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What is the solute when 10 g of NaCl is dissolved in 100 mL of water?

What is the solute when 10 g of NaCl is dissolved in 100 mL of water?. 13.1. NaCl Na Cl 2 H 2 O None of the above. What is the solute when 10 g of NaCl is dissolved in 100 mL of water?. 13.1. NaCl Na Cl 2 H 2 O None of the above.

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What is the solute when 10 g of NaCl is dissolved in 100 mL of water?

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  1. What is the solute when 10 g of NaCl is dissolved in 100 mL of water? 13.1 NaCl Na Cl2 H2O None of the above

  2. What is the solute when 10 g of NaCl is dissolved in 100 mL of water? 13.1 NaCl Na Cl2 H2O None of the above

  3. Which solvent would be most suitable to remove grease from an object? 13.2 H2O NH3 CH3OH CH3OCH3 C8H18

  4. Which solvent would be most suitable to remove grease from an object? 13.2 H2O NH3 CH3OH CH3OCH3 C8H18

  5. Which of the following substances is an example of a solution? 13.3 Salad dressing Blueberry muffin Wine Sugar Lead

  6. Which of the following substances is an example of a solution? 13.3 Salad dressing Blueberry muffin Wine Sugar Lead

  7. In theory which of the following would have the highest solubility in gasoline (C8H18) ? 13.4 CH3CH2CH3 CH3OCH3 CH3CH2OH CH3CH2NH2 CH3CH2COOH

  8. In theory which of the following would have the highest solubility in gasoline (C8H18) ? 13.4 CH3CH2CH3 CH3OCH3 CH3CH2OH CH3CH2NH2 CH3CH2COOH

  9. A supersaturated solution: 13.5 Holds less than the maximum amount of solute at that temperature Holds the maximum amount of solute at that temperature Holds more than the normal maximum amount of solute at that temperature All of above None of the above

  10. A supersaturated solution: 13.5 Holds less than the maximum amount of solute at that temperature Holds the maximum amount of solute at that temperature Holds more than the normal maximum amount of solute at that temperature All of above None of the above

  11. Which of the following NaCl solutions has the highest concentration of NaCl? 13.6 0.0175 mol NaCl in 1 L of solution 0.1 g NaCl in 100 mL of solution 0.5 g NaCl in 500 mL of solution 0.25 mol NaCl in 200 mL of solution All have the same concentration.

  12. Which of the following NaCl solutions has the highest concentration of NaCl? 13.6 0.0175 mol NaCl in 1 L of solution 0.1 g NaCl in 100 mL of solution 0.5 g NaCl in 500 mL of solution 0.25 mol NaCl in 200 mL of solution All have the same concentration.

  13. Which of the following would be worst at conducting electricity? 13.7 NaCl (aq) NH4NO3 (aq) H2O (l) MgCl2 (aq) HF (aq)

  14. Which of the following would be worst at conducting electricity? 13.7 NaCl (aq) NH4NO3 (aq) H2O (l) MgCl2 (aq) HF (aq)

  15. How is the solubility of a gas affected by the temperature of the solution? 13.8 Solubility increases with increasing temperature. Solubility increases with decreasing temperature. Solubility remains the same with increasing temperature. Solubility decreases with decreasing temperature. Two of the above

  16. How is the solubility of a gas affected by the temperature of the solution? 13.8 Solubility increases with increasing temperature. Solubility increases with decreasing temperature. Solubility remains the same with increasing temperature. Solubility decreases with decreasing temperature. Two of the above

  17. Which type of interaction must be strong in order to dissolve a salt? 13.9 Solvent–solvent Solvent–solute Solute–solute Solvent–solution All of the above

  18. Which type of interaction must be strong in order to dissolve a salt? 13.9 Solvent–solvent Solvent–solute Solute–solute Solvent–solution All of the above

  19. If the solubility of potassium nitrate at 20°C is 37 g per 100 g of water, how many grams of the compound will dissolve in 1.0 mL of water? 13.10 37 g 3.7 g 0.37 g 0.0037 g 370 g

  20. If the solubility of potassium nitrate at 20°C is 37 g per 100 g of water, how many grams of the compound will dissolve in 1.0 mL of water? 13.10 37 g 3.7 g 0.37 g 0.0037 g 370 g

  21. What happens to the solubility of a gas when the pressure above a liquid increases? 13.11 The solubility remains the same The solubility increases The solubility decreases It depends on the chemical nature of the gas It depends on the numerical value of the pressure

  22. What happens to the solubility of a gas when the pressure above a liquid increases? 13.11 The solubility remains the same The solubility increases The solubility decreases It depends on the chemical nature of the gas It depends on the numerical value of the pressure

  23. How many grams of KNO3 are in a 125-g solution containing 14.5% solute? 13.12 12.5 g 14.5 g 18.1 g 111 g 862 g

  24. How many grams of KNO3 are in a 125-g solution containing 14.5% solute? 13.12 12.5 g 14.5 g 18.1 g 111 g 862 g

  25. The molarity of a solution is defined asthe number of: 13.13 Moles of solute per liter of solution Moles of solute per kg of solution Grams of solute per liter of solution Moles of solute per kg of solvent Grams of solvent per kg of solution

