what is the solute when 10 g of nacl is dissolved in 100 ml of water?
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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. - PowerPoint PPT PresentationTRANSCRIPT
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1. NaCl2. Na3. Cl24. H2O
5. None of the above
13.1 What is the solute when 10 g of NaCl is dissolved in 100 mL of water?
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1. NaCl2. Na3. Cl24. H2O
5. None of the above
13.1 What is the solute when 10 g of NaCl is dissolved in 100 mL of water?
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1. H2O
2. NH3
3. CH3OH
4. CH3OCH3
5. C8H18
13.2 Which solvent would be most suitable to remove grease from an object?
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1. H2O
2. NH3
3. CH3OH
4. CH3OCH3
5. C8H18
13.2 Which solvent would be most suitable to remove grease from an object?
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1. Salad dressing2. Blueberry muffin3. Wine4. Sugar5. Lead
13.3 Which of the following substances is an example of a solution?
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1. Salad dressing2. Blueberry muffin3. Wine4. Sugar5. Lead
13.3 Which of the following substances is an example of a solution?
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1. CH3CH2CH3
2. CH3OCH3
3. CH3CH2OH
4. CH3CH2NH2
5. CH3CH2COOH
13.4 In theory which of the following would have the highest solubility in gasoline (C8H18) ?
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1. CH3CH2CH3
2. CH3OCH3
3. CH3CH2OH
4. CH3CH2NH2
5. CH3CH2COOH
13.4 In theory which of the following would have the highest solubility in gasoline (C8H18) ?
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1. Holds less than the maximum amount of solute at that temperature
2. Holds the maximum amount of solute at that temperature
3. Holds more than the normal maximum amount of solute at that temperature
4. All of above5. None of the above
13.5 A supersaturated solution:
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1. Holds less than the maximum amount of solute at that temperature
2. Holds the maximum amount of solute at that temperature
3. Holds more than the normal maximum amount of solute at that temperature
4. All of above5. None of the above
13.5 A supersaturated solution:
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1. 0.0175 mol NaCl in 1 L of solution2. 0.1 g NaCl in 100 mL of solution3. 0.5 g NaCl in 500 mL of solution4. 0.25 mol NaCl in 200 mL of solution5. All have the same concentration.
13.6 Which of the following NaCl solutions has the highest concentration of NaCl?
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1. 0.0175 mol NaCl in 1 L of solution2. 0.1 g NaCl in 100 mL of solution3. 0.5 g NaCl in 500 mL of solution4. 0.25 mol NaCl in 200 mL of solution5. All have the same concentration.
13.6 Which of the following NaCl solutions has the highest concentration of NaCl?
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1. NaCl (aq)2. NH4NO3 (aq)
3. H2O (l)
4. MgCl2 (aq)
5. HF (aq)
13.7 Which of the following would be worst at conducting electricity?
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1. NaCl (aq)2. NH4NO3 (aq)
3. H2O (l)
4. MgCl2 (aq)
5. HF (aq)
13.7 Which of the following would be worst at conducting electricity?
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1. Solubility increases with increasing temperature.2. Solubility increases with decreasing temperature.3. Solubility remains the same with increasing
temperature.4. Solubility decreases with decreasing temperature.5. Two of the above
13.8 How is the solubility of a gas affected by the temperature of the solution?
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1. Solubility increases with increasing temperature.2. Solubility increases with decreasing temperature.3. Solubility remains the same with increasing
temperature.4. Solubility decreases with decreasing temperature.5. Two of the above
13.8 How is the solubility of a gas affected by the temperature of the solution?
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1. Solvent–solvent2. Solvent–solute3. Solute–solute4. Solvent–solution5. All of the above
13.9 Which type of interaction must be strong in order to dissolve a salt?
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1. Solvent–solvent2. Solvent–solute3. Solute–solute4. Solvent–solution5. All of the above
13.9 Which type of interaction must be strong in order to dissolve a salt?
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1. 37 g2. 3.7 g3. 0.37 g4. 0.0037 g5. 370 g
13.10 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?
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1. 37 g2. 3.7 g3. 0.37 g4. 0.0037 g5. 370 g
13.10 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?
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1. The solubility remains the same2. The solubility increases3. The solubility decreases4. It depends on the chemical nature of the gas5. It depends on the numerical value of the
pressure
13.11 What happens to the solubility of a gas when the pressure above a liquid increases?
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1. The solubility remains the same2. The solubility increases3. The solubility decreases4. It depends on the chemical nature of the gas5. It depends on the numerical value of the
pressure
13.11 What happens to the solubility of a gas when the pressure above a liquid increases?
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1. 12.5 g2. 14.5 g3. 18.1 g4. 111 g5. 862 g
13.12 How many grams of KNO3 are in a 125-g
solution containing 14.5% solute?
