a. The pH of an aqueous solution of 0.272 M potassium hypochlorite, KClO (aq), is: __________
is this solution acidic/basic/neutral?
b. The pH of an aqueous solution of 0.274 M sodium cyanide, NaCN (aq), is: __________
is this solution acidic/basic/neutral?
a. The pH of an aqueous solution of 0.272 M potassium hypochlorite, KClO (aq), is: 10.445
is this solution acidic/basic/neutral? : basic
b. The pH of an aqueous solution of 0.274 M sodium cyanide, NaCN (aq), is: 11.416
is this solution acidic/basic/neutral? : basic
Explanation
(a.) initial concentration of ClO- = initial concentration of KClO = 0.272 M
Ka HClO = 3.5 x 10-8
Kb ClO- = (Kw) / (Ka)
Kb ClO- = (1.0 x 10-14) / (3.5 x 10-8)
Kb ClO- = 2.9 x 10-7
ICE table | ClO- (aq) | H2O (l) | HClO (aq) | OH- (aq) | |
Initial conc. | 0.272 M | - | 0 | 0 | |
Change | -x | - | +x | +x | |
Equilibrium conc. | 0.272 M - x | - | +x | +x |
Kb = [HClO]eq[OH-]eq / [ClO-]eq
2.9 x 10-7 = [(x) * (x)] / (0.272 M - x)
Solving for x, x = 2.786 x 10-4 M
[OH-] = x = 2.786 x 10-4 M
pOH = -log[OH-]
pOH = -log(2.786 x 10-4 M)
pOH = 3.555
pH = 14 - pOH
pH = 14 - 3.555
pH = 10.445
(b.) initial concentration of CN- = initial concentration of NaCN = 0.274 M
Ka HCN = 4.0 x 10-10
Kb CN- = (Kw) / (Ka)
Kb CN- = (1.0 x 10-14) / (4.0 x 10-10)
Kb CN- = 2.5 x 10-5
ICE table | CN- (aq) | H2O (l) | HCN (aq) | OH- (aq) | |
Initial conc. | 0.274 M | - | 0 | 0 | |
Change | -x | - | +x | +x | |
Equilibrium conc. | 0.274 M - x | - | +x | +x |
Kb = [HCN]eq[OH-]eq / [CN-]eq
2.5 x 10-5 = [(x) * (x)] / (0.274 M - x)
Solving for x, x = 2.786 x 10-4 M
[OH-] = x = 2.6 x 10-3 M
pOH = -log[OH-]
pOH = -log(2.6 x 10-3 M)
pOH = 2.584
pH = 14 - pOH
pH = 14 - 2.584
pH = 11.416
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