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WorksheetsREVIEW: Solutions
Total questions: 81
Worksheet time: 27mins
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
60 ºC
30 ºC
50 ºC
83 ºC
25 grams of NaCl are dissolved in 100 mL of water at 60 oC. How many more grams need to be dissolved for the solution to be saturated?
13 grams
25 grams
6 grams
38 grams
How many grams of K2Cr2O7, are soluble in 100 g of water at 90 ºC?
85 grams
70 grams
40 grams
15 grams
How many grams of K2Cr2O7, are soluble in 50 g of water at 90ºC?
70 grams
35 grams
140 grams
105 grams
How many grams of KClO3, are soluble in 200g of water at 30ºC?
5 grams
100 grams
10 grams
20 grams
How much KNO3 solute is present in a saturated solution at 40 oC in 100 g of H2O?
75
55
63
85
How much Ce2(SO4)3 solute is saturated at 40 oC in 100 g of H2O?
240 g
220 g
230 g
250 g
3 g
How much Ce2(SO4)3 solute is saturated at 80 oC in 100 g of H2O?
20
15
30
10
3
How much CaCl2 solute is saturated at 20 oC in 100 g of H2O?
65 g
75 g
10 g
5 g
100 g
At what temperature can you fully dissolve 88 g of NaNO3 in 100 g of H2O?
62 oC
73 oC
81 oC
34 oC
20 oC
At what temperature can you fully dissolve 60 g of KNO3 into 100 g of H2O?
27 oC
30 oC
39 oC
80 oC
55 oC
At what temperature can you fully dissolve 30 g of K2Cr2O7 into 100 g of H2O?
70 oC
20 oC
100 oC
50 oC
25 oC
What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
What type of a solution is 100g KNO3 at 40ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
What type of a solution is 65g of lead (II) nitrate at 30ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
What type of a solution is 25g NaCl at 70ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
What type of a solution is 55g KCl at 70ºC in 100g H2O?
Saturated
Unsaturated
Supersaturated
How many grams of NaCl, are soluble in 300g of water at 90ºC?
(a)
What compound shows a decrease in solubility from 0o to 100oC?
NaCl
KCl
CaCl2
Ce2(SO4)3
KNO3
How many grams of potassium chloride can be dissolved in 200g of water at 80oC?
104 g
125 g
40 g
160 g
300 g
At 40oC, how much potassium nitrate can be dissolved in 300 g of water?
104 g
126 g
63 g
160 g
195 g
If a solution of K₂Cr₂O₇ is saturated at 50°C and is then lowered to 20°C, how much solid comes out of solution?
19 g
30 g
50 g
11 g
41 g
Which solution is the most concentrated:
Solution A
Solution B
Solution C
They all have the same concentration
Which solution is the most concentrated:
Solution A
Solution B
Solution C
They all have the same concentration
Which solution is the least concentrated:
Solution A
Solution B
Solution C
They all have the same concentration
Match the description with the correct solution:
A homogeneous mixture. A solute dissolved into a solvent: (a)
The substance that dissolves another substance: (a)
The universal solvent: (a)
The substance that gets dissolved into another substance: (a)
A solution containing a large amount of solute: (a)
A solution containing a small amount of solute: (a)
A solution that can dissolve more solute at a given temperature: (a)
Identify the solute and solvent for the solution:
Identify the solute and solvent for the solution:
Identify the solute and solvent for the solution:
Identify the solute and solvent for the solution:
Identify the solute and solvent for the solution:
The solution cannot hold any more solute: (a)
When a solution is saturated at an elevated temperature and then allowed to cool but all of the solid remains dissolved: (a)
Identify the most concentrated solution:
Identify the least concentrated solution:
Identify the most diluted solution:
Identify the solution(s) that are definitely unsaturated:
What is the molarity of 3.00 mole of hydrochloric acid in 3.00 L of water.
3.00 M
1.00 M
6.00 M
9.00 M
0.333 M
What is the molarity of 4.00 grams of sodium chloride in 3,800 mL of solution? (NaCl molar mass = 58.44 g/mol)
0.0180 M
15,200 M
1.05 M
15.2 M
0.260 M
How many liters (L) are required to make 3.50 M hydrochloric acid using 1.10 moles?
