroxide under basic conditions. When 8.00 g of
chromium(III) chloride hexahydrate reacts with 9.022 g of KOH and 10.0 mL of
6.00 mol L–1 H2O2(aq), 2.77 g of potassium dichromate is recovered. Calculate
the percentage yield of potassium dichromate. The net ionic equation for the
reaction is:
2 Cr+3 (aq) + 3 H2O2(aq) + 8 OH–(aq) → Cr2O72– (aq) + 7 H2O(l)
35.
An 8.000 g sample of a compound containing carbon, hydrogen, and nitrogen
was burned in excess oxygen gas producing 15.83 g of carbon dioxide and
5.835 g of water. Determine the empirical formula of the compound.
6
36.
A crucible containing some limestone, CaCO3, has a total mass of 27.133 g.
The crucible is heated to decompose all the limestone according to the following
equation:
heat
CaCO3(s)  
→ CaO(s) + CO2(g)
After the decomposition was complete, the crucible was cooled to room
temperature and reweighed giving a mass of the crucible and its contents of
26.847 g. Calculate the mass of the crucible.
37.
An element X forms an iodide Xl3 and a chloride XCl3. The iodide is
quantitatively converted to the chloride when it is heated in a stream of chlorine:
2 Xl3 + 3 Cl2 6 2 XCl3 + 3 I2
If 0.5000 g of Xl3 is treated, 0.2360 g of XCl3 is obtained.
38.
(a)
Calculate the molar mass of element X
(b)
Identify element X.
A mixture containing KClO3, KHCO3, K2CO3, and KCl was heated strongly,
producing CO2, O2, and H2O gases according to the following equations:
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
2 KHCO3(s) → K2O(s) + 2 CO2(g) + H2O(g)
K2CO3(s) → K2O(s) + CO2(g)
The KCl is very stable and does not decompose under the conditions of the
experiment. If 100.0 g of the mixture produces 1.80 g of H2O, 13.20 g of CO2,
and 4.00 g of O2, calculate the mass percent of KCl in the mixture.
39.
A 25.00 mL aliquot of a mixture containing 0.03068 M HCl(aq) and an unknown
concentration of H2SO4(aq) requires 27.54 mL of 0.1107 M NaOH(aq) to
completely neutralize the acid mixture. Calculate the concentration of the H2SO4
in the mixture in mol LG1.
40.
A 1.9791 g sample of MnCl2·XH2O was heated to drive off the water of
hydration, leaving 1.2584 g of solid residue. Determine the value of X in the
formula of the hydrate.
41.
Calculate the [Na+] in a solution made by mixing 50.0 mL of 0.200 mol L–1
Na2SO4(aq) with 200.0 mL of 0.100 mol L–1 Na3PO4(aq).
7
42.
A 25.00 mL sample of HCl(aq) was added to a 0.1000 g sample of CaCO3. All
the CaCO3 reacted, leaving some unreacted HCl(aq).
CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + H2O + CO2(g)
The unreacted HCl(aq) required 43.82 mL of 0.01185 M Ba(OH)2(aq) to
complete the following reaction.
2 HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2 H2O(l)
Calculate the molar concentration of the original HCl(aq).
43.
The reaction below can be used as a laboratory method of preparing small
quantities of Cl2(g). When a 62.6 g sample that is 98.5% K2Cr2O7 by mass is
allowed to react with 325 mL of HCl(aq) with a density of 1.15 g mLG1 and 30.1%
HCl by mass, 38.9 grams of Cl2(g) are produced. Calculate the % yield of
chlorine gas.
K2Cr2O7 (aq) + 14 HCl (aq) → 2 CrCl3(aq) + 3 Cl2(g) + 7 H2O(l) + 2 KCl(aq)
44.
Zn can reduce NO3– to NH3(g) in basic solution as shown below:
NO3–(aq) + 4 Zn(s) + 7 OH–(aq) + 6 H2O(l) → 4 [Zn(OH)4]2– (aq) + NH3(g)
The gaseous NH3 is driven out of the reaction vessel into a second flask where it
is neutralized with an excess of HCl(aq). Then, the unreacted HCl can be
titrated with NaOH. In this way a quantitative determination of NO3– can be
achieved. A 25.00 mL sample of nitrate solution was treated with zinc in basic
solution. The NH3(g) was passed into 50.00 mL of 0.1500 M HCl(aq). The
unreacted HCl required 32.10 mL of 0.1000 M NaOH for its titration. What was
the [NO3–] in the original sample? Hint: Write balanced equations for the
reaction of NH3(aq) with HCl(aq) and HCl(aq) with NaOH(aq).
45.
(a)
(b)
46.
Determine the empirical formula of an acid which had the following
elemental composition by mass: Carbon - 48.64%, Hydrogen - 8.16%,
Oxygen !43.19%.
