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Standard XII

Chemistry

Factors Affecting Alpha

The pH of 0.1...

Question

The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

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Solution

$c = 0.1 M p H = 2.34 - l o g [H^{+}] = p H - l o g [H^{+}] = 2.34 [H^{+}] = 4.5 \times 10^{- 3}$
Also,
$[H^{+}] = c α 4.5 \times 10^{- 3} = 0.1 \times α \frac{4.5 \times 10^{- 3}}{0.1} = α α = 45 \times 10^{- 3} = .045$
Then,
$K_{a} = c α^{2} = 0.1 \times (45 \times 10^{- 3})^{2} = 202.5 \times 10^{- 6} = 2.02 \times 10^{- 4}$

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Factors Affecting Alpha

Standard XII Chemistry

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The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

c=0.1MpH=2.34−log[H+]=pH−log[H+]=2.34[H+]=4.5×10−3 Also, [H+]=cα4.5×10−3=0.1×α4.5×10−30.1=αα=45×10−3=.045 Then, Ka=cα2=0.1×(45×10−3)2=202.5×10−6=2.02×10−4