1) The total concentration of ions in a 0.300 M solution of HNO3 is __________.
A) essentially zero.
B) 0.150 M
C) 0.300 M
D) 0.600 M
E) 1.200 M
2) What is the correct net ionic equation for the metathesis reaction between MgCl2(aq) and
Ba(OH)2 (aq)?
a)
b)
c)
d)
e)
Mg2+ (aq) +OH2-(aq) -> MgOH(s)
Ba2+ (aq) + 2 Cl- (aq0 -> BaCl2 (s)
Mg2+ (aq) + Ba2+ (aq) +2 Cl-(aq) +2 OH- (aq) -> Mg(OH)2(s) +BaCl2(s)
Mg2+ (aq) +2 OH-(aq) -> Mg(OH)2 (s)
Mg2+ (aq) +Cl2-(aq) -> MgCl(s)
3) What is the concentration (M) of Cl- ions in a solution made by mixing 25.0 mL of 0.100 M
KCl with 50.0 mL of 0.100 M NaCl?
A) 0.100
B) 0.0500
C) 0.0333
D) 0.0250
E) 125
4) What is the concentration (M) of CH 3 OH in a solution prepared by dissolving 12. g of
CH 3 OH in sufficient water to give exactly 250 mL of solution?
A) 11.
B) 1.5 10-3
C) 0.081
D) 1.5
E) 11 10-3
5) There are __________ mol of bromide ions in 0.500 L of a 0.200 M solution of AlBr 3 .
A) 0.150
B) 0.0500
C) 0.300
D) 0.400
E) 0.500
6) Calculate the concentration (M) of Al3+ ions in a solution made by diluting 250.0 mL of a 1.5
M solution of Al2(SO4)3 to a total volume of 1.00 L.
A) 0.750
B) 0.375
C) 3.00
D) 3.75
E) 6.00
7) A 31.5 mL portion of H 2 SO 4 (aq) of unknown concentration was titrated with 0.0134 M
NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration
(M) of the acid was __________.
A) 0.0102
B) 0.00508
C) 0.0204
D) 0.102
E) 0.227
8) Which combination will produce a precipitate? (C2H3O2- is the sam as CH3COO-)
A) NH 4 OH (aq) and HCl (aq)
B) AgNO 3 (aq) and Ca(C 2H 3O 2) 2(aq)
C) NaOH (aq) and HCl (aq)
D) NaCl (aq) and HC 2 H 3 O 2 (aq)
E) NaOH (aq) and Fe(NO 3 ) 2 (aq)
9) Of the hydrogen halides, only __________ is a weak acid.
A) HCl (aq)
B) HBr (aq)
C) HF (aq)
D) HI (aq)
E) They are all weak acids.
10)
Answer: D (2.87/total Volume)