Single Choice

A compound $$MX_{2}$$ has observed and normal molar masses 65.6 and 164 respectively. The apparent degree of ionization of $$MX_{2}$$ is:

A$$75\%$$
Correct Answer
B$$85\%$$
C$$65\%$$
D$$25\%$$

Solution

Observed molar mass $$= 65.6$$ Normal molar mass $$=164$$ So, $$i\times 65\cdot 6=164$$; $$i =\dfrac{164}{65.6}=2.5$$ And we know that, $$i=1+\alpha(n-1)$$ $$n=3$$, as one $$M^+$$ and two $$X^{-1}$$ are present. Therefore, $$2.5=1+\alpha (3-1)$$ $$\alpha=\dfrac {1.5}{2}$$ $$\alpha = 0.75$$ $$\alpha \% = 0.75\times 100=75\%$$ Hence, the correct option is $$A$$

SIMILAR QUESTIONS

Solutions

A weak electrolyte $$(AB_2)$$ with formula mass 100 g / mole is dissociated in water upto 50%. The observed molar mass of the electrolyte is:

Solutions

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Solutions

0.0852 g of an organic halide (A) when dissolved in 2.0 g of camphor, the melting point of the mixture was found to be $$167^{\circ}$$C. Compound (A) when heated with sodium gives a gas (B). 280 mL of gas (B) at STP weighs 0.375g. What would be 'A' in the whole process? $$K_f$$ for camphor = 40, m.pt. of camphor = $$179^{\circ}$$C.

Solutions

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Solutions

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Solutions

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Solutions

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Solutions

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Solutions

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