Review (ACS)
The pH of a 0.03 M HCl solution is
a. 1.5
b. 2.5
c. 3.5
d. 12.5
Which of the following salt(s) will form a basic solution upon dissolving in water?
A) LiBr
B) NaNO2
C) CsF
D) BaSO4
E) NaCN
F) AlCl3
G) CaSO3
H) NH4NO3
B, C, E, G
What is a basic oxided?
Which pair of substances could form a buffered aqueous solution?
a) CH3NH3+, CH3NH2
b) H3PO4, NaH2PO4
c) NH3, NaOH
d) H2SO3, KOH
e) HCl, LiCl
f)
HF, LiF
A, B, F
The number of neutrons in the nucleus of
an atom of Al2713 is
a. 40
b. 13
c. 27
d. 14
e. 9
D) 14
A solution is prepared by adding 0.15 mol of iron(III) nitrate, Fe(NO3)3, to 1.25 L of water. Which statement about the solution is correct?
A) the solution is acidic.
B) the solution is neutral.
C) the solution is basic.
D) None of these
E) the value of Ka for the species in solution must be known before a prediction can be made.
F) the value of Kb for the species in solution must be known before a prediction can be made.
A
What is an acidic oxide?
A nonmetal with oxgygen
In a buffer solution, if [A-]=[HA], which of the following is true?
pH = pKa
The orbitals of 2p electrons are often
represented as being
a. elliptical.
b. Pyramidal
c. Tetrahedral
d. dumbbell shaped
e. spherical
D) Dumbbell
Determine which of the following is false for a salt introduced to water. Select all that applies.
a) The conjugate acid of a weak base will produce a basic solution.
b) The cations Li+, Na+, Ba2+, Ca2+ will not have an effect on the pH.
c) Small, highly charged metal ions will produce a basic solution
d) The conjugate base of a weak acid will make the solution basic.
e) The conjugate base of a strong acid will not have an effect on the pH.
A, C
In the following equation, identify the Lewis acid.
Zn2+(aq) + 4 NH3(aq) --> Zn(NH3)42+(aq)
Zn2+(aq)
Calculate the pH of a buffer solution that contains 0.29 M benzoic acid (C6H5CO2H) and 0.48 M sodium benzoate (C6H5COONa). Ka of benzoic acid is 6.5 x 10-5
4.41
What is the equilibrium constant expression
for the gas phase oxidation of CO to CO2 by O2?
a. K = [CO2]2
[CO][O2]
b. K= [CO]2 [O2]
[CO2]
c. K= [CO2]2
[CO]2 [O2]
d. K= [CO] [O2]
[CO2]
c
The Ka(HBrO) = 2.5 x 10–9 for 0.68 M NaBrO solution. Calculate the pH of this solution.
11.22
A Lewis acid
is a substance that accepts a pair of electrons
A buffer is prepared by adding 0.550 L of 1.47 M HBr to 1.20 L of 2.83 M NaHCOO. Calculate the pH of this buffer. Ka of HCOOH is 1.70 x 10-4
4.27
Which substance is most soluble in water?
a. C6H6
b. CaCO3
c. C2H5OH
d. CO2
C) C2H5OH
The Ka(HCN) = 4.9 x 10–10 for 0.039 M NaCN solution. Calculate the pH of this solution.
10.95
A Lewis base
is a substance that donates a pair of electrons
Calculate the pH of a buffer solution that contains 0.088 M lactic acid and 0.059 M sodium lactate. Ka of nitrous acid is 1.8 x 10-4
3.57