Worksheets9.1-8 | Unit 9 Review
Total questions: 25
Worksheet time: 1hrs 15mins
How much KNO3 solute is saturated at 40 degrees?
75g
55g
65g
85g
Which solute is MOST likely a gas?
KNO3
NaNO3
KCl
Ce2(SO4)3
At what temperature can you fully dissolve 140g of NaNO3?
62 °C
73 °C
81 °C
You cannot determine this
What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
Which would NOT increase the rate at which a sugar cube dissolves?
Reducing the amount of solvent
Crushing the sugar cube
Stirring the solution
Heating the solvent
You can make a solute dissolve more quickly in a solvent by
adding more solute.
adding ice.
heating the solvent.
removing some solvent.
A solution that contains all of the solute it can hold at a given temperature is
diluted.
saturated.
supersaturated.
unsaturated.
Three 10 g samples of sugar are represented below.
Sample A dissolves in water more slowly than sample B.
Sample B dissolves more slowly than sample C.
Which of the following best explains why sample A dissolves more slowly than the other two?
It has the most volume.
It has the smallest surface area.
It has the largest number of sugar molecules.
It has the fewest bonds between sugar modules.
A technican prepared a solution by heating 100 mL of distilled water while adding KCl crystals until no more KCl would dissolve. She then capped the clear solution and set it aside on the lab counter. After several hours she noticed the solution had become cloudly and some solid had settled to the bottom of the flask. Which statement best describes what happened?
As the solution cooled, evaporation of water increased the KCl concentration beyond its solubility.
Water molecules, trapped with the KCl crystals, were released after heating.
At lower temperatures the solubility of KCl decreased and recrystallization occurred.
At increased temperatures the solubility of KCl increased and remained too high after cooling.
A solution that is able to dissolve additional solute is best described as
supersaturated.
concentrated.
saturated
unsaturated.
What is the molarity of 4 g of NaCl in 3,800 mL of solution?
0.02 M
0.001 M
1 M
0.06 M
Diluting a solution:
increases the solvent, but not solute
increases the solute, but not solvent
increases both the solute and solvent
doesn't do anything to the solute or solvent
Which sweet tea would you expect to taste the sweetest?
1.0 M
3.0 M
3.1 M
2.5 M
What molarity of 50.0 mL Cu(NO3)2 is needed to make 300.0 mL of 0.25 M concentration?
6.0 x 104 M
0.042 M
1.5 M
6.0 M
What volume of 5.0 M AgNO3 is needed to make 250.0 mL of 1.25M?
0.025 mL
1.0 x 103 mL
63 mL
40. mL
Allowing a solution to evaporate will:
decrease the solvent and changes the solute
increase the solvent but not change the solute
decrease the solvent but not change the solute
increase the solvent and changes the solute
What volume of water must be added to create a 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
840 mL
84 mL
1.00 L
100. mL
What volume of 6.0 M NaOH is needed to make 300.0 mL of 0.25 M concentration?
7200 L
7200 mL
13 mL
13 L
2HCl + Ba(OH)2 → 2H2O + BaCl2
What concentration of 5.20 L of BaCl2 is formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?
0.0672 M BaCl2
0.0129 M BaCl2
11.5 M BaCl2
2.30 M BaCl2
KOH + HNO3 → KNO3 + H2O
How many moles would be in 85mL of 0.75M KOH?
110 mol KOH
1.1 mol KOH
0.11 mol KOH
0.064 mol KOH
64 mol KOH
KOH + HNO3 → KNO3 + H2O
How many grams of HNO3 would be needed to react with 85mL of 0.75M KOH?
980 g HNO3
0.0010 g HNO3
4.0 g HNO3
0.064 g HNO3
To convert liters of a solution to moles knowing the concentration of the solution, one should:
divide molarity by the volume in liters
multiply molarity by the volume in liters
multiply molarity by the molar mass of the solute
divide by the molar mass then multiply by the speed of light squared
To convert mL to L, one should:
divide by 1000
multiply by 1000
divide by 100
multiply by 100
To convert moles in an aqueous solution to liters knowing the concentration of the solution, one should:
divide moles by the molarity
multiply moles by the molarity
multiply moles by the molar mass of the solute
divide by the molar mass then multiply by the speed of light squared
