A) 0.855 g
B) 17.1 g
C) 8.55 g
D) 85.5 g
Correct Answer: C
Solution :
\[\Delta {{T}_{b}}={{m}_{solute}}{{K}_{b}}\] \[=0.3=\frac{\left( \frac{1.0}{M} \right)\times 1000}{10}\times 0.513\] = 171 [M = molecular weight of solute] We have, Molarity \[\text{=}\frac{\frac{\text{Weight}}{\text{M}}\text{ }\!\!\times\!\!\text{ 1000}}{\text{Volume}\,\text{of}\,\text{solution(in}\,\text{mL)}}\] \[\text{0}\text{.1=}\frac{\frac{\text{Weight}}{171}\text{ }\!\!\times\!\!\text{ 1000}}{500}\]Weight = 5.55 gYou need to login to perform this action.
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