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A $0.6 \%$ solution for urea (molecular mass $=60)$ would be isotonic with
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$0.1 \mathrm{M}$ glucose solution
Molarity of $0.6 \%$ solution $=\frac{0.6}{60} \times \frac{1000}{100}=0.1 \mathrm{M}$
From, the options, we know that $\mathrm{KCl}$ will dissociate as it ionic. Therefore, option (c) and (d) are incorrect.
And, molarity of $0.6 \%$ glucose $=\frac{0.6}{180} \times \frac{1000}{100}=0.3 \mathrm{M}$
So, $0.6 \%$ solution of urea is isotonic with $0.1 \mathrm{M}$ glucose solution.
From, the options, we know that $\mathrm{KCl}$ will dissociate as it ionic. Therefore, option (c) and (d) are incorrect.
And, molarity of $0.6 \%$ glucose $=\frac{0.6}{180} \times \frac{1000}{100}=0.3 \mathrm{M}$
So, $0.6 \%$ solution of urea is isotonic with $0.1 \mathrm{M}$ glucose solution.
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