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$$$ Quiz $$$ Solutions

$$$ Quiz $$$ Solutions. Liquids that are soluble in each other. miscible. $1. Liquids that are not soluble in each other. immiscible. $1. When a solution contains more solute than it should. supersaturated. $1. When you can’t add more solute to the solution without it precipitating out.

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$$$ Quiz $$$ Solutions

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  1. $$$ Quiz $$$ Solutions

  2. Liquids that are soluble in each other miscible $1

  3. Liquids that are not soluble in each other immiscible $1

  4. When a solution contains more solute than it should. supersaturated $1

  5. When you can’t add more solute to the solution without it precipitating out. saturated $1

  6. Solubility is usually expressed as …. grams of solute per 100 g of solvent $1

  7. What is the formula for Henry’s Law? What do the variables stand for? S = Solubility P = Pressure $2

  8. Roughly speaking, what is the difference between a dilute and concentrated solution? A dilute solution has a low amount of solute and a concentrated solution has a high amount of solute $1

  9. What is the molarity of a solution that has 15 moles of a solute in 3 liters of solution? 5 M $2

  10. What are the units of molarity? Mole/Liters $1

  11. How many moles of solute are in 1500 mL of a 0.333 M solution? 0.5 moles $2

  12. What is the name for a solid that is dissolved in a solution? Solute $1

  13. What is the name for a liquid that does the dissolving in a solution? Solvent $1

  14. What mass of CsBr (cesium bromide) is needed to make 1.5 L of a 3.0M solution? 212.8 g/mol x 4.5 moles = 957.6 grams CsBr $3

  15. True or False. When you dilute a solution, the moles of the solution stay the same. True $1

  16. If 5.0 mL of 5.0M HBr is used to make a 500 mL aqueous solution, what is the molarity of the dilute solution? M1V1=M2V2, (5)(5)=500x = 0.05M $2

  17. A solute plus a solvent gives a _______. Solution $1

  18. What is the formula for mass percent? mass solute (g) x 100% mass solution (g) $1

  19. What is the formula for parts per million (ppm)? mass solute (g) x 106 mass solution (g) $1

  20. What is the formula for volume percent? volume solute (mL) x 100% volume solution (mL) $1

  21. If the percent mass of a solution weighing 300 g is 6%, what is the mass of the solute? .06 = x/300g x = 18 g $2

  22. Name the three colligative properties we studied? • Vapor pressure lowering • Boiling point elevation • Freezing point depression $3

  23. What is the formula for freezing point depression? DTf = Kfx mxi $1

  24. What is the formula for freezing point depression? DTf = Kfx mxi $1

  25. What type of compounds are always electrolytes? Ionic compounds $1

  26. What is the formula for molality? moles solute/kg of solvent $1

  27. What is the Van’s Hoff factor of MgO? 2 $1

  28. What is the Van’s Hoff factor of Na2O? 3 $1

  29. What is the Van’s Hoff factor of SF3? 1, molecular (covalent) compound $1

  30. If you calculate a DTf of -12.3 oC for a pure substance that melts at 3.4oC, what is its new melting point? -8.9oC $1

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