14. Solutions

Types of Aqueous Solutions

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

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.)

Electrolytes: Definition, Examples, & Practice

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.

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.)

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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[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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