Identification
Acid/Base strength
Salts, Ka, Ionization, etc.
pH / pOH
pH / pOH
(cont'd)
(cont'd)
100
The conjugate base of CH3OH
CH3O-
100
The Bronsted acid that gives the weakest conjugate base:
HF, H2S, HCl, H2O
HCl
100
Predict whether Zn(NO3)2 will form a basic, acidic, or neutral salt solution.
acidic
100
What is the pH of a 0.75M HC2H3O2 solution?
Ka= 1.8 x 10-5
pH = 2.43
100
Calculate pH for 0.0080 M NH3 solution
Kb= 1.8 x 10-5
10.6
200
The conjugate acid of N3-
HN3
200
Rank the following compounds in order of increasing acidity:
CH3CH3, CH3OH, CH3NH2, CH3SH
CH3CH3 < CH3NH2 < CH3OH < CH3SH
200
Write the equation for the ionization and Ka expression for the following Bronsted-Lowry weak acid:
HOClO
HOClO(aq) + H2O(l) <=> H3O+(aq) + OClO-(aq)
200
What is the pH of a 0.25M NH3 solution? Kb=1.8 x 10-5
pH=11.33
200
Calculate pH of a 0.25 M solution of KF
Ka for HF = 7.0 x 10-4
8.28
300
Given the reaction:
C6H5OH(l) + NH2-(aq) -> C6H5O-(aq) + NH3(aq)
This is the role "NH2-" plays in the reaction and its resulting conjugate...
What is a base that is involved in the conjugate acid formation of NH3?
300
Ka values for H2SO3, HNO2, CH3COOH, and HCN are respectively 1.3 x 10-2, 4 x 10-4, 1.8 x 10-5, and 4 x 10-10.
Given the above acids, this one produces the strongest conjugate base in aqueous solutions.
HCN
300
Determine if (NH4)2SO4 would form an acidic, neutral, or basic solution when dissolved in water.
Acidic
300
A solution is created by measuring 3.60 x 10-3 mol NaOH and 5.95 x 10-4 mol HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution?
11.48
300
What is the pH?
[H3O+] = 10-11
11
400
Given the reaction:
O2-(aq) + H2O (l) -> 2OH- (aq)
Associate each reactant/product with its appropriate label...
O2- = base
H2O = acid
2OH- = conjugate acid and conjugate base
400
Four acids along with their pKa are given:
Acid A: pKa 50
Acid B: pKa 15.7
Acid C: pKa 38
Acid D: pKa 3.2
This acid is NEXT to the most weakest out of the 4.
What is Acid C?
400
Predict if the solutions of the following salts are neutral, acidic or basic.
NaCl, KBr, NaCN, NH4NO3, NaNO2 and KF
NaCl, KBr = neutral
NH4NO3 = acidic
NaCN, NaNO2, and KF = basic
400
Calculate the pH of 0.025 M Ca(OH)2
12.7
400
What is the pH?
[OH-]= 10-8
6
500
Given the reaction:
SO3 + H2O <=> H2SO4
This reactant acts as a Lewis base.
H2O (lone pair of electrons is donated)
500
Identify the stronger acid:
HNO2 vs. HNO3
HNO3
500
Calculate the % ionization of a solution of 0.75M HF.
Ka = 7.2 x 10-4
9.6%
500
Calculate the pH of 0.05 M solution of HClO.
Ka= 3.5 x 10-8
4.39
500
My middle name?
Lee