14. Solutions

Types of Aqueous Solutions

Electrolytes: Definition, Examples, & Practice

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of
water at 40 °C will lead to a saturated solution: (d) Pb1NO322.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/f21630295cff4938-1666023636192.jpg" alt="" />

What Are Electrolytes?

By referring to Figure 13.15, determine the mass of each
of the following salts required to form a saturated solution in 250 g of water at 30 °C: (c) Ce21SO423.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/6bf5b87a799f7ced-1666023481365.jpg" alt="" />

By referring to Figure 13.15, determine the mass of each
of the following salts required to form a saturated solution in 250 g of water at 30 °C: (b) Pb1NO322,<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b570cb09894e89c8-1666023407838.jpg" alt="" />

Types of Aqueous Solutions Example 1

A KCl solution containing 42 g of KCl per 100.0 g of water is
cooled from 60 °C to 0 °C. What happens during cooling? (Use
Figure 13.11.)<img src="https://lightcat-files.s3.amazonaws.com/problem_images/c848c8ef6799a3e9-1660314901253.jpg" alt="" />

The molarity of a solution of sodium acetate (CH3COONa) at 20 C is 7.5 M. Use the graph showing the solubility of sodium acetate as a function of temperature to describe the solution. The solution is . (LO 13.7, 13.8) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/3cc4d3e3ce88918f-1671636852929.jpg" alt="" /> (a) Saturated (b) Unsaturated (c) Supersaturated (d) Colloidal

The Strong Electrolytes

A KNO3 solution containing 45 g of KNO3 per 100.0 g of water is 
cooled from 40 °C to 0 °C. What happens during cooling? (Use 
Figure 13.11.)

Indicate whether each statement is true or false:
(d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the 
solution even more concentrated.

Identifying Strong Electrolytes, Weak Electrolytes, and Nonelectrolytes - Chemistry Examples

The following pictures represent solutions of AgCl, which also may contain ions other than Ag+ and Cl- that are not shown. If solution 1 is a saturated solution of AgCl, classify solutions 2–4 as unsaturated, saturated, or supersaturated.
 
(1) 
(2) 
(3) 
(4)

A solution contains 25 g of NaCl per 100.0 g of water at 25 °C. Is
the solution unsaturated, saturated, or supersaturated? (Use
Figure 13.11.)<img src="https://lightcat-files.s3.amazonaws.com/problem_images/0bbbc5269f9f31ad-1660314826390.jpg" alt="" />

How to Identify Strong, Weak, and Non-Electrolytes Examples & Practice Problems

Water & Solutions - for Dirty Laundry: Crash Course Chemistry #7

The solubility of KClO3 in water at 30ºC is 10 g per 100 mL of water. A 0.95 M solution of KClO3 in water at 30ºC is:

A solution contains 32 g of KNO3 per 100.0 g of water at 25 °C. 
Is the solution unsaturated, saturated, or supersaturated? (Use 
Figure 13.11.)

Correct, 0.990 M corresponds to 11.3 g KNO3per 100 g water.

0.990 M corresponds to 11.3 g KNO3per 100 g water.

Use the molar mass of the solute and density of the solution to convert the molarity to the equivalent concentration in g KNO3 per 100 g of water.

 If the concentration of the solution is equal to the solubility, the solution is saturated; lower than this value, the solution is unsaturated, and higher than this value, supersaturated. 

At 88 &#176;C the solubility of KNO3 is 88 g per 100 g of water. Would a solution that has a molarity of 0.990 M KNO3 and a density of 0.988 g/mL be considered unsaturated, saturated, or supersaturated?

Types of Aqueous Solutions Concept 1

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of
water at 40 °C will lead to a saturated solution:(c) K2Cr2O7<img src="https://lightcat-files.s3.amazonaws.com/problem_images/fced9c5898fecb10-1666023593146.jpg" alt="" />

Types of Aqueous Solutions Concept 2

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4. BONUS: Lab Techniques and Procedures

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[BOOK CHEM] Clutch Version

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

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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