Chemistry Solutions Flashcards
A ___ consists of a solute (e.g., NaCl, NH3, or C12H22O11) dispersed (dissolved) in a solvent (e.g., H2O or benzene)
solution
The ___ is the component of the solution whose phase remains the same after mixing
solvent
If the two substances are already in the same phase, the ___ is the component present in greater quantity
solvent
The interaction between solute and solvent molecules is known as ___ or dissolution
solvation
Solvation is possible when the attractive forces between ___ and solvent are stronger than those between the solvent particles
solute
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
polar
For nonionic ___, solvation involves van der Waals forces between the solute and solvent molecules
solutes
The general ___ is that like dissolves like: ionic and polar solutes are soluble in polar solvents, and nonpolar solutes are soluble in nonpolar solvents
rule
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
energy
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
solubility
When the maximum amount of solute has been added, the solution is ___; if more solute is added, it will not dissolve
saturated
Similarly, when a dissolved ___ comes out of solution and forms crystals, this process is known as crystallization
solute
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
solution
Typically, the solubility of ___ or solids will increase with increasing temperature and the solubility of gas will increase with decreasing temperature and increasing pressure
liquids
Some substances can form supersaturated solutions, which are ___ that contain more solute than found in a saturated solution
solutions
Concentration denotes the amount of ___ dissolved in a solvent
solute
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
proportion
The ___ of a solution is most commonly expressed as percent composition by mass, mole fraction (X), molarity (M), molality (m), or normality (N)
concentration
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
mole fraction
X sub B = moles of B / sum of ___ of all components
moles
The ___ (M) of a solution is the number of moles of solute per liter of solution
molarity
___ depends on the total volume of the solution, not on the volume of solvent used to prepare the solution
molarity
The ___ (m) of a solution is the number of moles of solute per kilogram of solvent
molality
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
dilute aqueous
The ___ (N) of a solution is equal to the number of gram equivalent weights of solute per liter of solution
normality
Normality is unique among concentration units in that it is ___ dependent
reaction
One can calculate ___ by multiplying the molarity (M) of a solution by the number of equivalents per mol
normality
A solution is ___ when solvent is added to a solution of higher concentration to produce a solution of lower concentration
diluted
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
concentration
When water is the solvent, the dissolving process is called ___, and the resulting solution is known as an aqueous solution
hydration
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+
salts
Pure water does not conduct an ___ well, since the concentrations of hydrogen and hydroxide ions are very small
electrical current
___ that make conductive solutions are called electrolytes
solutes
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
electrolytes
A ___, on the other hand, ionizes or hydrolyzes incompletely in aqueous solution, and only some of the solute is present in ionic form
weak electrolyte
Many ___ do not ionize at all in aqueous solution, retaining their molecular structure in solution, which usually limits their solubility
compounds
___ which retain their structure in aqueous solution are called nonelectrolytes and include many nonpolar gases and organic compounds such as oxygen and sugar
compounds
