Question

What is the ph of 1M ch3coona solution if Ka is 1.8*10^-5

Answer 1

Explanation:

hope this helps you.plz follow and mark as brainliest ans.

Answer 2

The pH of the solution is, 9.35

Explanation : Given,

$K_a=1.8\times 10^{-5}$

Concentration of $CH_3COONa$ = C = 1 M

First we have to calculate the value of $pK_a$.

The expression used for the calculation of $pK_a$ is,

$pK_a=-\log (K_a)$

Now put the value of $K_a$ in this expression, we get:

$pK_a=-\log (1.8\times 10^{-5})$

$pK_a=5-\log (1.8)$

$pK_a=4.7$

Now we have to calculate the pH of solution.

$pH=7+\frac{1}{2}pK_a+\frac{1}{2}\log C$

Now put all the given values in this expression, we get:

$pH=7+\frac{1}{2}\times 4.7+\frac{1}{2}\times \log(1)$

$pH=9.35$

Therefore, the pH of the solution is, 9.35

Learn more about : pH for weak acid and strong base

https://brainly.in/question/2590552

#learnwithbrainly