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please helpWhat’s the pH of a solution of ammonia that has a concentration of 0.335 M? The Kb of ammonia is
1.8 × 10–5
. First complete the ICE chart.
HA H3O+ AInitial
Change
Equilibrium
iii. Calculate the pH. Please show all work.

please helpWhats the pH of a solution of ammonia that has a concentration of 0335 M The Kb of ammonia is 18 105 First complete the ICE chart HA H3O AInitial Cha class=

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From the calculation, the pH of the solution is 4.85.

What is the pH?

The pH is defined as the hydrogen ion concentration of the solution. We have the ICE table as;

         HA    +    H2O ⇔     H3O^+    +    A^-

I       0.335                          0                0

C     -x                                  +x              +x

E   0.335 - x                         x                x

Ka = 1 * 10^-14/Kb

Ka = 1 * 10^-14/1.8 × 10^–5

Ka = 5.56 * 10^-10

Ka = [H3O^+] [A^-]/[HA]

But  [H3O^+] = [A^-] = x

5.56 * 10^-10 = x^2/ 0.335 - x

5.56 * 10^-10(0.335 - x ) =  x^2

1.86  * 10^-10 - 5.56 * 10^-10x =  x^2

x^2 + 5.56 * 10^-10x - 1.86  * 10^-10 = 0

x=0.000014 M

Now;

pH = -log 0.000014 M

pH = 4.85

Learn more about pH:https://brainly.com/question/15289741

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