Solutions

(12 Days)

Tentative Dates

Topic(s)

Reading

Homework

3/19

  • Solution Formation
  • Solubility
  • Factors Affecting Solubility
  • Solutions & Solutes, The Solution Process, pp. 482-483
  • Solution Formation, Solubility Factors Affecting Solubility, pp 501 - 507
  • Pre-Lab: Molar Concentration

3/20

  • Concentrations of Solutions I (Molarity)
  • Molarity, pp 509 - 511
  • Section Review: 3 - 7, p 508
  • Concept Practice 41, 44 - 46, p 528

3/21 

  • Concentrations of Solutions II (Molarity)
  • Worksheet/ Practice Calculations
  • Molarity, pp 509 - 511
  • Section Review: 21, p 515
  • Concept Practice: 49 - 52, p 528

3/22 

  • Electron/Proton Model of Atoms (An Explanation of Ions)
  • Prepared Reading on Electron/Proton Model of Atoms
  • Supplemental Problems: 1 - 7

3/31

  • Molar Concentration Lab I
  • Stoichiometry with Solutions
 
  • Supplemental Problems: 8-14

4/1

  • Molar Concentration Lab II
  • More Stoichiometry with Solutions

  • Write-Up: Molar Concentration

4/2

  • Electric Properties of Solutions
  • The Dissolution Process
  • Dissolution Reactions
  • Solvents and Solutes, The Solution Process, Electrolytes and Nonelectrolytes, pp 482 - 485 (Chapter 17)
  • Supplemental Problems 15 - 19

4/3

  • Ionic and Net Ionic Reactions that form Precipitates
  • Demonstration: NaCl + AgNO3
 
  • Pre-Lab: Reactions of Ions in Aqueous Solution

4/4

  • Reactions of Ions in Aqueous Solution Lab
 
  • Write-Up: Reactions of Ions in Aqueous Solution

4/7

  • Solubility of Ionic Compounds
  • Net Ionic Equations and Predicting the Formation of of a Precipitate pp 225 - 228 (Chapter 8)
  • Supplemental Problems 20 - 23

4/8 

  • Review
  • Chapter Review: Chapter 8 (Section 8.3) Chapter 11 (Section 11.3), Chapter 17 (Section 17.3), Chapter 18 (All Sections except 18.4)
  • Study!

4/9

  • Solutions Test
   

Labs: Dissolved Oxygen, Behavior of Solutions, Molar Concentration, Reactions of Ions in Aqueous Solution, Introduction to Qualitative Analysis, Qualitative Analysis-Relative Solutibilities

Suplemental Problems:

1) How many grams of ammonium chloride, NH4Cl, are present in 0.30 liter of a 0.40 M NH4Cl solution?

2) 25 mL of 0.10 M NaCl would react with an excess of AgNO3 to produce how many grams of AgCl (s)?

NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3 (aq)

3) Use the equation in problem 2 to determine the volume (in mL or L) of 0.50 M AgNO3 to produce 1.0 g of AgCl (s).

4) Use the equation in problem 2 to determine the concentration of NaCl if 250 mL of NaCl produced 2.5 g of AgCl (s).

5) 40.0 mL of 0.75 M HCl would require how many grams of CaCO3 to react completely?

HCl (aq) + CaCO3 (s) CaCl2 (aq) + CO2 (g) + H2O (l) (unbalanced)

6) Repeat problem 5 to determine how many liters of CO2 gas would be produced at STP. (Remember 22.4 L = 1 mole of a gas at STP.)

7) Use the equation in problem 5 to determine the concentration of HCl if 50.0 mL reacted completely with 3.00 g of CaCO3.

8) How many moles of KBr are present in 30.0 mL of a 2 M solution?

9) How many liters of 0.250 M K2CrO4 solution contain 38.8 grams of K2CrO4?

10) A 0.250 M solution of K2CrO4 reacts with PbNO3 as shown below. How many milliliters of K2CrO4 would be required to produce 5.00 g of PbCrO4 (s)?

K2CrO4 (aq) + Pb(NO3)2 (aq) PbCrO4 (s) + KNO3 (aq)

11) A neutral sodium atom has 11 electrons and protons. How many protons and electrons does Na+ have? A neutral chlorine atoms has 17 electrons and protons. How many protons and electrons does Cl- have?