The acid in (a) is monobasic (has one ionizable hydrogen) and hence can
be given the formula HX. A 8.558 g sample of the acid was dissolved in
water to produce a total volume of 1000.0 mL. A 25.00 mL aliquot of the
acid solution required 28.88 mL of 0.1000 mol L–1 aqueous sodium
hydroxide to react with all the acid. Determine the molecular formula of
the acid.
The molar concentration of nitric acid, HNO3, in a sample of concentrated nitric
acid is to be determined.
(a)
Initially, a NaOH solution was standardized by titration with a sample of
potassium hydrogen phthalate, KHC8H4O4, a monoprotic acid (HX) often
used as a primary standard. A sample of pure KHC8H4O4 weighing 1.518
8
grams was dissolved in water and titrated with NaOH solution. To reach
the equivalence point, 26.90 milliliters of base was required. Calculate
the molarity of the NaOH solution. (Molecular weight: KHC8H4O4 = 204.2
g molG1).
HC8H4O4G(aq) + OHG(aq) → C8H4O42G(aq) + H2O(l)
(b)
A 10.00 milliliter sample of the concentrated nitric acid was diluted with
water to a total volume of 500.0 milliliters. Then 25.00 milliliters of the
diluted acid solution was titrated with the standardized NaOH solution
prepared in part (a). The equivalence point was reached after 28.35
milliliters of the base had been added. Calculate the molarity of the
concentrated nitric acid.
47.
A hydrated nickel salt is 23.8% Ni, 13.0% S, 58.3% O and 4.9% H by mass. If
its molar mass is 246.9 g mol–1, determine the formula of the hydrated salt.
48.
A 2.500 g sample of a compound of lithium, chlorine and oxygen is heated for an
extended period to drive off the oxygen. The residue weighs 1.170 g. It is now
dissolved in water and treated with silver nitrate. All of the chloride precipitates
as AgCl, which weighs 3.963 g. Calculate the empirical formula of the lithiumchlorine-oxygen compound.
49.
When M2S3(s) is heated in air, it is converted to MO2(s) and SO2(g). A 4.000 g
sample of M2S3(s) is heated in air producing 3.732 g of MO2(s). Calculate the
molar mass of M and identify it. Hint: Write a balanced equation for the
reaction.
50.
An electric furnace produces phosphorus by the following reaction:
2 Ca3(PO4)2(s) + 10 C(s) + 6 SiO2(s) → 6 CaSiO3(s) + 10 CO(g) + P4(g)
An initial reaction mixture containing 750.0 kg calcium phosphate, 125.0 kg
carbon and 500.0 kg silicon dioxide. If 95.8 kg of phosphorus is recovered,
calculate the % yield of phosphorus.
51.
Predict whether or not a precipitate will form when the following aqueous
solutions are mixed using your knowledge of the solubility rules. Write balanced
molecular (whole formula) equations for all reactions which yield a precipitate.
(a)
AgNO3(aq) + CaCl2(aq)
(b)
Na2S(aq) + Mg(C2H3O2)2(aq)
(c)
CuSO4(aq) + Fe(NO3)3(aq)
(d)
Na2SO4(aq) + BaBr2(aq)
9
52.
(e)
Pb(NO3)2(aq) + HI(aq)
(f)
CrCl3(aq) + NaOH(aq)
(g)
NH4NO3(aq) + Na3PO4(aq)
(h)
Hg2(NO3)2(aq) + NaCl(aq)
(i)
K2S(aq) + NiCl2(aq)
(j)
Ca(NO3)2(aq) + K2CO3(aq)
(k)
Co(C2H3O2)2(aq) + FeCl2(aq)
(l)
CaI2(aq) + (NH4)3PO4(aq)
Given the following word equations, write molecular (whole-formula form),
total ionic (ionic form) and net ionic equations for each:
(a)
Aluminum metal is added to a solution of nitric acid yielding hydrogen gas
and a solution of aluminum nitrate.
(b)
Aqueous solutions of ammonium phosphate and iron(II) chloride are
mixed yielding a precipitate of iron(II) phosphate and aqueous ammonium
chloride.
(c)
Magnesium metal is added to a solution of silver nitrate.
(d)
The addition of hydrochloric acid to solid sodium carbonate decahydrate.
(e)
The complete neutralization of nitric acid by aqueous barium hydroxide.
(f)
Chlorine water is added to aqueous potassium bromide.
(g)
The complete neutralization of acetic acid by aqueous sodium hydroxide.
(h)
The complete neutralization of aqueous ammonia by aqueous nitric acid.
Answers:
I
II
III
1.
2.
3.
4.
