The 0.0500 M HNO2 solution has a pH of 1.81 and a 44.5% ionisation percentage.
What is pH and how is it determined?A solution's acidity or basicity is determined by its pH. It is described as the solution's hydrogen ion concentration's negative logarithm. While lower pH values denote acidity and higher ones denote basicity, a pH of 7 is regarded as neutral.
Since HNO2 is a weak acid, the percent ionisation and pH of the solution can be determined using the acid dissociation constant (Ka) formula.
Ka = (H+)(NO2-)/(HNO2)
We can write: Ka = x2 /, where x is the concentration of H+ and NO2- and (0.0500-x) is the concentration of HNO2 (0.0500 - x)
The quadratic formula is used to solve for x, and the result is x = 0.0154 M
For these reasons, [H+] = [NO2-] = 0.0154 M and [HNO2] = 0.0346 M.
We apply the formula: to determine the % ionisation.
% ionisation is calculated as [H+]/[HNO2] x 100%, or (0.0154 / 0.0346) x 100, or 44.5%
We use the following formula to determine pH:
pH = -log(0.0154) = 1.81 where pH = -log(H+)
As a result, the 0.0500 M HNO2 solution has a pH of 1.81 and a 44.5% ionisation percentage.
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