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Chapter 11: Q41 E (page 648)

A 13.0% solution of \({\bf{K_2CO_3}}\) by mass has a density of 1.09\({\bf{g/g}}{{\bf{m}}^{\bf{3}}}\). Calculate the molality of the solution.

Short Answer

Expert verified

The molality of \({\bf{K_2CO_3}}\) = 1.08 molal

Step by step solution

01

Molality

Molality may be defined as the number of moles of the solute present in the solvent in kilogram. It depends upon the concentration of the solution.

02

Molality of Glucose

13.0% solution means 13 g of \({\bf{K_2CO_3}}\) is in the 100 g solution

Solutionmass = Solute mass+ solvent mass

100 g = 13 g + SolventWeight

Solvent weight = 100 g - 13 g = 87 g

Number of Moles of \({\bf{K_2CO_3 = }}\frac{{{\bf{13}}}}{{{\bf{138}}{\bf{.2}}}}{\bf{ = 0}}{\bf{.094}}\)

Convert the massof solvent into grams

87g = 0.087kg

\({\bf{Molality = }}\frac{{{\bf{Numberofmoles}}}}{{{\bf{MassofSolvent(kg)}}}}\)

Molality of\(K_2CO_3 = \frac{{0.094}}{{0.087}} = 1.08molal\)

Thus, the molality of the answeris 1.08 m

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Most popular questions from this chapter

Question: The vapor pressure of methanol, \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\) , is 94 tor at 20 掳C. The vapor pressure of ethanol,\({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\) , is 44 tor at the same temperature.

(a) Calculate the mole fraction of methanol and of ethanol in a solution of 50.0 g of methanol and 50.0 g of ethanol.

(b) Ethanol and methanol form a solution that behaves like an ideal solution. Calculate the vapor pressure of methanol and of ethanol above the solution at 20 掳C.

(c) Calculate the mole fraction of methanol and of ethanol in the vapor above the solution.

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The osmotic pressure of a solution containing 7.0 g of insulin per litre is 23 torr at 25 掳C. What is the molar mass of insulin?

What is the osmotic pressure (atm) of a solution with a volume of 0.750 L that contains 5.0 g of methanol,\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\), in water at 37 掳C?

Calculate the mole fraction of each solute and solvent:

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