Equilibrium Question 535
Question: What will be the $ pH $ value of 0.05 M $ Ba{{(OH)}_2} $ solution [CPMT 2004]
Options:
A) 12
B) 13
C) 1
D) 12.96
Show Answer
Answer:
Correct Answer: B
Solution:
$ Ba{{(OH)}_2}\ \to \ \underset{.05M}{\mathop{B{a^{+2}}}},+\underset{2\times 0.5M}{\mathop{2O{H^{-}}}}, $
$ pOH=\log \frac{1}{{{[OH]}^{-}}}=\log \frac{1}{.1}=1 $
$ pH+pOH=14 $ ; $ pH+1=14 $ ; $ pH=14-1=13 $
