A $17.2 \cdot g$ $17.2g$ mass of ethylene glycol was dissolved in a $500 \cdot g$ $500g$ mass of water to give a solution of $515 \cdot m L$ $515*mL$ volume. What are....?

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A $17.2 \cdot g$ $17.2g$ mass of ethylene glycol was dissolved in a $500 \cdot g$ $500g$ mass of water to give a solution of $515 \cdot m L$ $515*mL$ volume. What are....?

$(i) Molarity...$ $"(i) Molarity..."$
$(ii) Molality...$ $"(ii) Molality..."$
$(iii) Percentage by mass...$ $"(iii) Percentage by mass..."$
$(iv) Moles fractions of each component...$ $"(iv) Moles fractions of each component..."$

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Answer 1 · 2017-02-02T15:42:23

$Moles of solute$ $"Moles of solute"$ $=$ $=$ $\frac{17.2 \cdot g}{62.07 \cdot g \cdot m o l^{- 1}} = 0.277 \cdot m o l$ $(17.2*g)/(62.07*g*mol^-1)=0.277*mol$

Explanation:

$Molarity = \frac{Moles of solute}{Volume of solution} = \frac{0.277 \cdot m o l}{0.515 \cdot L}$ $"Molarity"="Moles of solute"/"Volume of solution"=(0.277*mol)/(0.515*L)$

$≅ 0.50 \cdot m o l \cdot L^{- 1}$ $~=0.50*mol*L^-1$

$Molality = \frac{Moles of solute}{Kilograms of solvent} = \frac{0.277 \cdot m o l}{0.500 \cdot k g}$ $"Molality"="Moles of solute"/"Kilograms of solvent"=(0.277*mol)/(0.500*kg)$

$≅ 0.50 \cdot m o l \cdot k g^{- 1}$ $~=0.50*mol*kg^-1$

$Percentage by mass$ $"Percentage by mass"$ $=$ $=$ $\frac{Mass of solute}{Mass of solution} \times 100 %$ $"Mass of solute"/"Mass of solution"xx100%$

$= \frac{17.2 \cdot g}{17.2 \cdot g + 500 \cdot g} \times 100 % = 3.33 % (\frac{m}{m})$ $=(17.2*g)/(17.2*g+500*g)xx100%=3.33%(m/m)$

$Mole fraction, χdiol$ $"Mole fraction, "chi_"diol"$ $=$ $=$ $\frac{Moles of diol}{Moles of diol + moles of solvent}$ $"Moles of diol"/"Moles of diol + moles of solvent"$

$= \frac{0.277 \cdot m o l}{0.277 \cdot m o l + \frac{500 \cdot g}{18.01 \cdot g \cdot m o l^{- 1}}} ≅ 0.001$ $=(0.277*mol)/(0.277*mol+(500*g)/(18.01*g*mol^-1))~=0.001$

What is $χ_{water}$ $chi_"water"$ ?

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A $17.2 \cdot g$ $17.2g$ mass of ethylene glycol was dissolved in a $500 \cdot g$ $500g$ mass of water to give a solution of $515 \cdot m L$ $515*mL$ volume. What are....?

$(i) Molarity...$ $"(i) Molarity..."$
$(ii) Molality...$ $"(ii) Molality..."$
$(iii) Percentage by mass...$ $"(iii) Percentage by mass..."$
$(iv) Moles fractions of each component...$ $"(iv) Moles fractions of each component..."$

1 Answer

Explanation:

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A 17.2*g17.2⋅g17.2*g mass of ethylene glycol was dissolved in a 500*g500⋅g500*g mass of water to give a solution of 515*mL515⋅mL515*mL volume. What are....?

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Explanation:

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A $17.2 \cdot g$ $17.2g$ mass of ethylene glycol was dissolved in a $500 \cdot g$ $500g$ mass of water to give a solution of $515 \cdot m L$ $515*mL$ volume. What are....?