Determine the pH of each of the following two-component
solutions.
1)4.5×10−2 M KOH and 2.5×10−2 M Ba(OH)2
2)0.265 M NH4NO3 and 0.102 M HCN
3)7.5×10−2 M RbOH and 0.120 M NaCl
4)9.2×10−2 M HClO4 and 2.2×10−2 M KOH
5)0.115 M NaClO and 5.50×10−2 M KI
Determine the pH of each of the following two-component
solutions.
1)4.5×10−2 M KOH and 2.5×10−2 M Ba(OH)2
2)0.265 M NH4NO3 and 0.102 M HCN
3)7.5×10−2 M RbOH and 0.120 M NaCl
4)9.2×10−2 M HClO4 and 2.2×10−2 M KOH
5)0.115 M NaClO and 5.50×10−2 M KI
Determine the pH of an HNO2 solution of each of the following
concentrations.
0.540 M
0.100 M
1.30×10−2 M
In which cases can you not make the simplifying assumption that
x is small?
determine the pH of each two component solution
a.) 0.550 M HI and 0.850 M HF
b.) 0.112 M NaCl and 0.953 M HF
c.) 0.050 M KOH and 0.015 M Ba(OH)2
d.) 0.088 M HClO4 and 0.022 M KOH
Determine the pH of each of the following solutions.
Part A
0.25 M KCHO2 (Ka for HCHO2 is 1.8×10−4)
Express your answer to two decimal places.
pH =
Part B
0.18 M CH3NH3I (Kb for CH3NH2 is 4.4×10−4)
Express your answer to two decimal places.
pH =
Part C
0.15 M KI
Express your answer to two decimal places.
pH =
1. Calculate the pH of the following solutions.
a. A solution containing 0.100 M KH2PO4 and 0.200 M K2HPO4
b. A solution prepared by mixing 100.0 mL 0.100 M H3PO4 with
50.0 mL 0.150 M K3PO4
c. A solution prepared by mixing 100.0 mL of 0.100 M H3PO4 and
80.0 mL of 0.200 M KOH.
Determine the pH of each of the following solutions.
(a) 0.113 M ascorbic acid (weak acid with Ka =
8e-05).
(b) 0.261 M phenol (weak acid with Ka = 1.3e-10).
(c) 0.150 M pyridine (weak base with Kb =
1.7e-09).