Question

Calculate the ph of a 0.036 m nitrous acid (hno2) solution

Answer 1

ANSWER:

                                                    Given,

Formulae:pH = -㏒[H⁺]                                       Molarity(M)=0.036M

∴pH = -㏒[0.036]

        =1.44

Answer 2

pH of a 0.036 m nitrous acid solution is 2.4

Explanation:

pH : It is defined as the negative logarithm of the hydrogen ion concentration.

First we have to calculate the hydrogen ion concentration [tex](H^+) [/tex]

$pH=-\log [H^+]$

$HNO_2\rightarrow H^++NO_2^-$

As 1 mole of $HNO_2$ gives 1 mole of $H^+$

0.0036 moles of $HNO_2$ gives =$\frac{1}{!}\times 0.0036=0.0036$ moles of $H^+$

$pH=-\log [0.0036]=2.4$

Thus the pH of a 0.036 m nitrous acid solution is 2.4

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