Chemistry Solutions

Question 1

A ___ consists of a solute (e.g., NaCl, NH3, or C12H22O11) dispersed (dissolved) in a solvent (e.g., H2O or benzene)

Answer 1

solution

Question 2

The ___ is the component of the solution whose phase remains the same after mixing

Answer 2

solvent

Question 3

If the two substances are already in the same phase, the ___ is the component present in greater quantity

Answer 3

solvent

Question 4

The interaction between solute and solvent molecules is known as ___ or dissolution

Answer 4

solvation

Question 5

Solvation is possible when the attractive forces between ___ and solvent are stronger than those between the solvent particles

Answer 5

solute

Question 6

Because water is ___, ion-dipole interactions can occur between the Na+ and Cl- ions and the water molecules, which are stronger and more favorable than the hydrogen-bonding found between H2O molecules in pure water

Answer 6

polar

Question 7

For nonionic ___, solvation involves van der Waals forces between the solute and solvent molecules

Answer 7

solutes

Question 8

The general ___ is that like dissolves like: ionic and polar solutes are soluble in polar solvents, and nonpolar solutes are soluble in nonpolar solvents

Answer 8

rule

Question 9

The summation of ___ associated with separating solute particles and solvent particles and combining solute with solvent particles is the energy of solvation, which if positive describes an endothermic process and if negative, an exothermic process

Answer 9

energy

Question 10

The ___ of a solute is measured in terms of the maximum amount of that solute that can be dissolved in a particular solvent at a particular temperature

Answer 10

solubility

Question 11

When the maximum amount of solute has been added, the solution is ___; if more solute is added, it will not dissolve

Answer 11

saturated

Question 12

Similarly, when a dissolved ___ comes out of solution and forms crystals, this process is known as crystallization

Answer 12

solute

Question 13

The solubility of a substance varies depending on the temperature of the ___, the solvent, and, in the case of a gas-phase solute, the pressure

Answer 13

solution

Question 14

Typically, the solubility of ___ or solids will increase with increasing temperature and the solubility of gas will increase with decreasing temperature and increasing pressure

Answer 14

liquids

Question 15

Some substances can form supersaturated solutions, which are ___ that contain more solute than found in a saturated solution

Answer 15

solutions

Question 16

Concentration denotes the amount of ___ dissolved in a solvent

Answer 16

solute

Question 17

A solution in which the proportion of solute to solvent is mall is said to be dilute, and one in which the ___ is large is said to be concentrated

Answer 17

proportion

Question 18

The ___ of a solution is most commonly expressed as percent composition by mass, mole fraction (X), molarity (M), molality (m), or normality (N)

Answer 18

concentration

Question 19

The ___ (X) of a compound is equal to the number of moles of the compound divided by the total number of moles of all species within the system

Answer 19

mole fraction

Question 20

X sub B = moles of B / sum of ___ of all components

Answer 20

moles

Question 21

The ___ (M) of a solution is the number of moles of solute per liter of solution

Answer 21

molarity

Question 22

___ depends on the total volume of the solution, not on the volume of solvent used to prepare the solution

Answer 22

molarity

Question 23

The ___ (m) of a solution is the number of moles of solute per kilogram of solvent

Answer 23

molality

Question 24

For ___ solutions at 25 degrees Celsius, the molality is approximately equal to the molarity because the density of water at this temperature is 1 kilogram per liter, but note that this is an approximation and true only for dilute aqueous solutions

Answer 24

dilute aqueous

Question 25

The ___ (N) of a solution is equal to the number of gram equivalent weights of solute per liter of solution

Answer 25

normality

Question 26

Normality is unique among concentration units in that it is ___ dependent

Answer 26

reaction

Question 27

One can calculate ___ by multiplying the molarity (M) of a solution by the number of equivalents per mol

Answer 27

normality

Question 28

A solution is ___ when solvent is added to a solution of higher concentration to produce a solution of lower concentration

Answer 28

diluted

Question 29

The ___ of a solution after dilution can be conveniently determined using the equation below: M sub i x V sub i = M sub f x V sub f where M is molarity, V is volume, and the subscripts i and f refer to initial and final values, respectively

Answer 29

concentration

Question 30

When water is the solvent, the dissolving process is called ___, and the resulting solution is known as an aqueous solution

Answer 30

hydration

Question 31

All salts of alkali metal ions (e.g., Li+, Na+, K+, Rb+, Cs+, Fr+) are water soluble All salts of the ammonium ion (NH4+) are water soluble All salts with chloride (Cl-), bromide (Br-), and iodide (I-) ions are water soluble, with the exception of salts containing Ag+, Pb2+, and Hg2 2+ All ___ of the sulfate ion (SO4 2-) are water soluble, with the exception of those containing Ca2+, Sr2+, Ba2+, and Pb2+

Answer 31

salts

Question 32

Pure water does not conduct an ___ well, since the concentrations of hydrogen and hydroxide ions are very small

Answer 32

electrical current

Question 33

___ that make conductive solutions are called electrolytes

Answer 33

solutes

Question 34

Strong ___ include ionic compounds, such as NaCl and KI, and molecular compounds with highly polar covalent bonds that dissociate into ions when dissolved, such as HCl in water

Answer 34

electrolytes

Question 35

A ___, on the other hand, ionizes or hydrolyzes incompletely in aqueous solution, and only some of the solute is present in ionic form

Answer 35

weak electrolyte

Question 36

Many ___ do not ionize at all in aqueous solution, retaining their molecular structure in solution, which usually limits their solubility

Answer 36

compounds

Question 37

___ which retain their structure in aqueous solution are called nonelectrolytes and include many nonpolar gases and organic compounds such as oxygen and sugar

Answer 37

compounds