Chapter 14: Solutions Campbell Chemistry Name: ______________________

1

Date In Class Homework

2/1 W Chapter 12 Test Watch Solution Video 1: Types of

Solutions

2/2 Th Discuss video 1 and Concentration Activity Prelab acid base lab

2/3 F Acid Base Titration Lab Watch Solution Video 2: What

and How Much Dissolves

2/6 M LSM/Club pics

Video 2 Discussion and How to Increase the Rate in class notes

2/7 Tu Molarity and Dilution Calculations (in class

notes) Prelab for mixing solutions

2/8 W Mixing Solutions Lab

2/9 Th Solution Stoichiometry (in class notes)

2/10 F Winter pep assem

BRING HEADPHONES- Watch Solution Video 3: Colligative Properties

2/13 M Finish Unit Packet/Get study guide

2/14 Tu Review for test Study for Test

2/15 W Chapter 14 Solution Test

Chapter 14: Solutions Campbell Chemistry Name: ______________________

2

Video 1. Solution Types: https://youtu.be/zOo5dU8MbV0

Textbook:14.1 & 14.3 pg 476-479 & 489-490

Guided Notes for Video on Solution Types Questions:

Define suspension? What type of mixture is a suspension? What happens when a suspension sits still for a while?

Define solution? What type of mixture is a solution?

Define Solute: Define Solvent: Which is in the lesser amount: Which is in the greater amount:

List some of the types of solutions and give examples of each. (turn page!)

Chapter 14: Solutions Campbell Chemistry Name: ______________________

3

List the steps in the process of solvation (dissolving): 1. 2.

Define Unsaturated solution Saturated Solution Supersaturated Solution

How do you make a solution Supersaturated?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

4

Molarity and Dilution In Class notes:

Textbook: 14.2 pg 482-486

1. Define Dilute Solution:

2. Define Concentrated Solution:

3. What is the Symbol, equation and units for Molarity:

4. Show the work for the three types of Molarity calculations:

a. Find the Molarity of saline solution if there is 2.23 g of NaCl in 225 mL of solution.

b. Find the moles of solute in 0.678 L of a 0.333M H2SO4 solution.

c. Find the grams of solute in a 5.51 liters of a 2.20M NaHCO3 solution.

5. Define dilution:

6. What is the dilution equation?

7. Show work for the following example problems:

a. How many mL of 18.1 M KMnO4 is needed to produce 125mL of 0.100M KMnO4 solution?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

5

b. What is the molarity of a solution if 350 mL of a 0.5 M NaOH solution is diluted to 1.0 L?

8. Your Turn:

a. Calculate the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr.

b. Calculate how many moles of NaOCl are in 2.75 L of a 0.128 M solution of bleach.

c. Find the amount of NaOH in grams present in 0.250 mL of a 0.280 M solution.

d. You took 15 mL of a concentrated HCl solution and diluted it to a volume of 100 mL with a

concentration of 0.2M. What was the concentration of the original HCl?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

6

Video 2. What and How Much Dissolves: https://youtu.be/jsGBmcZOc-s Textbook: 14.3 pg 492-495

Guided Notes for Video on What and How Much Dissolves: Questions:

What does Like Dissolves Like Mean?

Fill out the following table: INCLUDE THE EXAMPLES OF POLAR AND NONPOLAR SOLUTES AND SOLVENTS:

Solute

Polar Solvent EXAMPLE:

Non-Polar Solvent EXAMPLE:

Ionic EXAMPLE:

Polar EXAMPLE:

Nonpolar EXAMPLE:

What is an aqueous solution?

Why is water a good solvent? (turn page!)

Chapter 14: Solutions Campbell Chemistry Name: ______________________

7

How do you determine if a molecule is nonpolar or polar?

List and describe the three factors that affect the AMOUNT of solute that dissolves in a solvent: 1. 2. Solids: Gases: 3.

Rate of Dissolving In Class Notes:

What are the three things you can do to increase the RATE at which a solute dissolves in a solvent?

1.

2.

3.

Chapter 14: Solutions Campbell Chemistry Name: ______________________

8

H2SO

4(aq) + 2NaHCO

3 2H

2O(l) + Na

2SO

4(aq) + 2CO

2(g)

Solution Stoichiometry In Class Notes:

1. What are the steps in solving a solution stoichiometry problem?

2. Show your work solving: How many grams of AgCl are produced if 10.0 mL of a 0.75 M

Ag2SO4 solution react with NaCl? Ag2SO4 + NaCl AgCl(s)+ Na2SO4

3. How many mL of 0.25 M Na2SO4 solution is needed to produce 1.65 g NaNO3?

Na2SO4 + Ba(NO3)2 BaSO4 + NaNO3

4. You Try: 50.0 mL of 6.0 M H2SO4 (battery acid) were spilled and solid NaHCO3 is to be used

to neutralize the acid. How many grams of NaHCO3 must be used?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

9

Video 3. Colligative Properties: https://youtu.be/CuL8NNgOzWo

Textbook: 14.4 pg 498-503

Guided Notes for Video on Colligative Properties Questions:

What is a colligative property?

What type of nonvolatile solutes are most effective?

Define freezing point depression

Define vapor pressure reduction

Define boiling point elevation

Which is more effective at reducing the freezing point of water: ________ Sugar (C6H12O6) ________ Salt (NaCl) Why?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

10

In Class Work:

Video 1. 1. You are making Lemonade from a powder. You mix the powder in water.

a. What is the Solute: What is the Solvent:

b. How do you know when the water has become saturated with the lemonade powder:

c. If you wanted to make the lemonade supersaturated how could you do that?

