Chemistry Test Review – Water and Solubility
Water:
1. ______Hydrogen_______ bonding occurs when the positive hydrogen end and the negative oxygen
end of the water molecule attract.
2. Hydrogen bonding is responsible for which three unique characters of water?
High Boiling Point, High surface tension, More dense as a liquid than a solid
3. What is surface tension? Give an example Surface tension is the inward force that minimizes the
surface area of a liquid; surface tension allows water bugs to walk on the surface of the water
4. A _____surfactant_____ decreases surface tension
5. What is considered the universal solvent? Water
6. Draw the molecule of water and indicate the polar ends of water.
Types of Mixtures
1. Rank the terms “Suspension” “Solution” and “Colloid” in order of smallest particle size to largest
particle size.
Solutions have the smallest particles, Colloids are in between and Suspensions have the largest
perticles
2. Define Tyndall Effect. What two types of mixtures can it be used to distinguish from each other?
The Tyndall Effect states that light scatters as it is shined through a colloid. This distinguishes
between colloids and solutions.
3. What is a solution considered if it conducts electricity? If it does not conduct electricity?
Electrolytes conduct electricity and Nonelectrolytes do not conduct electricity
The Solution Process
1. In sweet tea, what would be the solute and what would be the solvent?
Solute – Tea & Sugar
Solvent – Water
2. Define saturated solution.
A saturated solution has dissolved all of the solute it can hold at a given temperature; it’s full
3. Explain how you can make a supersaturated solution.
Supersaturated solutions require both heating and stirring to dissolve more solute than it should
theoretically hold.
4. What are the three factors that increase the rate of dissolving a solute?
Stirring the solution, Heating the solution, Crushing the solute
Solubility Chart
Use the solubility chart to the left to answer the following
questions.
1. How much KNO3 should be able to dissolve at 65oC in 100
g of water? About 118 g
2. Which compound’s solubility changes the least as the
temperature is increased? NaCl changes the least
3. Which compound has the lowest solubility at 50oC? At
10oC? At 50°C = Ce2(SO4)3 At 10°C = KClO3
4. At what temperature can only 80 g of NaNO3 dissolve in
100 g of water? 10°C
5. If you dissolved exactly 100 g of KCl in 100 g of water at
80oC, would the solution be saturated, unsaturated, or
supersaturated? Supersaturated
5. If you dissolved 125 g of NaNO3 at 60 oC and then
cooled the solution down to 40 oC, what would the solution
be considered? Saturated, unsaturated, or supersaturated?
Supersaturaed
Solubility Rules
Use your solubility chart for the following questions
1. Label the following as soluble or insoluble
a. CaSO4 Soluble
b. AgBr Insoluble
c. NH4OH Soluble
d. BaCO3 Insoluble
2. A _______Precipitate________ is an insoluble solid that forms in a chemical reaction.
3. Predict if the following reactions would form a precipitate. Write either “precipitate” or “no
precipitate” in the blank. If there is a precipitate, circle it!
a. LiOH + AgNO3  AgOH + LiNO3
________Precipitate_________
b. FeS + NaNO3  Na2 S
_______No Precipitate_______
+ Fe(NO3)2
Concentration
Show your work and circle your answer.
4. What is the molarity of a solution that contains 5.8 Liters of water and 9.4 grams of NaNO3?
9.4 g NaNO3 x 1 mole = 0.111 moles
84.994 g
M = moles
L
M = 0.111 moles
5.8 L
M = 0.0191 M
5. How many moles of solute are needed to make a 3.0M solution with 5Liters of water?
moles = Molarity x Liters
moles = 3.0 M x 5 L
moles = 15.0 moles
6. If I have 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be if I
diluted to 250 mL ?
M2 = M1V1
V2
M2 = 0.15 x 125
250
M2 = 0.075 M
7. What volume is needed to make a 4.5 M solution if it was diluted from 8.0 M of 2.0 L?
V2 = M1V1
M2
V2 = 8.0 x 2.0
4.5
V2 = 3.56 L