Lesson 2 Ion Concentration
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Transcript of Lesson 2 Ion Concentration
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Lesson 2Ion
Concentration
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1. What is the concentration of each ion in a 0.300 M AlCl3
solution?
AlCl3 Al3+ + 3Cl-
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1. What is the concentration of each ion in a 0.300 M AlCl3
solution?
AlCl3 Al3+ + 3Cl-
0.300 M
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1. What is the concentration of each ion in a 0.300 M AlCl3
solution?
AlCl3 Al3+ + 3Cl-
0.300 M 0.300 M
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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
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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 =
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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
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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
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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
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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-
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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
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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
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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
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4. If the [Cl-] = 0.600 M, calculate the number of grams AlCl3
that would be dissolved in 3.00 L of water.
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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
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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
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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
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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
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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
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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
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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
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5. If the [SO42-] = 0.900 M in 20.0 mL of Ga2(SO4)3, determine
the [Ga3+] and the molarity of the solution.
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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-
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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
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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
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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
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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!
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6. Write the formula, complete, and net ionic equation for the reaction:
Ca(s) + H2SO4(aq)→
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6. Write the formula, complete, and net ionic equation for the reaction:
Ca(s) + H2SO4(aq) → H2(g) + CaSO4(s)
low solubility
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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!
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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!