522 g of K2SO4 in 1.5 of solution
Answers
Answer:
The bold, underlined words are important vocabulary words that you should be able to define and use properly in
explanations. This is a study guide for what you will be tested on throughout the year. The objectives are divided into
categories of “Knowledge” (what you have to know) and “Application” (what you have to be able to do).
PHYSICAL BEHAVIOR OF MATTER – AQUEOUS SOLUTIONS
Knowledge Application
1. o Physical processes, such as a compound dissolving in a
solution, can be exothermic or endothermic.
o Interpret ∆H values for physical
processes given in Table I
2.
o A solution is a homogeneous mixture of a solute dissolved in a
solvent.
o Identify the solute and the solvent
in a given solution
o Give examples of different types
of solutions
o The solubility of a solute in a given amount of solvent is
dependent on the temperature, the pressure, and the chemical
natures of the solute and solvent.
o General rules:
a. solubility of a solid increases as temperature increases
(direct relationship)
b.solubility of a gas decreases as temperature increases
(inverse relationship)
c. solubility of a gas increases as pressure increases (direct)
d. “like dissolves like” – polar solvents dissolve polar solutes;
nonpolar solvents dissolve nonpolar solutes
o Predict the effect of temperature,
pressure, and nature of solvent on
solubility for a given solute
o Use a solubility curve to
distinguish among unsaturated,
saturated, and supersaturated
solutions
o Calculate the amount of a specific
solute dissolved at different
temperatures using Table G
3.
o Many chemical reactions happen in solution. When different
ionic compounds are mixed together in the same solution, a
double replacement reaction may occur and a stable precipitate
(insoluble/solid compound) may form.
o Use Table F (Solubility
Guidelines) to determine a
compound’s solubility
o Determine if a precipitate will
form when ionic compounds are
mixed in solution
o Write and balance chemical
equations for double replacement
reactions
4.
o The concentration of a solution may be expressed as:
molarity (M), percent by volume (%v/v), percent by mass
(%m/v), or parts per million (ppm).
o Calculate solution concentrations
in molarity (M), percent by
volume, percent by mass, or parts
per million (ppm)
o Describe how you would prepare a
solution from scratch, given the
desired molarity
o Describe how you would dilute a
solution of known concentration
(must use the equation M1V1 =
M2V2)