Chemistry Solutions Flashcards

1
Q

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

A

solution

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2
Q

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

A

solvent

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3
Q

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

A

solvent

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4
Q

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

A

solvation

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5
Q

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

A

solute

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6
Q

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

A

polar

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7
Q

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

A

solutes

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8
Q

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

A

rule

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9
Q

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

A

energy

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10
Q

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

A

solubility

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11
Q

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

A

saturated

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12
Q

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

A

solute

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13
Q

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

A

solution

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14
Q

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

A

liquids

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15
Q

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

A

solutions

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16
Q

Concentration denotes the amount of ___ dissolved in a solvent

A

solute

17
Q

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

A

proportion

18
Q

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

A

concentration

19
Q

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

A

mole fraction

20
Q

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

A

moles

21
Q

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

A

molarity

22
Q

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

A

molarity

23
Q

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

A

molality

24
Q

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

A

dilute aqueous

25
Q

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

A

normality

26
Q

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

A

reaction

27
Q

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

A

normality

28
Q

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

A

diluted

29
Q

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

A

concentration

30
Q

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

A

hydration

31
Q

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+

A

salts

32
Q

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

A

electrical current

33
Q

___ that make conductive solutions are called electrolytes

A

solutes

34
Q

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

A

electrolytes

35
Q

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

A

weak electrolyte

36
Q

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

A

compounds

37
Q

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

A

compounds