Units & Formulas
General Equilibrium
Acids and Bases
Buffers
Solubility
100
This equation involves the addition of pH and pOH.
What is pH + pOH=14?
100
The name for the equilibrium constant for pressure.
What is Kp?
100
Which of the following acids will dissociate 100% in water?
A. nitrous acid, HNO2
B. hydrofluoric acid, HF
C. sulfurous acid,H2SO3
D. perchloric acid, HClO4
E. carbonic acid, H2CO3
D. perchloric acid, HClO4
100
What are the two possible combinations that produce a buffer solution?
A weak acid and its conjugate base and a weak base and its conjugate acid.
100
When Qsp>Ksp, the solution is said to be _______, therefore a ____ will form
A.Saturated, precipitate
B.Unsaturated, nothing
C.Supersaturated, precipitate
D.Saturated, nothing
Option C (Supersaturated, precipitate)
200
This formula can be used to calculate pKa when given pH and concentrations of buffer components.
What is pH=pKa +log (base)/(acid)?
200
True or false: If Qc <Kc,the reaction shifts left to reestablish equilibrium.
False.
200
In the Brønsted–Lowry definition of acids and bases, an acid__________
is a proton donor.
is a proton acceptor.
forms stable hydrogen bonds.
breaks stable hydrogen bonds.
corrodes metal.
1. is a proton donor
200
Which of the following is not a buffer system? A solution containing roughly equal concentrations of __________.
fluoride ion and hydrofluoric acid.
bromide ion and hydrobromic acid.
carbonate ion and hydrogen carbonate ion.
phosphoric acid and dihydrogen phosphate ion.
Option 2 (Bromide ion and hydrobromic acid)
200
The solubility product expression for tin(II) hydroxide, Sn(OH)2, is
(a) [Sn2+][OH-]
(b) [Sn2+]2[OH-]
(c) [Sn2+][OH-]2
(d) [Sn2+]3[OH-]
(e) [Sn2+][OH-]3
Option C ( [Sn2+][OH-]2).
300
The units for solubility (hint: not Molar solubility).
What is grams per Liters (g/L)?
300
True or False: The Law of Mass Action states that the value of K depends only on the chemical equation and temperature.
True.
300
The following titration curve is most likely to be associated with:
A. the titration of a strong acid with a strong base titrant.
B. the titration of a weak acid with a strong base titrant.
C. the titration of a strong base with a strong acid titrant.
D. the titration of a weak base with a strong acid titrant.
D. the titration of a weak base with a strong acid titrant
300
Which one of the following would make the best buffer? (Ac = acetate, CH3CO2)?
a solution of hydrochloric acid and sodium chloride, HCl and NaCl
a solution of acetic acid and ammonia, NaAc and NH3
a solution of acetic acid and ammonium chloride, HAc and NH4Cl
a solution of sodium acetate and ammonium chloride, NaAc and NH4Cl
a solution of ammonia and ammonium chloride, NH3 and NH4Cl
Option 5, a solution of ammonia and ammonium chloride.
300
Write a chemical equation representing solubility equilibrium for Ag(CN)2.
Ag(CN)2(s) → ← Ag2+(aq) + 2 CN–(aq)
400
This formula can be used to convert a Kp value to Kc.
What is Kp=KcRTΔn?
400
The equilibrium constant for the acid ionization of mercaptoethanol (HSCH2CH2OH) is 1.91 x 10^-10.
HSCH2CH2OH(aq) -> H+(aq) + SCH2CH2OH–(aq)
Which of the following statements (is/are) true regarding this equilibrium?
The reaction is product-favored.
The reaction is reactant-favored.
Equilibrium lies far to the right.
Equilibrium lies far to the left.
Options 2 and 4 are correct.
400
HNO2 has a pKa = 3.35 and HOCl has a pKa = 7.45. Which is the stronger acid?
HNO2.
400
The pH of a solution that’s 0.65M in NaF and 0.75M in HF is? (HF, Ka = 7.2 × 10–4)
What is 3.08?
400
The molar solubility of PbCl2 is 0.016 mol/L. What is the value of Ksp for PbCl2?
a. 4.1 × 10-6
b. 1.6 × 10-5
c. 2.6 × 10-4
d. 5.1 × 10-4
e. 4.8 × 10-2
Option B.
500
Percent ionization of a 0.010 M solution of HA solution if in the ICE table, x =2.76 x 10^-4.
What is 0.28%?
500
The [OH-] of a 0.200 M aqueous solution of NaF is?
What is 1.7 x 10-6M?
500
A student prepares a solution of a weak monoprotic acid by dissolving 0.080 moles of the acid in enough water to make 1.0 liter of solution. The pH of the resulting solution is 4.51. What is the Ka for this acid?
Ka=1.2x10-8
500
Consider a solution initially containing 0.300 mol of hydrogen fluoride (HF). How many grams of NaF (42.0 g/mol) would be needed to set the pH = 3.00? (HF, Ka = 7.2 × 10–4)?
What is 9.07 grams NaF?
500
What is the molar solubility of Fe3+ in a solution that is buffered at a pH of 4.00? The Ksp for Fe(OH)3 is 6.3 × 10-38.
a. 6.3 × 10-23 mol/L
b. 2.3 × 10-9 mol/L
c. 6.3 × 10-8 mol/L
d. 2.3 × 10-6 mol/L
e. 1.4 × 10-4 mol/L
Option C.