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Free_Kalibri [48]
2 years ago
7

Calculate the pH in an aqueous 0.120 M nitrous acid solution.

Chemistry
2 answers:
Anvisha [2.4K]2 years ago
8 0

Answer:-  pH is 2.14.

Solution:- Nitrous acid, HNO_2 is a weak acid so first of all we solve for H_3O^+ and then figure out the pH.

the equation is written as:

HNO_2(aq)+H_2O(l)\leftrightharpoons H_3O^+(aq)+NO_2^-(aq)

Initial concentration for the acid is given as 0.120 M. Let's say the change in concentration is x. Then the equilibrium concentrations would be as:

HNO_2=0.120-x

H_3O^+ = x

NO_2^- = x

Ka for nitrous acid is 4.5*10^-^4 and the equilibrium expression for this would be written as:

Ka=\frac{[H_3O^+][NO_2^-]}{HNO_2}

Let's plug in the values in it.

4.5*10^-^4=\frac{(x)^2}{0.120-x}

To make the calculations easy we could ignore x for the bottom and the expression becomes:

4.5*10^-^4=\frac{(x)^2}{0.120}

On cross multiply:

x^2=4.5*10^-^4*0.120

On taking square root to both sides:

x=7.3*10^-^3

So, [H_3O^+]=7.3*10^-^3M

Now we could calculate the pH using the pH formula:

pH=-log[H_3O^+]

pH=-log(7.3*10^-^3)

pH = 2.14

So, the pH of 0.120M nitrous acid is 2.14.

artcher [175]2 years ago
8 0

pH can be calculated from pKa of aniline hydrochloride

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