Ionic EquilibriumHard
Question
Which of the following solutions would have same pH?
Options
A.100 ml of 0.2 M HCl + 100 ml of 0.4 M NH3
B.50 ml of 0.1 M HCl + 50 ml of 0.2 M NH3
C.100 ml of 0.3 M HCl + 100 ml of 0.6 M NH3
D.All will have same pH.
Solution
(a) NH4OH + HCI → NH4CI + H2O
0.2 M 0.1 0 0
0.1 0 0.1 0.1
pOH = pKb
(b) NH4OH + HCI → NH4CI + H2O
0.1 0.05 0 0
0.05 0 0.05
pOH = pKb + log
= pKb
(c) NH4OH + HCI → NH4CI + H2O
0.3 0.15
0.15 0 0.15
pOH = pKb So all solution have same pH
0.2 M 0.1 0 0
0.1 0 0.1 0.1
pOH = pKb
(b) NH4OH + HCI → NH4CI + H2O
0.1 0.05 0 0
0.05 0 0.05
pOH = pKb + log
= pKb(c) NH4OH + HCI → NH4CI + H2O
0.3 0.15
0.15 0 0.15
pOH = pKb So all solution have same pH
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