Chapter 15

Front 1

Which of the following solutes will generally not dissolve in the specified solvent? (Assume all of the compounds are in the liquid state)

Back 1

CCl4 mized with water (H2O)

Front 2

Which of the following illustrates the like dissolves like rule for two liquids?

Back 2

-A polar solvent is miscible with polar solvent.
-A nonpolar solvent is miscible with nonpolar solvent.
-A polar solvent is immiscible with nonpolar solvent.
(All of the above)

Front 3

You have two HCl solutions, labeled Solution A and Solution B. Solution A has a greater concentration than Solution B. Which of the following statements is true?

Back 3

If you have equal moles of HCl in both solutions, Solution B must have a greater volume.

Front 4

A 0.50 M solution of sodium chloride in an open beaker sits on a lab bench. Which of the following would decrease the concentration of the salt solution?

Back 4

Add water to the solution

Front 5

A solution is?

Back 5

a homogeneous mixture

Front 6

Solution =

Back 6

Solution = Solute (lesser part) + Solvent (greater part)

Front 7

Solutions and mixtures

Back 7

Amounts of substances can vary in different solutions

Specify the amounts of solvent and solutes.
Qualitative measures of concentration
- concentrated - relatively large amount of solute
- dilute - relatively small amount of solute

Front 8

Solution Composition: Percent by Mass

Back 8

Mass percent = mass of solute / mass of solution * 100%

mass percent = grams of solute / grams of solute + grams of solvent * 100%

Front 9

Standard Solution

Back 9

A solution whose concentration is accurately known

Front 10

Steps for making a standard solution

Back 10

1. Weigh out a sample of solute
2. Transfer to a volumetric flask
3. Add enough solvent to mark on flask

Front 11

Dilution

Back 11

-Process of adding water to a concentrated or stock solution to achieve molarity desired for a particular solution.
-Dilution w/water does not alter the number of moles of solute present. Moles of solute before dilution = moles of solute after dilution.
M1V1=M2V2

Front 12

Steps for Solving Stoichiometric Problems Involving Solutions

Back 12

1. Write the balanced equation for the reaction. For reactions involving ions, it is best to write the net ionic equation.
2. Determine which reactant is limiting in the usual manner.
3. Calculate the moles of other reactants or products, as required and convert to grams or other units, if required.

Front 13

Neutralization Reaction

Back 13

An acid base reaction is called a Neutralization Reaction. Steps to solve these problems are the same as before.

Front 14

Gas Summary

Back 14

Gas solubility decreases as the temp increases.
Gas solubility increases as the pressure increases.

Front 15

When determining whether a substance will be soluble in a given solvent, apply the like dissolves like rule

Back 15

-Polar molecules dissolve in polar solvent.
-Nonpolar molecules dissolved in nonpolar solvents

Front 16

Saturated solution

Back 16

contains as much solute as will dissolve at that temperature

Front 17

Unsaturated solution

Back 17

has not reached the limit of solute that will dissolve

Front 18

Supersaturated solution

Back 18

occurs when a solution is saturated at an elevated temp and then allowed to cool but all of the solid remains dissolved.

Front 19

Three factors can increase the rate of dissolving for a solute:

Back 19

-heating the solution
-stirring the solution
-grinding the solid solute