Solutions Worksheet
Name____________________
1) How many grams of beryllium chloride are needed to make 125 mL of a 0.050 M
solution?
2) What is the concentration of ions in a 1.2M solution of calcium hydroxide?
3) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make
a 1.0 M solution?
4) How many moles of solute do you need to make one liter of a 1.25 mol/L
ammonium hydroxide solution.
5) What is the molarity of a solution in which 0.45 grams of sodium nitrate are
dissolved in 265 mL of solution?
6) What is the concentration of ions in the solution of 0.22g of sodium chloride are
dissolved in 300.0 mL?
7) If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150
mL, what will the molarity of the diluted solution be?
8) What will the volume of a 0.50 M solution be if it contains 25 grams of calcium
hydroxide?
9) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
10) How many grams of ammonia are present in 5.0 L of a 0.050 M solution?
11) If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the
molarity of the diluted solution be?
Concentration Worksheet – Answers
1)
How many grams of beryllium chloride are needed to make 125 mL of a 0.050 M
solution?
0.50 grams
2)
Explain how to make at least one liter of a 1.25 M ammonium hydroxide
solution.
Dissolve 43.8 grams (1.25 moles) of ammonium hydroxide in 1 L H 2O.
3)
What is the molarity of a solution in which 0.45 grams of sodium nitrate are
dissolved in 265 mL of solution.
0.020 M
4)
What will the volume of a 0.50 M solution be if it contains 25 grams of calcium
hydroxide?
680 mL
5)
How many grams of ammonia are present in 5.0 L of a 0.050 M solution?
4.3 grams
Dilutions Worksheet - Solutions
6)
If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the
molarity of the diluted solution be?
M1V1 = M2V2
(0.15 M)(125 mL) = x (150 mL)
x = 0.125 M
7)
If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150
mL, what will the molarity of the diluted solution be?
M1V1 = M2V2
(0.15 M)(100 mL) = x (150 mL)
x = 0.100 M
8)
How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
M1V1 = M2V2
(10 M)(250 mL) = (0.05 M) x
x = 50,000 mL
9)
How much water would I need to add to 500 mL of a 2.4 M KCl solution to make
a 1.0 M solution?
M1V1 = M2V2
(2.4 M)(500 mL) = (1.0 M) x
x = 1200 mL
1200 mL will be the final volume of the solution. However, since there’s
already 500 mL of solution present, you only need to add 700 mL of water to
get 1200 mL as your final volume. The answer: 700 mL.