Application of Colligative Properties

Multiple Choice

What kind of solution is salt?

• Ideal

• Non-ideal

• Can be both ideal and non-ideal

• It is not a solution.

Dropdown

The total vapor pressure is the same as predicted by Raoult’s law​

Select answer

​ ​

The total vapor pressure increases or decreases from the predicted value according to Raoult’s law ​

Select answer

Drag and Drop

No heat is released or absorbed, so the enthalpy of mixing is zero​

Placeholder

Heat is either absorbed or released​

Placeholder

Drag these tiles and drop them in the correct blank above

Ideal

Non-ideal

Multiple Choice

What is K_b?

• molal boiling point elevation constant

• boiling point elevation

• van’t Hoff factor

• molal concentration of solute particles

Multiple Select

$$\Delta T_b$$ can be solved by...

• Subtracting T_b of solvent from T_b of solution

• Subtracting T_f of solvent from T_f of solution

• Multiplying molal boiling point elevation constant with molality

• T_{b, solvent} - T_{b, solution}

Multiple Choice

Review. Which of the following is the formula for molality (m)?

Fill in the Blanks

What is the new boiling point of a solution, ΔT_b prepared by adding 96.0 g of sodium chloride to 383mL of water?

The boiling point constant for water is 0.52 °C/m.

Molar Mass of NaCl is 58.44g/mol

Assume 1L = 1kg

Fill in the Blanks

What is the molality of a solution dissolved in chloroform that boils at 62.8°C? Boiling point of chloroform is 61.2°C?

K_b chloroform is 3.63°C/m

Fill in the Blanks

What is the freezing point of a solution prepared by adding 140g trichothecin (C₁₉H₂₄O₅) to 0.746kg of benzene? The freezing point of pure benzene is 5.5°C. The freezing point constant for benzene is 5.12°C/m.

(Molar Mass: C: 12; H: 1.008, O: 16)

Fill in the Blanks

When 5.16g of an unknown molecular compound, was

dissolved in 40.0g of benzene, the freezing point of the solution was lowered to 5.23°C. What is the molar mass of unknown compound? (K_f benzene: 5.12°C/m)

EVALUATION

​Answer on sheets of whole paper

Fill in the Blanks

A solution that contains 12.6 g of a nonvolatile non-dissociating solute in 400 g of benzene freezes at 3.6°C The normal freezing point of benzene is 5.5 °C. What is the molar mass of the solute? (K_f for benzene is 4.96 °C kg/m)

Fill in the Blanks

Calculate the freezing point of a solution made from 32.7g of propane, C₃H₈, dissolved in 137.0g of benzene, C₆H₆. The freezing point of benzene is 5.50°C and its K_f is 5.12°C/m. (C: 12.01; H: 1.008)

Fill in the Blanks

Calculate the boiling point of a solution made from 227g of MgCl₂ dissolved in 700g of water. What is the boiling point of the solution?

K_b = 0.512°C/m. Find i from table previously given.

Reorder

Arrange the following steps on how to titrate for an unknown vinegar concentration

• Add a sample vinegar into a beaker.

• Withdraw 10.0 mL of vinegar from the 25.0 mL and transfer it to a 250 mL Erlenmeyer flask. Dilute to 50 mL with water.

• Add 1 drop of phenolphthalein as indicator.

• Titrate to the end point (solution must have a permanent faint pink color) with the standardized NaOH solution.

• Calculate the mass of acetic acid (CH3COOH) in the vinegar solution.

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