Download Honors Chemistry Chapter 16 Worksheets 1-4

Honors Chemistry
Chapter 16 Worksheet 1
Name __________________
1. What is the solubility of _______________, at ______________ in 100 cm3 of
water?
A. Sodium Nitrate
25 Co
__________ g/ 100 cm3
B. Potassium Nitrate
50 Co
__________ g/ 100 cm3
C. Sodium Nitrate
40 Co
__________ g/ 100 cm3 (extrapolate)
D. Sodium Chloride
0 Co
__________ g/ 100 cm3
2. What is the solubility of _______________, at ______________ in 50 cm3 of
water?
A. Sodium Nitrate
25 Co
__________ g/ 50 cm3
B. Potassium Nitrate
10 Co
__________ g/ 50 cm3
C. Sulfur Dioxide
25 Co
__________ g/ 50 cm3
3. What is the solubility of _______________ , at ______________ in 300 cm3 of
water?
A. Sodium Chloride
100 Co
__________ g/ 300 cm3
B. Sodium Nitrate
10 Co
__________ g/ 300 cm3
C. Ammonium Chloride 0 Co
__________ g/ 300 cm3
4. If 25 g of Potassium Nitrate is added to 100 mL of water at 30 Co, how much of
the salt will dissolve?
5. At what temperature do two of the Potassium compounds have the same
solubility? Is there more than one possible answer to this question?
___________________ Co
6. 71.0 g of Sodium Chloride is added to 100 mL of water at 100 Co. Is the solution
saturated or unsaturated? _______________
If saturated, how many grams of NaCl remain undissolved? ____________________
If unsaturated, how many more grams of NaCl could be dissolved? _____________
7. Repeat problem # 6 for 78 g of Potassium Nitrate in 200 cm3 of water at 50 Co.
8. Repeat # 6 for 15 grams of Sodium Nitrate in 50 mL of water at 30 Co.
9. Describe the following solutions using the following terms that apply:
unsaturated, saturated with no undissolved salt, saturated with undissolved salt
A. 20 g of Sodium Chloride in 50 mL of water at 50 Co.
B. 5 g of KNO3 in 35 cm3 of water at 10 Co.
C. 120 g of Copper (II) Sulfate in 300 cm3 of water at 60 Co.
10. Suppose 150 g of Potassium Chlorate was dissolved in 0.300 L of water at 100
Co. If the solution was cooled to 50 Co, how much of the salt would be
precipitated?
11. Suppose you created an unsaturated solution of Sodium Chloride by adding 1
mole of the salt to 300 grams of water at 50 CO.
A. If the solution was then heated to 100 Co, how many more grams would
you need to add of the salt to make the solution saturated?
B. Let’s say you didn’t have any more salt to add. How much water would
you have to evaporate in order to make the solution saturated?
12. If a student takes a 44.8 L sample of Sulfur Dioxide at standard temperature
and pressure and attempts to dissolve the gas in water at that temperature, how
many grams of the gas will not dissolve in 200 g of water?
Honors Chemistry
Chapter 16 Worksheet #2
Name ____________
1. Calculate the weight % of 1.75 g of NaCl in 250 g of solution.
2. Calculate the weight % of a solution made by adding 20.0 g of sucrose to 120.0 g of
water.
3. What is the Molarity of a solution made by dissolving 19.6 g of H2SO4 to a volume of
500.0 ml?
4. How many g of NaCl are needed to make 2000.0 g of a 25.0 % weight solution?
5. How many g of NaCl are needed to make 2000.0 mL of a 2.50 molar solution?
6. Calculate the Molarity of a solution made by dissolving 17.5 g of NaCl in 4.50 L of
solution.
7. What is the molality of a solution made by dissolving 2.50 g of Ca(OH)2 in 250.0 g of
water?
8. What is the molality of a solution made by dissolving 5.25g of C6H12O6 in 200.0 g of
H2O?
9. What is the Molarity of a solution made by dissolving 6.50 g of KCl in 500.0 mL of
solution?
10. How many grams of potassium nitrate are in 250.0 mL of a 0.250 M solution?
11. How many grams of sodium hydroxide are needed to make 150.0 g of 15.0%
solution?
12. What is the molality of a solution which is 12.5 % by weight C6H12O6?
13. Calculate the molality of a solution containing 4.75 g of C6H12O6 dissolving in 50.0 g
of H2O.
Honors Chemistry
Chapter 16 Worksheet # 3
Name______________
1. Calculate the Molarity of a solution made by dissolving 14.8 grams of potassium
chloride to a volume of 500.0 mL.
2. What is the Molarity of a solution made by adding 35.0 mL of 6.00 M HCl to 100.0
mL of water.
3. What is the molality of a solution made by dissolving 9.80 g of H2SO4 in 200.0 g of
H2O?
4. How many mL of 12.0 M H2SO4 are needed to make 2.00 L of a 0.250 M solution?
5. How many g of silver nitrate are needed to make 500.0 mL of a 0.0100 M solution?
6. How many mL of a solution containing 11.70 g of NaCl in 200.0 mL of solution would
be needed to prepare 500.0 mL of a 0.05 M solution?
7. Calculate the molality of a solution containing 2.75 g of C6H12O6 dissolved in 50.00 g
of HC2H3O2.
8. How many grams of potassium hydroxide are needed to prepare 200.0 mL of 0.300 M
solution?
9. Calculate the Molarity of 10.50 mL of 0.248 M H2SO4 added to 15.00 mL of water.
10. Calculate the freezing point of a solution containing 2.55 g of C6H12O6 dissolved in
25.00 g of water. ( Kf = 1.86 Co/m )
11. Calculate the boiling point of a solution containing 3.25 g of HC2H3O2 in 50.00 g of
water.
(Kb = 0.512 Co/m )
12. Calculate the boiling point of a solution containing 5.75 g of CH2O in 75.00 g of
C3H6O.
(For C3H6O, BP = 56.00 Co, Kb = 1.71 Co/m )
Honors Chemistry
Chap. 16 worksheet # 4
Name ____________
1. If 200.0 grams of Sodium nitrate are dissolved in 200.0 mL of water at 40.0 degrees C, how
much will become undissolved if the solution is cooled to 10 degrees C?
2. How many more grams of Potassium chlorate can be dissolved if 10.0 grams are currently
dissolved in 50.0 grams of water at 50.0 degrees C?
3. Calculate the molality of a 5.00 % (w/w) solution of sodium chloride
4. What is the molecular weight of a binary ionic compound compound if 14.62 grams of the
solute dissolved in 1.00 kg of solvent lowers the freezing point of an aqueous solution by 0.93
degrees C? Assuming the solute is made by combining an alkali metal and a diatomic halogen
gas, what is the formula for the chemical?
5. Refer to your notes for any necessary information not included in the following problem:
A solution is made by taking 57.5 mL of ethyl alcohol (C2H5OH) and mixing it with 2.56 moles
of water. Calculate:
molarity
molality
w/w %
w/v%
v/v %
overall density of the solution