5.
mass NaCl = 5.71 g
1.09 x 103 mL
(a)
345 g solution, mass NaCl = 51.8 g
[HCl] = 1.362 mol LG1, [Cd(NO3)2 = 7.650 x 10-3 mol L–1
0.6640g KI
225.7 mL
21.3 mL
60 mL
10
6.
7.
8.
9.
10.
11.
12.
[NaCl] = 0.160 mol L–1, [KBr] = 0.640 mol L–1
(a) 33.90% (b) 78.01%
B2CH3
EF = C3H6O MF = C6H12O2
C3H8S2
Co3O4
Coefficients of reactants (R) and products (P) are given below:
(a)
3 R1 + 2 R2 6 3 P1 + 3 P2 + P3
(b)
2 R1 + 9 R2 6 8 P1 + 6 P2
(c)
3 R1 + 2 R2 6 3 P1 + P2
(d)
R1 + 3 R2 6 2 P1
(e)
R1 + 2 R2 6 P1 + 2 P2
(f)
2 R1 6 2 P1 + 2 P2 + P3
(g)
4 R1 + 19 R2 6 12 P1 + 10 P2 + 4 P3
(h)
R1 + 6 R2 6 4 P1
(i)
3R1 + R2 6 3 Pl + P2
13.
14.
15.
16.
17.
18.
19.
(a)
177 g O2, 133 g NO, 120 g H2O (b)
375g NO, 213g NH3, 502 g O2
91.5% yield
0.868 g Ag2S
(a)
HNO3 is LR (b)
11.4g KCl
(c)
121.5 g KNO3
(a)
2.25 g NO (b)
90.6% yield
84.1 g Mn
(a)
n(AgBr) 0.04335 mol
(b) n(XBr3) 0.01445 mol
(c)
molar mass of XBr3 295.4 g mol–1 (d) molar mass of X = 55.8 g mol–1
(e)
X is iron
Empirical formula is Col2
X = 5, compound is CuSO4·5H2O
0.1225 mol L–1 H2SO4(aq)
(a)
0.4863 g
(b)
99.20% purity
94.71%
42.74 mL
[Na+] = 0.0656 mol L–1, [SO42–] = 0.0328 mol L–1
[Cl–] = 0.425 mol L–1
[Al3+(aq)] = 0.128 M [Na+(aq)] = 0.384 M [SO42G(aq)] = 0.384 M
4.75% HC2H3O2
x = 12
x = 2, potassium bromite
M is iron
15.0 g Ca3(PO4)2
62.7% yield of K2Cr2O7
C5H9N3
mass of crucible = 26.483 g
(a) molar mass of X = 138.9 g mol–1 (b) X is La (atomic # = 57)
56.0 % KCl
[H2SO4(aq)] = 0.04563 M
X=4
[Na+] = 0320 mol L–1
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
11
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
[HCl] = 0.1215 mol L–1
87.3% yield
[NO3–] = 0.1716 mol L–1
EF = MF = C3H6O2
(a) [NaOH] = 0.2764 mol L–1 (b) [HNO3] = 15.67 mol L–1
NiSO3·6 H2O
LiClO3
Iridium
74.3 g P4
2 AgNO3(aq) + CaCl2(aq) → 2 AgCl(s) + Ca(NO3)2(aq)
Na2SO4(aq) + BaBr2(aq) → BaSO4(s) + 2 NaBr(aq)
Pb(NO3)2(aq) + 2 HI(aq) → PbI2(s) + 2 HNO3(aq)
CrCl3(aq) + 3 NaOH(aq) → Cr(OH)3(s) + 3 NaCl(aq)
Hg2(NO3)2(aq) + 2 NaCl(aq) → Hg2Cl2(aq) + 2 NaNO3(aq)
K2S(aq) + NiCl2(aq) → NiS(s) + 2 KCl(aq)
Ca(NO3)2(aq) + K2CO3(aq) → CaCO3(s) + 2 KNO3(aq)
3 CaI2(aq) + 2 (NH4)3 PO4(aq) → Ca3(PO4)2 (s) + 6 NH4I(aq)
52.
net ionic equations
(a)
(b)
(c)
(d)
(e)
(f)
(g)
(h)
2 Al(s) + 6 H+(aq) → 2 Al3+(aq) + 3 H2(g)
3 Fe2+(aq) + 2 PO43–(aq) → Fe3(PO4)2(s)
Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s)
2 H+(aq) + Na2CO3•10 H2O(s) → 2 Na+(aq) + CO2(g) + 11 H2O(l)
2 H+(aq) + OH–(aq) → H2O(l)
Cl2(aq) + 2 Br–(aq) → 2 Cl–(aq) + Br2(aq)
CH3COOH(aq) + OH–(aq) → CH3COO–(aq) + H2O(l)
NH3(aq) + H+(aq) → NH4+(aq)
Developed by Dr. Chris Flinn
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