  26. The molarity of a solution is defined asthe number of: 13.13 Moles of solute per liter of solution Moles of solute per kg of solution Grams of solute per liter of solution Moles of solute per kg of solvent Grams of solvent per kg of solution

  27. Calculate the mass percent of 2.50 moles of NaOH in 0.900 L of water at 25 °C? Hint: The density of water is 1.00 g/mL at 25 °C. 13.14 10.0% 9.09% 71.4% 2.50% 40.0%

  28. Calculate the mass percent of 2.50 moles of NaOH in 0.900 L of water at 25 °C? Hint: The density of water is 1.00 g/mL at 25 °C. 13.14 10.0% 9.09% 71.4% 2.50% 40.0%

  29. What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution? 13.15 0.049 M 204 M 2.45 M 0.500 M 4.90 M

  30. What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution? 13.15 0.049 M 204 M 2.45 M 0.500 M 4.90 M

  31. What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution? 13.16 53.3 M 1.33 M 0.00133 M 4.00 M 0.0533 M

  32. What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution? 13.16 53.3 M 1.33 M 0.00133 M 4.00 M 0.0533 M

  33. Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water. 13.17 0.234 mL 0.250 mL 1.39 mL 14.6 mL 234 mL

  34. Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water. 13.17 0.234 mL 0.250 mL 1.39 mL 14.6 mL 234 mL

  35. A practical problem. How could you safely prepare 500 mL of 1.00 M H2SO4 solution from a 12.4 M H2SO4 stock solution? Select the closest answer. 13.18 Add 40.3 mL of 12.4 M stock to 500 mL of water. Add 12.4 mL of 12.4 M stock to 500 mL of water. Add 40.3 mL of 12.4 M stock to 459.7 mL of water. Add 459.7 mL of water to 40.3 mL of 12.4 M stock. Add 500 mL of water to 40.3 mL of 12.4 M stock.

  36. A practical problem. How could you safely prepare 500 mL of 1.00 M H2SO4 solution from a 12.4 M H2SO4 stock solution? Select the closest answer. 13.18 Add 40.3 mL of 12.4 M stock to 500 mL of water. Add 12.4 mL of 12.4 M stock to 500 mL of water. Add 40.3 mL of 12.4 M stock to 459.7 mL of water. Add 459.7 mL of water to 40.3 mL of 12.4 M stock. Add 500 mL of water to 40.3 mL of 12.4 M stock.

  37. What volume of 0.100 M sodium hydroxide is required to completely neutralize 50.0 mL of 0.100 M phosphoric acid? 13.19 50.0 mL 100. mL 150. mL 200. mL 250. mL

  38. What volume of 0.100 M sodium hydroxide is required to completely neutralize 50.0 mL of 0.100 M phosphoric acid? 13.19 50.0 mL 100. mL 150. mL 200. mL 250. mL

  39. 35.0 mL of 0.155 M lead(II) nitrate and 45.0 mL of 0.287 M potassium chloride are mixed. How much precipitate is produced? 13.20 0.877 g 1.25 g 1.51 g 1.80 g 3.59 g

  40. 35.0 mL of 0.155 M lead(II) nitrate and 45.0 mL of 0.287 M potassium chloride are mixed. How much precipitate is produced? 13.20 0.877 g 1.25 g 1.51 g 1.80 g 3.59 g

  41. Which of the following is NOT an example of a colligative property? 13.21 Osmotic pressure Freezing point depression Boiling point depression Boiling point elevation All are colligative properties.

  42. Which of the following is NOT an example of a colligative property? 13.21 Osmotic pressure Freezing point depression Boiling point depression Boiling point elevation All are colligative properties.

  43. Calculate the molality of a solution containing 0.455 mol of sucrose (table sugar) and 1.00 L of water at a temperature at which the water has a density of 1.00 g/mL. 13.22 0.455 m 455 m 0.910 m 910. m 4.55 x 10-4 m

  44. Calculate the molality of a solution containing 0.455 mol of sucrose (table sugar) and 1.00 L of water at a temperature at which the water has a density of 1.00 g/mL. 13.22 0.455 m 455 m 0.910 m 910. m 4.55 x 10-4 m

  45. What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.) 13.23 -1.4 °C 1.4 °C 4.2 °C 0.0 °C -4.2 °C

  46. What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.) 13.23 -1.4 °C 1.4 °C 4.2 °C 0.0 °C -4.2 °C

  47. To the nearest degree, calculate the boiling point of an aqueous solution containing 36 g NaCl in 100 ml of water. (Note: Kb = 0.512 °C·kg/molparticles.) 13.24 6 °C 94 °C 97 °C 103 °C 106 °C

  48. To the nearest degree, calculate the boiling point of an aqueous solution containing 36 g NaCl in 100 ml of water. (Note: Kb = 0.512 °C·kg/molparticles.) 13.24 6 °C 94 °C 97 °C 103 °C 106 °C

  49. A red blood cell with an inner concentration of 0.9 g NaCl per 100 mL of solution is placed into a 2.0 g NaCl per 100 mL solution. The cell: 13.25 Shrinks Swells Leaks Bursts Two of the above

  50. A red blood cell with an inner concentration of 0.9 g NaCl per 100 mL of solution is placed into a 2.0 g NaCl per 100 mL solution. The cell: 13.25 Shrinks Swells Leaks Bursts Two of the above

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