WorksheetsAqueous Reactions Quizizz
Total questions: 37
Worksheet time: 1hrs 14mins
The solvent in an aqueous solution is (a) .
Calculate the concentration (M) of arsenic acid (H3AsO4) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.
0.08892
0.2668
0.1345
0.8003
Of the species below, only ________ is not an electrolyte.
KOH
Ar
Rb2SO4
NaCl
HCl
The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution is ________.
0.0657
1.85 × 10-3
0.104
1.85
3.52
The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is ________.
0.197
1.85
11.8
3.52
2.12
The concentration of chloride ions in a 0.193 M solution of potassium chloride is ________.
0.0643 M
0.193 M
0.0965 M
0.579 M
0.386 M
The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium ion and ________ M sulfate ion.
2.104, 1.052
4.208, 2.104
2.104, 2.104
2.104, 4.208
1.052, 1.052
There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr3.
0.167
0.0500
0.150
0.525
0.500
The net ionic equation for the reaction between aqueous solutions of HF and KOH is ________.
HF + K+ + OH- → H2O + KF
H+ + OH- → H2O
HF + OH- → H2O + F-
H+ + F- + K+ + OH- → H2O + K+ + F-
HF + KOH → H2O + K+ + F-
The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.
Ca+2 (aq) + CO32- (aq) → CaCO3 (s)
2 Na+ (aq) + CO32- (aq) → Na2CO3 (aq)
Na+ (aq) + Cl- (aq) → NaCl (aq)
Na2CO3 (aq) + CaCl2 (aq) → 2 NaCl (aq) + CaCO3 (s)
2 Na+ (aq) + 2 Cl- (aq) → 2 NaCl (aq)
The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are ________.
H+ and Ba2+
H+ and OH-
H+, OH- , ClO4-, and Ba2+
OH- and ClO4-
ClO4- and Ba2+
Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:
Pb2+ (aq) + 2I- (aq) → PbI2 (s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.600 mol of Pb(NO3)2 (aq) to completely precipitate the lead?
338
0.338
0.169
2.96 × 10-3
169
Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.
6.99 × 10-4
2.52 × 103
42.0
0.699
0.0420
What volume (mL) of 0.102 M NaOH is required to neutralize 17.1 mL of 0.443 M HCl?
0.0135
3.94
0.000773
74.3
0.773
What is the concentration (M) of 39.88 mL of an unknown NaOH solution if it required 46.08 mL of 0.6592 M HCl to neutralize?
2788
1.211
1211
1.313
0.7617
What mass (g) of CaF2 is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous calcium nitrate?
1.04
1040
0.520
5420
0.171
A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.
1.57
254
0.635
0.254
635
Which one of the following compounds is insoluble in water?
Na2CO3
K2SO4
AgNO3
ZnS
Fe(NO3)3
What are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?
K+ only
Ag+ and Cl-
K+ and Ag+
K+ and NO3-
Ag+ and NO3-
With which of the following will the ammonium ion form an insoluble salt?
carbonate
sulfate and carbonate
sulfate
chloride
none of these
How many grams of NaCl are contained in 350 mL ofa 0.102 M solution of sodium chloride?
6.0 g
2.09 g
4.17 g
35.7 g
What mass of calcium chloride, CaCl2, is needed to prepare 3.840 L of a 1.56 M solution?
273 g
5.99 g
45.1 g
111 g
665 g
A 79.1 g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.
56.1 M
4.44 M
111.5 M
2.00 M
What mass of solute is contained in 256 mL of a 0.887 M ammonium chloride solution?
12.1 g
185 g
15.4 g
227 g
What volume of 18.0 M sulfuric acid must be used to prepare 13.2 L of 0.195 M H2SO4?
143 mL
2.57 mL
266 mL
6.08 mL
3.51 mL
The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?
Ca2+ (aq)
3 Ca2+ (aq)
PO43- (aq)
2 Ca3(PO4)2 (s)
6 NaBr (aq)
Which of the following is a strong acid?
HF
KOH
HClO4
HClO
HBrO
All of the following are weak acids except
HCNO
HBr
HF
HNO2
HCN
Which of the following is NOT a strong base?
Ca(OH)2
KOH
NH3
LiOH
Sr(OH)2
When solutions of cobalt (II) chloride and carbonic acid react, which of the following terms will be present in the net ionic equation?
CoCO3 (s)
H+ (aq)
2 CoCO3 (s)
2 Cl- (aq)
two of these
In writing the total ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species?
KOH
Mg(NO3)2
Mg(OH)2
KNO3
Aqueous solutions of sodium sulfide & copper (II) chloride are mixed together. Which statement is correct?
Both NaCl & CuS precipitate from solution.
No precipitate forms.
CuS will precipitate from solution.
NaCl will precipitate from solution.
No reaction will occur.
Which of the following salts is insoluble in water?
Na2S
K3PO4
Pb(NO3)2
CaCl2
All of these are soluble in water.
Which of the following ions is most likely to form an insoluble sulfate?
K+
Li+
Ca2+
S2-
Cl-
Which of the following compounds is soluble in water?
Ni(OH)2
K3PO4
BaSO4
CoCO3
PbCl2
If all of the chloride in a 3.213 g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, What is the percentage of chloride in the sample?
50.52%
15.72%
1.425%
6.360%
none of these
You mix 60. mL of 1.00 M silver nitrate with 25 mL of 1.02 M sodium chloride. What mass of silver chloride should you form?
3.7 g
7.3 g
18.6 g
8.8 g
none of these