12) A neutral atom of barium has 56 electrons.

a) Draw a picture of a neutral barium indicating the proper number of electrons and protons.

b) Barium becomes a Ba2+ ion. Draw a picture of a the barium ion that shows the proper number of electrons and protons.

c) Write a chemical reaction that shows the transformation of a neutral Ba atom to a Ba2+ ion. Are electrons gained or lost in this process?

 

13) A neutral fluorine atom has 9 protons. Fluorine forms an ion with a -1 ion. How many electrons does a fluoride (F-) have? Starting with F2, show the reaction to form 2 F- ions as an electron gain process.

14) Using information from problems 12) and 13) what would you expect the formula for barium fluoride to be?

15) Use the periodic table and your knowledge of the atom to list the properties of protons and electrons in the atoms and ions below:

Atom / Ion

# Protons

# Electrons

Atom / Ion

# Protons

# Electrons

H

?

?

Se 2-

?

?

Ba

?

?

Cr

?

?

O

?

?

Cr +2

?

?

N 3-

?

?

Cr +3

?

?

Fe 2+

?

?

Cr +6

?

?

 

16) Write reactions to show how metal atoms lose electrons to form cations and nonmetals gain electrons to form anions:

Metallic Elements

Reaction

Nonmetallic Elements

Reaction

Magnesium (Mg)

e.g. Mg Mg 2+ + 2 e -

Fluorine (F)

e.g. F + e - F -1

Aluminum (Al)

 

Sulfur (S)

 

Potassium (K)

 

Arsenic (As)

 

Calcium (Ca)

 

Bromine (Br)

 

 

17) Which of the following substances would you expect would dissolve in water to conduct electricity (i.e. which are ionic)?

a) CaCl2 b) N2

c) CO2

d) Mg(NO3)2 e) AlI3 f) C6H12O6

18) The KBr conducts electricity when it dissolves in water because it forms potassium and bromide ions. Write the dissolution reaction. Repeat the problem for Sr(C2H3O2)2.

19) The salt ammonium sulfate (NH4)2SO4 dissolves in water to form a conducting solution containing ammonium ions, NH4+, and sulfate ions, SO42-.

a) Write a balanced equation for the reaction when this ionic solid dissolves in water.

b) Verify the conservation of charge by comparing the charge of the reactant to the sum of the charges of the products.

c) Suppose 1.32 g of ammounium sulfate are dissolved to make 0.500 L of solution. Calculate the concentrations of NH4+ and SO42-.

 

20) Assume the following solid compounds dissolve in water to form separate, mobile ions in solution. Write the formulas and the names of ions that will form when the solid dissolves.

e.g. NaCl forms Na+ (sodium ion) and Cl- (chloride ion).

  a) HI b) CaCl2 c) Na2CO3 d) Ba(OH)2 e) KNO3 f) NH4Cl

 

21) Write the equation for the reaction that occurs when each of these electrolytes is dissolved in water:

a) lithium hydroxide (solid)

b) nitric acid (liquid)

c) potassium sulfate (liquid)

d) sodium nitrate (solid)

e) ammonium iodide

f) potassium carbonate (solid)

 

22) Use your solubility table (See Handout) to predict whether the following are soluble in water:

a) KCl

b) CaCO3 c) Na2SO4 d) PbS e) Ba(OH)2

f) Mg(NO3)2

g) NH4SO3 h) AgCH3COO i) AgI j) Li3PO4

23) Use your solubility table to predict if any reactions occur. If they occur, write the ionic and net ionic equation.

a) Na2SO4 + NH4Cl

b) MgSO4 + K2CO3

c) Pb(CH3COO)2 + AlCl3

d) Ca(NO3)2 + Li2S

e) BaI2 + NaOH

f) Sr(OH)2 + Zn(NO3)2

24) Write ionic and net ionic reactions for the following reactions. In some instances a precipitate will form, in others no reaction will occur.

a) NaCl (aq) + AgCH3COO (aq)

b) KNO3 (aq) + MgSO4 (aq)

c) Rb2SO4 + BaCl2 (aq)

d) AgNO3 (aq) + KOH (aq)

 

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