14. Solutions

Freezing Point Depression

Boiling point elevation and freezing point depression | Chemistry | Khan Academy

What mass of salt (NaCl) should you add to 1.00 L of water in an
ice cream maker to make a solution that freezes at -10.0 °C?
Assume complete dissociation of the NaCl and density of 1.00 g>mL for water.

Use the van’t Hoff factors in Table 13.9 to calculate each colligative property:
a. the melting point of a 0.100 m iron(III) chloride solution

Elemental analysis of b@carotene, a dietary source of vitamin A, shows that it contains 10.51% H and 89.49% C. Dissolving 0.0250 g of b@carotene in 1.50 g of camphor gives a freezing- point depression of 1.17 °C. What are the molecular weight and formula of b@carotene? [Kf for camphor is 37.7 1°C kg2>mol.]

13 - Solutions and Colligative Properties

An ethylene glycol solution contains 28.3 g of ethylene glycol, C2H6O2 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

Freezing Point Depression Concept 1

Calculate the freezing point and boiling point of each aqueous
solution, assuming complete dissociation of the solute.
c. 5.5% NaNO3 by mass (in water)

Freezing Point Depression Example 1

Molality and Colligative Properties

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of
the resulting solution was - 3.53 °C.
(f) What is the identity of the metal M?

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of
the resulting solution was - 3.53 °C.
(c) What is the molality of particles (ions) in the solution of MClx?

A small cube of lithium 1density = 0.535 g/cm32 measuring 1.0 mm on each edge is added to 0.500 L of water. The 
following reaction occurs: 
2 Li1s2 + 2 H2O1l2 ¡ 2 LiOH1aq2 + H21g2 
What is the freezing point of the resulting solution, assuming that the reaction goes to completion?

How many moles of ethylene glycol, C2H6O2, must be added to 1,000 g of water to form a solution that has a freezing point of –10ºC?

A solution prepared by dissolving 3.00 g of ascorbic acid (vitamin C, C6H8O6) in 50.0 g of acetic acid has a freez- ing point that is depressed by ΔT = 1.33 °C below that ofpure acetic acid. What is the value of the molal freezing- point-depression constant for acetic acid?

Colligative Properties Explained

A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g 
of water. Determine the freezing point and boiling point of the 
solution.

When 825 g of an unknown is dissolved in 3.45 L of water, the freezing point of the solution is decreased by 2.89°C. Assuming that the unknown compound is a non-electrolyte, calculate its molar mass.

Freezing Point Depression Explained - Clutch Prep Chemistry

Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

A solution prepared by dissolving 100.0 g of a mixture of sugar 1C12H22O112 and table salt (NaCl) in 500.0 g of water has a freezing point of - 2.25 °C. What is the mass of each individual solute? Assume that NaCl is completely dissociated.

Calculate the freezing point and boiling point of each aqueous
solution, assuming complete dissociation of the solute.
b. 21.5 g of CuCl2 in 4.50 * 102 g water

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of
the resulting solution was - 3.53 °C.
(e) What are the formula and molecular weight of MClx?

A solution contains 10.05 g of unknown compound dissolved 
in 50.0 mL of water. (Assume a density of 1.00 g>mL for water.) 
The freezing point of the solution is -3.16 °C. The mass percent 
composition of the compound is 60.97% C, 11.94% H, and the 
rest is O. What is the molecular formula of the compound?

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 0.240 mol of naphthalene 1C10H82 in 2.45 mol of chloroform, g glucose 1C6H12O62 in 188 g of water.

124. A 50.0-mL solution is initially 1.55% MgCl2 by mass and 
has a density of 1.05 g>mL. What is the freezing point of the 
solution after you add an additional 1.35 g MgCl2? 
(Use i = 2.5 for MgCl2.)

The van’t Hoff factor for CaCl2 is 2.71. What is its mass % in an aqueous solution that has Tf = - 1.14 °C?

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 20.0 g of decane, C10H22, in 50.0 g CHCl3;

When HNO2 is dissolved in water, it partially dissociates according
to the equation HNO2ΔH+ + NO2- . A solution is prepared
that contains 7.050 g of HNO2 in 1.000 kg of water. Its
freezing point is -0.2929 °C. Calculate the fraction of HNO2
that has dissociated.

Lauryl alcohol is obtained from coconut oil and is used to 
make detergents. A solution of 5.00 g of lauryl alcohol in 
0.100 kg of benzene freezes at 4.1 °C. What is the molar 
mass of lauryl alcohol from this data?

What is the freezing point of an aqueous solution that boils
at 105.0 °C?

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[BOOK CHEM] Clutch Version

Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

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