Question

Ph of 0.05 m of naoh solution
Ph of 0.05 m of Ba(oh)2 aqueous solution

Answer 1

What is the pH value of 0.05M NaOH solution?

Here, the molarity of the solution is 0.05M.

That means,every 1 litre solution has 0.05 M NaOH in it.

Thus, [NaOH] = 0.05

Now, the dissociation goes like:

NaOH —-> Na+ + OH-

Further, the dissociation is practically 100%.

[OH-] = [NaOH] = 0.05

Thus, pOH = - log [OH-] = -log 0.05 = 1.30102999566

Also,

pH + pOH = 14

=> pH = 14 - pOH = 14 - 1.30102999566 = 12.699 (approx.)

FOR Ba(OH)2

Normality Is 2, So N=2M (molarity)

For Ba(OH)2= 2*0.5= 1 .

" For Solve Any question Always Use N"

Now For A Basic Solution Question Gives Always pOH , Same For It.pOH= -log (OH)

-log(10^-1)

=1

So pH iS 14-1= 13

;)

Hope

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Helps

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:::)