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Solutions and Molarity

Solutions and Molarity. 1. 13.8 L of CO 2 @ STP is dissolved in 250.0 mL of water. What is the molarity of the resulting solution?. 13.8 L CO 2. x 1 mol CO 2. 22.4 L. Molarity. =. 0.250 L. = 2.46 M.

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Solutions and Molarity

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  1. Solutions and Molarity

  2. 1. 13.8 L of CO2 @ STP is dissolved in 250.0 mL of water. What is the molarity of the resulting solution? 13.8 L CO2 x 1 mol CO2 22.4 L Molarity = 0.250 L = 2.46 M

  3. 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? x 22.4 L = 25.4 L of Cl2 gas 0.600 L x 1.89 mol 1 mol 1 L

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

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

  6. 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 x 1 mole Zn(OH)2 0.0800 L ZnCl2 x 0.336 mole x 99.4 g 1 L 1 mole ZnCl2 1 mol = 2.67 g Zn(OH)2

  7. 6. Calculate the volume of 0.100 M HCl solution that is required to completely neutralize 250.0 mL of 0.200 M Ba(OH)2 solution. 2HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2H2O (l) ? L 0.2500 L x 2 mole HCl 0.2500L Ba(OH)2 x 0.200 mole x 1 L 1 L 1 mole Ba(OH)2 0.100 mol = 1.00 L

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