General Chemistry Ch 9. Solutions

Question 1

Solutions

Answer 1

Homogenous mixtures composed of two or more substances, combine to form a single phase, generally the liquid phase

Question 2

Solvent

Answer 2

Particles that surround solute particles via electrostatic interactions in a process called salvation or dissolution

Question 3

Solute

Answer 3

Particles surrounded by solvent particles via electrostatic interactions in a process called solvation or dissolution

Question 4

Solvation

Answer 4

aka dissolution, process where solvent particles surround solute particles via electrostatic interaction, most endothermic although dissolution of gas into liquid is exothermic

Question 5

Dissolution

Answer 5

aka solvation, process where solvent particles surround solute particles via electrostatic interaction, most endothermic although dissolution of gas into liquid is exothermic

Question 6

Aqueous solutions

Answer 6

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Question 7

Hydration

Answer 7

Solvation in water

Question 8

Solubility

Answer 8

The maximum amount of solute that can be dissolved in a given solvent and a given temperature, it is often expressed as molar solubility

Question 9

Molar solubility

Answer 9

The molarity of the solute at saturation

Question 10

Complex ions

Answer 10

aka coordination compounds, composed of metallic ions bonded to various neural compounds and anions, referred to as ligands, formation of them increases the solubility of otherwise insoluble ions (opposite of common ion effect), formation of the involves electron pair donors and electron pair acceptors similarly to coordinate covalent bonding

Question 11

Coordination compounds

Answer 11

aka complex ions, composed of metallic ions bonded to various neural compounds and anions, referred to as ligands, formation of them increases the solubility of otherwise insoluble ions (opposite of common ion effect), formation of the involves electron pair donors and electron pair acceptors similarly to coordinate covalent bonding

Question 12

Coordinate covalent bonding

Answer 12

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Question 13

Percent composition by mass

Answer 13

Mass of solute per mass of solution times 100, used for aqueous solutions and solid in solid solutions

Question 14

Mole fraction

Answer 14

Moles of solute per total moles, used for calculating vapor pressure depression and partial pressures of gases in a system

Question 15

Molarity

Answer 15

Moles of solute per liters of solution, most common unit for concentration and is used for rate laws, the law of mass action, osmotic pressure, pH and pOH, and the Nernst equation

Question 16

Molality

Answer 16

Moles of solute per kilograms of solvent, used for boiling point elevation and freezing point depression

Question 17

Normality

Answer 17

Number of equivalents per liters of solution, the molarity of the species of interest and is used for acid-base and oxidation-reduction reactions

Question 18

Saturated solutions

Answer 18

Are in equilibrium at that particular temperature

Question 19

Solubility product constant (Ksp)

Answer 19

Simple the equilibrium constant for a dissociation reaction

Question 20

Ion product (IP)

Answer 20

Can compare to Ksp to determine the level of saturation and behavior of the solution

Question 21

IP

Answer 21

The solution is unsaturated, and if more solute is added, it will dissolve

Question 22

IP=Ksp

Answer 22

The solution is saturated (at equilibrium) and there will be no change in concentrations

Question 23

IP>Ksp

Answer 23

The solution is supersaturated and a precipitate will form

Question 24

Formation or stability constant (Kf)

Answer 24

The equilibrium constant for complex formation, usually much greater than Ksp, increases the solubility of other salts containing the same ions because it uses up the products of those dissolution reactions, shifting the equilibrium to the right (opposite of common ion)

Question 25

Common ion effect

Answer 25

Decreases the solubility of a compound in a solution that already contains one of the ions in the compound, the presence of that ion in solution shifts the dissolution to the left, decreasing its dissociation

Question 26

Colligative properties

Answer 26

Physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity

Question 27

Vapor pressure depression

Answer 27

Follows Raoult’s law, the presence of other solutes decreases the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure, also explains boiling point elevation - as the vapor pressure decreases, the temperature (energy required to boil the liquid must be raised)

Question 28

Freezing point depression

Answer 28

Shift in the phase equilibria dependent on the molality of the solution

Question 29

Boiling point elevation

Answer 29

Shifts in the phase equilibria dependent on the molality of the solution

Question 30

Osmotic pressure

Answer 30

Primarily dependent on the molarity of the solution

Question 31

Van’t Hoff factor (i)

Answer 31

For solutions that dissociate, this can be used in freezing point depression, boiling point elevation, and osmotic pressure calculations