What is the $pH$ of a mass of $4.66mg$ of barium hydroxide dissolved in a $1L$ volume of water?

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Answer 1 · 2016-10-26T19:23:10

$pH=9.74$

We need to find (i), $[HO^-]$ $=$ $(2xx4.66xx10^-3g)/(171.34*g*mol^-1)xx1/L$ $=$ $5.44xx10^-5mol*L^-1$ .

And (ii), $pOH$ $=$ $-log_10[HO^-]$ $=$ $-log_10(5.44xx10^-5)$ $=$ $4.26.$

And since (iii) $pH+pOH=14, pH=14-4.26=9.74$ .

What is the pHpH of a mass of 4.66*mg4.66*mg of barium hydroxide dissolved in a 1*L1*L volume of water?