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katrin2010 [14]
3 years ago
14

assuming complete dissociation, what is the pH of a 0.606 M Ba(OH)2 solution? round to 3 significant figures​

Chemistry
1 answer:
masha68 [24]3 years ago
5 0

Answer:

pH = 14.05.

Explanation:

Hello!

In this case, since barium hydroxide ionizes according to the following equation:

Ba(OH)\rightarrow Ba^{2+}+2OH^-

We can compute the concentration of hydroxyl ions based on:

[OH^-]=0.606\frac{molBa(OH)_2}{L}*\frac{2molOH^-}{1molBa(OH)_2}  =1.21M

Next we compute the pOH:

pOH=-log([OH^-])=-log(1.12)=-0.0500

Thus the pH is:

pH=14-pOH=14+0.05\\\\pH=14.05

Which means it is very concentrated basic solution.

Best regards!

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