Solutions and Molarity Part II

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Solutions and MolarityPart II
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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?

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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?
• Molarity

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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?
• Molarity 13.8 L CO2 x

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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?
• Molarity 13.8 L CO2 x 1 mol CO2
  22.4 L

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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?
• Molarity 13.8 L CO2 x 1 mol CO2
  22.4 L
• 0.250 L

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• 1. 13.8 L of CO2 _at_ STP is dissolved in 250.0 mL
  of
• water. What is the molarity of the resulting
• solution?
• Molarity 13.8 L CO2 x 1 mol CO2
  22.4 L
• 0.250 L
• 2.46 M

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• 2. If a 1.89 M solution is made by dissolving
  chlorine gas in 600.0 mL of water, what volume
  of Cl2 gas was dissolved?

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• 2. If a 1.89 M solution is made by dissolving
  chlorine gas in 600.0 mL of water, what volume
  of Cl2 gas was dissolved?
• 0.600 L x

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• 2. If a 1.89 M solution is made by dissolving
  chlorine gas in 600.0 mL of water, what volume
  of Cl2 gas was dissolved?
• 0.600 L x 1.89 mol
• 1 L

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• 2. If a 1.89 M solution is made by dissolving
  chlorine gas in 600.0 mL of water, what volume
  of Cl2 gas was dissolved?
• 0.600 L x 1.89 mol x 22.4 L
• 1 L 1 mol

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• 2. If a 1.89 M solution is made by dissolving
  chlorine gas in 600.0 mL of water, what volume
  of Cl2 gas was dissolved?
• 0.600 L x 1.89 mol x 22.4 L
• 1 L 1 mol
• 25.4 L of Cl2 gas

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?
• Molarity

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?
• Molarity 2.96 x 1024 FU

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?
• Molarity 2.96 x 1024 FU x 1 mol
• 6.02 x 1023 FU

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?
• Molarity 2.96 x 1024 FU x 1 mol
• 6.02 x 1023 FU 0.500 L

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• 3. Calculate the molarity of a solution when
• 2.96 x 1024 FUs of CaF2 are dissolved in
• 0.500 L of water?
• Molarity 2.96 x 1024 FU x 1 mol
• 6.02 x 1023 FU 0.500 L
• 9.83 M

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• 4. How many molecules are dissolved in 1.00 L
• of water if the molarity of the H2SO4 solution
• is 0.2 M?

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• 4. How many molecules are dissolved in 1.00 L
• of water if the molarity of the H2SO4 solution
• is 0.2 M?
• 1.00 L

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• 4. How many molecules are dissolved in 1.00 L
• of water if the molarity of the H2SO4 solution
• is 0.2 M?
• 1.00 L x 0.2 mol
• 1L

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• 4. How many molecules are dissolved in 1.00 L
• of water if the molarity of the H2SO4 solution
• is 0.2 M?
• 1.00 L x 0.2 mol x 6.02 x 1023 molecules
• 1L 1 mol

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• 4. How many molecules are dissolved in 1.00 L
• of water if the molarity of the H2SO4 solution
• is 0.2 M?
• 1.00 L x 0.2 mol x 6.02 x 1023 molecules
• 1L 1 mol
• 1 x1023 molecules

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate.

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate.

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate..

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g
• 0.0800 L ZnCl2

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate..

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g
• 0.0800 L ZnCl2 x 0.336 mole ZnCl2
• 1 L ZnCl2

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate.

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g
• 0.0800 L ZnCl2 x 0.336 mole ZnCl2 x 1
  mole Zn(OH)2
• 1 L ZnCl2 1 mole ZnCl2
  

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate.

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g
• 0.0800 L ZnCl2 x 0.336 mole ZnCl2 x 1
  mole Zn(OH)2 x 99.4 g Zn(OH)2
• 1 L ZnCl2 1 mole ZnCl2
  1 mol Zn(OH)2

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5. Excess sodium hydroxide solution is added to
80.0 mL of 0.336 M ZnCl2, calculate the mass of
zinc hydroxide that will precipitate.

• 2 NaOH (aq) ZnCl2(aq) ? Zn(OH)2(s) 2NaCl
  (aq)
• 0.0800 L ? g
• 0.0800 L ZnCl2 x 0.336 mole ZnCl2 x 1
  mole Zn(OH)2 x 99.4 g Zn(OH)2
• 1 L ZnCl2 1 mole ZnCl2
  1 mol Zn(OH)2
• 2.67 g Zn(OH)2

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Class work and Homework Workbook Molarity 2 and
Molarity 3