A $0.1$ M solution of an acid (density $= 1.01$ g/cc) is $4.5 %$ ionised. Calculate the f.p. of the solution. The molecular weight of the acid is $300$ . $K_{f} = 1.86$ .

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0.1

M solution of an acid (density

= 1.01

g/cc) is

4.5 %

ionised. Calculate the f.p. of the solution. The molecular weight of the acid is

300

K_{f} = 1.86

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0.1 M

aqueous solution of a monoprotic acid

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Given:

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0.1

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A 0.1 M solution of an acid (density =1.01 g/cc) is 4.5% ionised. Calculate the f.p. of the solution. The molecular weight of the acid is 300. Kf=1.86.

A $0.1$ M solution of an acid (density $= 1.01$ g/cc) is $4.5 %$ ionised. Calculate the f.p. of the solution. The molecular weight of the acid is $300$ . $K_{f} = 1.86$ .