3.18 L
0.314 L
3.85 L
4.6 L
3.50 L
If you have 0.0450 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
20.9 mol
10.3 mol
0.0968 mol
0.0209 mol
0.465 mol
What is the molarity of a solution containing 4.00 moles of KCl in 2.50 L of solution?
1.60 M
0.630 M
10.0 M
2.60 M
4.00 M
What volume is needed to make a 2.45 M solution of KCl using 0.500 mol of KCl?
4.90 L
0.204 L
1.22 L
0.500 L
2.45 L
How many grams of KCl would be dissolved in 5.50 L of a 0.250 M solution of KCl? *molar mass of KCl = 74.55 g/mol*
1.48 g
103 g
1640 g
3.39 g
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 0.5 L?
300. M
31.3 M
3.13 M
1.56 M
What is the molarity of 2.50 mol of NaOH in 12.0 L of solution?
0.210 M
30.0 M
4.80 M
20.8 M
12.0 M
If 2.50 L of a 4.00 M solution of FeCl3 is diluted to a volume of 6.00 L by the addition of water, what is the molarity of the diluted solution?
2.50 M
4.17 M
6.25 M
1.67 M
6.00 M
If a chemist starts with 25.0 mL of 6.00 M HCl and prepares a new solution with a concentration of 0.500 M, what with be the new volume?
200. mL
500. mL
300. mL
400. mL
100. mL
A chemist dilutes 25.0 mL of a 2.00 M solution to make 500. mL of new solution. What is the molar concentration of the new solution?
0.100 M
0.200 M
6,250 M
1.00 M
40.0 M
How many moles of calcium chloride are needed to make up 2.00 L of a 0.476 M solution?
(a)
How many moles of KHCO₃ are needed to make up 2,510 ml of 0.750 M solution?
(a)
How many grams of solid NaOH are needed to make up 2.00 liters of a 0.500M aqueous solution of sodium hydroxide?
(a)
How many moles of solid CuCl₂ are needed to make up 15.00 liters of a 0.300 M aqueous solution of copper (II) chloride?
(a)
I used 117.0 g of NaCl to make up a 0.500 M solution. What volume is that?
(a)
I used 100.0 g of NaOH to make up 0.750 L of solution. What is the molarity of the solution?
(a)
I use 215 g of Fe(NO₃)₂ to make up 1000.0 ml of solution. What is the molarity of the solution?
(a)
How many grams of CuSO₄ should you weigh out if you want to make up 2.00 L of 0.200 M solution?
(a)
You need to make up solution that has a concentration of chloride ions that is 2.00 M. You use barium chloride to make up the solution. How much barium chloride (in moles) do you need to make a 5.30 L solution?
(a)
Determine the volume (in liters) of a 4.50 molar solution of NaOH made by diluting 2.00 L of a 12.0 molar solution.
(a)
How much water would need to be added to dilute 2.50 L of a 10.0 molar solution of Fe(NO₃)₂ to make a 1.25 molar solution.
(a)
1.20 L of a 7.50 molar solution of CoCl₂ is diluted to 1.75 L, what is the molarity of the new solution?
(a)
Determine the volume (in liters) of a 2.00 molar solution of Ca(NO₃)₂ made by diluting 855 mL of a 12.0 molar solution.
(a)
925 mL of a 1.50 molar solution is diluted to 2.75 L, what is the molarity of the new solution?
(a)
Determine the volume (in liters) of a 0.450 molar solution of Co(NO₃)₂ made by diluting 950 mL of a 0.750 molar solution.
(a)
To make 242 mL of a 0.650 M dilution from a 11.3 M concentrated stock solution, determine the volume of the stock solution:
(a)
A 116 g sample of NaCl (Molar Mass = 58.44 g/mol) is dissolved in enough water to make 1.43 L of solution. What volume of this original solution must be used to dilute it to make 7.00 L of 0.484 M NaCl?
(a)
A 116 g sample of NiCl₂ (Molar Mass = 129.59 g/mol) is dissolved in enough water to make 1.43 L of solution. What volume of this original solution must be used to dilute it to make 7.00 L of 0.484 M NaCl?
(a)
