1. Lesson 2
Ion
Concentration

2. 1. What is the concentration of each ion in 2. 0 L of a 0. 300 M AlCl3
1. What is the concentration of each ion in 2.0 L of a M AlCl3 solution?
AlCl3  Al3+ + 3Cl-
0.300 M
0.300 M
0.900 M

3. 2. What is the concentration of each ion in the solution formed by dissolving g of CaCl2 in mL of water?
1 mole
80.0 g x
111.1 g
Molarity =
= M
0.600 L
CaCl2  Ca2+ + 2Cl-
1.20 M
1.20 M
2.40 M

4. 3. If 40. 0 mL of 0. 400 M AlCl3 solution is added to 60. 0 mL of 0
3. If 40.0 mL of M AlCl3 solution is added to 60.0 mL of M CaCl2 solution, what is the resulting concentration of all ions?
AlCl  Al3+ + 3Cl- x
0.400 M
0.160 M
0.480 M
100.0
CaCl  Ca2+ + 2Cl-
60.0 x M
0.360 M
0.720 M
100.0
[Cl-] = M = M

5. 4. If the [Cl-] = 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 g
= g
1 L
1 mole

6. 5. Write the formula, complete, and net ionic equation for the
5. Write the formula, complete, and net ionic equation for the reaction:
Ca(s) + H2SO4(aq) →
H2(g) + CaSO4(s)
only break up aqueous!
low solubility
Ca(s)
H SO42- →
H2(g) + CaSO4(s)
Ca(s) H SO42- → H2(g) + CaSO4(s)