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WorksheetsUnit 9/10: Solutions, Acids, and Bases
Total questions: 15
Worksheet time: 17mins
The solubility graph shows a number of solutes dissolved in 100 g of water:
At what temperature are equal amounts of sodium chloride and potassium chlorate dissolve in 100g of water?
80oC
25oC
72oC
7oC
A graph of the solubility of several compounds is shown:
Which of these would result in a supersaturated solution at 50 oC when dissolved in 100 g of water?
30 g NaCl
50g KCl
80 g KNO3
100g NaNO3
In a colligative properties experiment, a lab group prepares four solutions. What must they also prepare too make their experiment testable?
A pure solvent sample to allow the lab group to predict the colligative properties of the solvent.
A pure solvent sample to rule out phase changes as a source of error.
A pure solvent sample to serve as the control for the experiment.
A pure solvent sample to help the lab group remember what solvent is being used in the experiment.
Which type of mixture forms when calcium chloride is completely dissolved in water?
compound
solution
colloid
suspension
When a student performs an acid-base test on a household cleaner, phenolphthalein turns pink. Based on the results, which statement is a valid conclusion?
It is an acid.
It is a base.
It is neutral.
It is a salt.
Which type of mixture forms when sand is mixed with water?
compound
solution
colloid
suspension
A student received three 100 mL samples of Ammonium Nitrate solution and measured the boiling points using a thermometer, a hot plate, and a fume hood. The results are presented in the table.
Which statement most likely explains the differences in the sample boiling points?
The hot plate was heated at different temperatures.
The solute concentrations were different for each sample.
The sample volumes were measured differently.
The samples were heated for different lengths of time.
If a solution contains 250.0 mL of a 0.82 M solution of Barium Fluoride how many grams of magnesium iodide are in the solution?
0.205g
32g
575g
36g
Which of the following solutions will have the lowest concentration?
2 moles of solute dissolved in 1 liter of solution
0.3 mole of solute dissolved in 0.6 liter of solution
2 moles of solute dissolved in 15 liters of solution
0.1 mole of solute dissolved in 0.5 liter of solution
How many kilograms of solution would you have if you used 75.0 moles of NaOH to make a 1.50 molal solution?
50.00 kg
53.00 kg
112.50 kg
115.50
1.7 x 106 kg of pond water contained 0. 78 kg of lead ions. What is the concentration of lead ions in the pond in ppm?
ppm = mg solute / L solution
Density of pond water ≅ 1.00 g/mL
4.59x10-7 ppm
4.59x10-4 ppm
0.459 ppm
0.0459 ppm
What is the main factor resulting in a lower freezing point of a solvent after solute has been dissolved in the solvent?
How many particles are in the solution.
The type of metal in the solute compound.
The type of non-metal in the solute compound.
The original freezing point of the solvent.
What is the difference between molarity and molality?
Molarity involves liters of solution and molality involves kg of solvent.
Molality involves liters of solution and molarity involves kg of solvent.
Molarity involves liters of solute and molality involves kg of solvent.
Molarity involves liters of solution and molality involves kg of solute.
All of the following will allow a solute to dissolve slower in a solvent EXCEPT.
Heating the solvent.
Cooling the solute.
Increasing the pressure over the solvent.
Making the solute into large cubes before adding them to the solvent.
Which of the solute's solubility decreases with increasing temperature?
CHOOSE ALL THAT APPLY!
NH3
NaCl
Ce2(SO4)3
KClO3
KCl