2. Give one example of each of the following types of solutions:

a) gas-gas

b) gas-liquid

c) liquid-liquid

d) solid-liquid

e) solid-solid

In Class Molarity and Dilution Calculations:

3. Calculate the molarity for the following:

a. 0.250 moles of NaCl in 0.750 L of solution

b. 1.3 moles of K2SO4 in 435 ml of solution

c. 0.0035 moles of Cu(NO3)2 in 0.68 ml of solution

4. For each of the following solutions the mass of the solute is given, followed by the total volume of

the solution prepared. Calculate the molarity.

a. 4.25 g CuCl2; 125 mL

b. 0.101 g NaHCO3; 11.3 mL

c. 52.9 g Na2CO3; 1.15 L

Chapter 14: Solutions Campbell Chemistry Name: ______________________

11

5. Calculate the number of moles and number of grams of the indicated solutes contained in each of

the following solution samples.

a. 1.29 L of 0.411 M HCl

b. 145 mL of 0.215 M CaCl2

c. 24.9 mL of 1.15 M HNO3

6. Calculate the new molarity that results when 250. mL of water is added to each of the following

solutions (for your second volume: take the initial volume given and add 250 to it!!).

a. 125 mL of 0.251 M HCl

b. 445 mL of 0.499 M H2SO4

c. 1.65 L of 0.101 M HNO3

7. Concentrated sulfuric acid is typically 18.1 M H2SO4. Calculate the volume in mL of concentrated

sulfuric acid needed to prepare 125 mL of 0.100 M H2SO4 solution.

8. Calculate the molarity after 150ml of 2.5 M HCl is diluted to 400ml.

9. What volume of 16M sulfuric acid must be used to prepare 1.5 L of a 0.10M sulfuric acid

solution?

Chapter 14: Solutions Campbell Chemistry Name: ______________________

12

Video 2 In class Work: 10. Which of the following compounds would you expect to dissolve in water? Explain why.

hexane (C6H14) or hexanol (C6H13OH)

11. Tell whether the following compounds are soluble or insoluble in water, and explain why.

a. KNO3

b. C3H8

c. CH3OH

d. Cu

12. Tell whether the following compounds are soluble or insoluble in gasoline (C8H18), and explain why.

a. MgCl2

b. C6H14

c. N2|

d. Fe

13. You have a cube of rock salt that measures 1 m x 1 m x 1m (one cubic meter).

a) If you placed it in a tub of water, explain whether you think it would dissolve quickly or not.

b) Tell what you would do to get the block of salt to dissolve more quickly.

Solution Stoichiometry BALANCE EACH EQUATION! 14. If an aqueous AgNO3 sample reacts with 27.2 mL of 0.104 M CaCl2 , how many grams of AgCl

will be made?

AgNO3(aq) + CaCl2 (aq) AgCl(s) + Ca(NO3)2 (aq)

Chapter 14: Solutions Campbell Chemistry Name: ______________________

13

15. How many grams of NaCl is needed to precipitate all the BaCl2 (s) from 12.5 mL of 0.15 M

Ba(NO3)2 solution?

Ba(NO3)2(aq) + NaCl(s) BaCl2(s) + NaNO3(aq)

16. What mass (in grams) of AgNO3 is required to precipitate allof the chloride ion, as AgCl, from 135

mL of 0.101 M AlCl3 solution?

AgNO3(aq) + AlCl3(aq) AgCl(s) + Al(NO3)3(aq)

17. How many mL of 0.20 M NiCl2 solution are needed to produce 50g of NiS?

NiCl2(aq) + Na2S(aq) NiS(s) + NaCl(aq)

18. How many ml of 0.35 M aluminum chloride are needed to react with 52g of calcium?

AlCl3(aq) + Ca(s) CaCl2(aq) + Al(s)

19. How many ml of 0.75 M iron (III) nitrate are required to react with 4.25 grams of potassium

bromide?

Fe(NO3)3(aq) + KBr(aq) FeBr3(aq) + KNO3(aq)

Chapter 14: Solutions Campbell Chemistry Name: ______________________

14

Nomenclature practice:

20. Give the name or formula for the following:

a) acetic acid f) H3P

b) ammonium sulfide g) Al(NO3)3

c) lead (II) chlorite h) SnO

d) magnesium iodide i) Ca(OH)2

e) dinitrogen heptabromide j) Cl3F8

Answers to Problems in problem set

3. a. 0.333 M b. 3.0 M c. 5.1 M

4. a. 0.253 M b. 0.106 M c. 0.434 M

5. a. 0.530 moles 19.3 g

b. 0.0312 moles 3.46 g

c. 0.0286 moles 1.80 g

6. a. 0.0837 M b. 0.320 M c. 0.0877 M

7. 0 .691 ml

8. 0.938 M

9. 0.0094 L

10. Hexanol it is polar because it has the OH group

11. a. soluble – ionic b. insoluble – non-polar c. soluble – polar d. insoluble - metal

12. a. insoluble – ionic b. soluble – nonpolar c. soluble – nonpolar d. insoluble - metal

14. 0.811g

15. 0.22 g

16. 6.93 g

17. 2.75 L or 2750 mL

18. 2.471 L or 2471 mL

19. 0.159 L or 15.9 mL

20. Answer to nomenclature

a) HC2H3O2 f) hydrophosphoric acid

b) (NH4)2S g) aluminum nitrate

c) Pb(ClO2)2 h) tin (II) oxide

d) MgI2 i) calcium hydroxide

e) N2Br7 j) trichlorine octafluoride