Lesson 2Ion

Concentration

1. What is the concentration of each ion in a 0.300 M AlCl3

solution?

AlCl3 Al3+ + 3Cl-

1. What is the concentration of each ion in a 0.300 M AlCl3

solution?

AlCl3 Al3+ + 3Cl-

0.300 M

1. What is the concentration of each ion in a 0.300 M AlCl3

solution?

AlCl3 Al3+ + 3Cl-

0.300 M 0.300 M

1. What is the concentration of each ion in a 0.300 M AlCl3

solution?

AlCl3 Al3+ + 3Cl-

0.300 M 0.300 M 0.900 M

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity =

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

0.600 L

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

0.600 L

= 1.20 M

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

0.600 L

= 1.20 M

CaCl2 Ca2+ + 2Cl-

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

0.600 L

= 1.20 M

CaCl2 Ca2+ + 2Cl-

1.20 M

2. What is the concentration of each ion in the solution formed by dissolving 80.0 g of CaCl2 in 600.0 mL of water?

Molarity = 80.0 g x 1 mole 111.1 g

0.600 L

= 1.20 M

CaCl2 Ca2+ + 2Cl-

1.20 M 2.40 M

3. If 40.0 mL of 0.400 M Potassium chloride solution is added to 60.0 mL of 0.600 M Calcium nitrate solution, what is the resulting concentration of all ions?

KCl K+ + Cl-

40.0 x 0.400 M = 0.160 M 0.160 M100.0

Dilution Factor

Ca(NO3)2 Ca2+ + 2NO3-

60.0 x 0.600 M = 0.360 M 0.720 M

100.0

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.600 M

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.600 M

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.200 M 0.600 M

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.200 M 0.600 M

3.00 L

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.200 M 0.600 M

3.00 L x 0.200 mole 1 L

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.200 M 0.600 M

3.00 L x 0.200 mole x 133.5 g = 1 L 1 mole

4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3

that would be dissolved in 3.00 L of water.

AlCl3 Al3+ + 3Cl-

0.200 M 0.200 M 0.600 M

3.00 L x 0.200 mole x 133.5 g = 80.1 g 1 L 1 mole

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

Ga2(SO4)3 2Ga3+ + 3SO42-

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

Ga2(SO4)3 2Ga3+ + 3SO42-

0.900 M

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

Ga2(SO4)3 2Ga3+ + 3SO42-

0.600 M 0.900 M

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

Ga2(SO4)3 2Ga3+ + 3SO42-

0.300 M 0.600 M 0.900 M

5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine

the [Ga3+] and the molarity of the solution.

Ga2(SO4)3 2Ga3+ + 3SO42-

0.300 M 0.600 M 0.900 M

Do not use the 20.0 mL!

6. Write the formula, complete, and net ionic equation for the reaction:

 Ca(s) + H2SO4(aq)→

6. Write the formula, complete, and net ionic equation for the reaction:

 Ca(s) + H2SO4(aq) → H2(g) + CaSO4(s)

low solubility

6. Write the formula, complete, and net ionic equation for the reaction:

 Ca(s) + H2SO4(aq) → H2(g) + CaSO4(s)

low solubility

Ca(s) + 2H+ + SO42- → H2(g) + CaSO4(s)

only break up aqueous!

6. Write the formula, complete, and net ionic equation for the reaction:

 Ca(s) + H2SO4(aq) → H2(g) + CaSO4(s)

low solubility

Ca(s) + 2H+ + SO42- → H2(g) + CaSO4(s)

only break up aqueous!

Ca(s) + 2H+ + SO42- → H2(g) + CaSO4(s)

nothing cancels!