Which of the following pairs of solutions is | vedclass

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(A) For isotonic solutions,the molar concentrations must be equal: $C_{	ext{urea}} = C_{	ext{sucrose}}$.First,calculate the molarity for each option

Vedclass · Accepted Answer

$3.0 \ g \ L^{-1}$ urea and $17.19 \ g \ L^{-1}$ sucrose

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(A) For isotonic solutions,the molar concentrations must be equal: $C_{	ext{urea}} = C_{	ext{sucrose}}$.First,calculate the molarity for each option.For option $A$: Molarity of urea $= \frac{3.0 \ g \ L^{-1}}{60 \ g \ mol^{-1}} = 0.05 \ mol \ L^{-1}$.Molarity of sucrose $= \frac{17.19 \ g \ L^{-1}}{342 \ g \ mol^{-1}} = 0.05026 \ mol \ L^{-1} \approx 0.05 \ mol \ L^{-1}$.Since the molar concentrations are equal,the solutions are isotonic.

Which of the following pairs of solutions is isotonic? (Molar mass: urea $= 60 \ g \ mol^{-1}$,sucrose $= 342 \ g \ mol^{-1}$)

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