Chapter 9: Solutions

Question 1

Solvation is an (endothermic/exothermic?) process when the new interactions are stronger than the original ones. This is favored at low temperatures.

Answer 1

exothermic

Question 2

Solvation is an (endothermic/exothermic?) process when the new interactions are weaker than the original ones. This is favored at high temperatures.

Answer 2

endothermic

Question 3

what does solvation do?

Answer 3

breaks intermolecular interactions between solute molecules and between solvent molecules and forming new intermolecular interactions betweeen solute and solvent molecules together

Question 4

At constant temperature and pressure, ________ always increases upon dissolution.

Answer 4

entropy

Question 5

When the change in Gibbs free energy for the dissolution reaction is negative at a given temperature, the process will be ____________ and the solute is ____________. If positive, the process is ________________ and the solute is ____________.

Answer 5

spontaneous; soluble
nonspontaneous; insoluble

Question 6

The most common type of solution is the ____________ solution, in which the solvent is water.

Answer 6

aqueous

Question 7

Some solutions, such as acids, the formation of a complex called the ____________ ________ can occur. This occurs how?

Answer 7

hydronium ion (H3O+); H+ is donated from the molecule in solution to a water molecule

Question 8

All salts containing ammonium (NH4+) and alkali metals are ____________.

Answer 8

soluble

Question 9

All salts containing nitrate (NO3-) and acetate (CH3COO-) anions are ____________

Answer 9

soluble

Question 10

Halides except fluorides are ________, except for those formed with which elements?

Answer 10

soluble; Ag+, Pb^{2+, and Hg₂₂₊}

Question 11

All salts of the sulfate ion (SO4^{2+) are ____________, except for those formed with which elements?}

Answer 11

soluble; Ca^{2+, Sr2+, Ba2+, and Pb2+}

Question 12

All metal oxides are ____________, except for those formed with which things?

Answer 12

insoluble;
1. alkali metals
2. ammonium
3. CaO, SrO, and BaO

THese all hydrolyze to form solutions of the corresponding metal hydroxides

Question 13

All hydroxides are ____________, except for those formed with which things?

Answer 13

insoluble;
1. alkali metals
2. ammonium
3. Ca^{2+, Sr2+, and Ba2+}

Question 14

All carbonates (CO3^{2-), phosphates (PO43-), sulfides (SO32-) are ____________ except for those formed with which things?}

Answer 14

insoluble;
1. alkali metals
2. ammonium

Question 15

ON MCAT, please know

Which 2 groups are always soluble?

Answer 15

1. All salts of Group 1 metals
2. All nitrate salts

Question 16

________ and ________ ions are generally used as counterions to what is actually chemically important. Meaning, focus on the positive cation as the chemically reacting species.

Answer 16

sodium, nitrate

Question 17

A ________ ion, or ____________ ____________, refers to a molecule in which a cation is bonded to at least one electron pair donor (which could include the water molecule)

Answer 17

complex; coordination compound

Question 18

The electron pair donor molecules in coordination compounds are called ________.

Answer 18

ligands

e.g. The classic ligands that reversibly bind to hemoglobin, dioxygen, carbon dioxide, and protons, are bound covalently

Question 19

Complexes are held together with ____________ ____________ bonds, in which an electron pair donor (a Lewis base) and an electron pair acceptor (a Lewis acid) form very stable Lewis acid-base adducts.

Answer 19

coordinate covalent

Question 20

In some complexes, the central cation can be bonded to the same ligand in multiple places. This is called ____________, and it generally requires large organic ligands that can double back to form a second (or even third) bond with the central cation.

Answer 20

chelation

Question 21

The normality (N) of a solution is equal to what?

Answer 21

The number of equivalents of interest per liter of solution

Question 22

An equivalent is a measure of what? What is it equal to?

Answer 22

A measure of the reactive capacity of a molecule; it is equal to a mole of the species of interest

e.g. 1 mol of permanganate ion in acidic solution will readily accept 5 mol of e-, so a 1M solution would be 5 N

Question 23

In solubility equations, equilibrium is defined as what?

Answer 23

The saturation point, where the solute concentration is at its maximum value for the given temp and pressure

Question 24

What is molar solubility?

Answer 24

the concentration at saturation

Question 25

____________ properties are physical properties of solutions that are dependent on the concentration of dissolved particles but not on the chemical identity of the dissolved particles.

Answer 25

colligative

Question 26

Raoult’s law accounts for what?

Answer 26

vapor pressure depression caused by solutes in solution

Question 27

On a molecular level, the presence of solute molecules can do what to evaporation? How about condensation?

Answer 27

block evaporation of solvent molecules; does not affect condensation

Question 28

When a nonvolatile solute is dissolved into a solvent to create a solution, the boiling point of the solution will be (greater/less) than that of the pure solvent/

Answer 28

greater

Question 29

what is the van’t Hoff factor?

Answer 29

the number of particles into which a compound dissolves into solution

Question 30

The presence of solute particles interferes with the formation of lattice arrangement of solvent molecules associated with solid state. So, ____________ point is lowered with solute.

Answer 30

freezing

Question 31

____________ ____________ refers to a “sucking” pressure generated by solutions in which water is drawn into solution. It is the amount of pressure that must be applied to counteract this attrattion of water molecules for the solution.

Answer 31

osmotic pressure