Question

calculate the ph of 0.05m ba(oh)2 solution

Answer 1

pH calculation:

The reaction is as follows:

$B a(O H)_{2} \rightarrow B a_{2}^{+}+2 O H^{-}$

Since, $n = 2M$

$= 2 \times 0.05$

= 0.10

Putting log,

$p (OH) = log (OH)$

$= log (0.10)$

$= 1$

The pH of $B a(O H)_{2}$ is

$= 14-1= 13.$

Thus, the solution of $B a(O H)_{2}$ is more basic in nature.

The pH scale ranges from 0 to 14, with 1 being most acidic, 7 being neutral and 14 being most basic or alkaline in nature.

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