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1. 12.5 g2. 14.5 g3. 18.1 g4. 111 g5. 862 g
13.12 How many grams of KNO3 are in a 125-g
solution containing 14.5% solute?
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1. Moles of solute per liter of solution2. Moles of solute per kg of solution3. Grams of solute per liter of solution4. Moles of solute per kg of solvent5. Grams of solvent per kg of solution
13.13 The molarity of a solution is defined asthe number of:
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1. Moles of solute per liter of solution2. Moles of solute per kg of solution3. Grams of solute per liter of solution4. Moles of solute per kg of solvent5. Grams of solvent per kg of solution
13.13 The molarity of a solution is defined asthe number of:
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1. 10.0%2. 9.09%3. 71.4%4. 2.50%5. 40.0%
13.14 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.
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1. 10.0%2. 9.09%3. 71.4%4. 2.50%5. 40.0%
13.14 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.
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1. 0.049 M2. 204 M3. 2.45 M4. 0.500 M5. 4.90 M
13.15 What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution?
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1. 0.049 M2. 204 M3. 2.45 M4. 0.500 M5. 4.90 M
13.15 What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution?
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1. 53.3 M2. 1.33 M3. 0.00133 M4. 4.00 M5. 0.0533 M
13.16 What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution?
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1. 53.3 M2. 1.33 M3. 0.00133 M4. 4.00 M5. 0.0533 M
13.16 What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution?
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1. 0.234 mL2. 0.250 mL3. 1.39 mL4. 14.6 mL5. 234 mL
13.17 Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water.
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1. 0.234 mL2. 0.250 mL3. 1.39 mL4. 14.6 mL5. 234 mL
13.17 Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water.
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1. Add 40.3 mL of 12.4 M stock to 500 mL of water.2. Add 12.4 mL of 12.4 M stock to 500 mL of water.3. Add 40.3 mL of 12.4 M stock to 459.7 mL of water.4. Add 459.7 mL of water to 40.3 mL of 12.4 M stock.5. Add 500 mL of water to 40.3 mL of 12.4 M stock.
13.18 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.
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1. Add 40.3 mL of 12.4 M stock to 500 mL of water.2. Add 12.4 mL of 12.4 M stock to 500 mL of water.3. Add 40.3 mL of 12.4 M stock to 459.7 mL of water.4. Add 459.7 mL of water to 40.3 mL of 12.4 M stock.5. Add 500 mL of water to 40.3 mL of 12.4 M stock.
13.18 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.
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1. 50.0 mL2. 100. mL3. 150. mL4. 200. mL5. 250. mL
13.19 What volume of 0.100 M sodium hydroxide is required to completely neutralize 50.0 mL of 0.100 M phosphoric acid?
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1. 50.0 mL2. 100. mL3. 150. mL4. 200. mL5. 250. mL
13.19 What volume of 0.100 M sodium hydroxide is required to completely neutralize 50.0 mL of 0.100 M phosphoric acid?
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1. 0.877 g2. 1.25 g3. 1.51 g4. 1.80 g5. 3.59 g
13.20 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?
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1. 0.877 g2. 1.25 g3. 1.51 g4. 1.80 g5. 3.59 g
13.20 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?
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1. Osmotic pressure2. Freezing point depression3. Boiling point depression4. Boiling point elevation5. All are colligative properties.
13.21 Which of the following is NOT an example of a colligative property?
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1. Osmotic pressure2. Freezing point depression3. Boiling point depression4. Boiling point elevation5. All are colligative properties.
13.21 Which of the following is NOT an example of a colligative property?
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1. 0.455 m2. 455 m3. 0.910 m4. 910. m5. 4.55 x 10-4 m
13.22 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.
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1. 0.455 m2. 455 m3. 0.910 m4. 910. m5. 4.55 x 10-4 m
13.22 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.
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1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C
13.23 What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.)
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1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C
13.23 What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.)
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1. 6 °C2. 94 °C3. 97 °C4. 103 °C5. 106 °C
13.24 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.)
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1. 6 °C2. 94 °C3. 97 °C4. 103 °C5. 106 °C
13.24 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.)
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1. Shrinks2. Swells3. Leaks4. Bursts5. Two of the above
13.25 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:
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1. Shrinks2. Swells3. Leaks4. Bursts5. Two of the above
13.25 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:
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What is the freezing point of a 0.75 m aqueous solution of table sugar (sucrose)? (Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C
13.26
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What is the freezing point of a 0.75 m aqueous solution of table sugar (sucrose)? (Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C
13.26