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Chapter 15-16 Practice Problems
Transcript of Chapter 15-16 Practice Problems
amount of carbon dioxide that could be
dissolved in the soda. (This is why heating DOESN'T always increase the amount of solute that can dissolve.) 2. You add 12.01 g table salt to 2.5 L of water. What is the molarity of the solution? 3. You add 0.109 g of solute to 3 L of water, which yields a solution with a molarity of .001 mol/L. What is the solute's molar mass? 1. A 1.07 M solution has a volume of 300 mL. How many moles of solute are in the solution? Answers 1. 0.321 mol
2. 1.95 M
3. 36.5 g/mol
4. HCl I'm happy to answer any more questions you may have. Don't be shy about raising your hand! :D Great job! Good luck on your test! 1. What will NOT dissolve in water? Why? What kind of solvent would you need to dissolve such compounds? Questions 2. Why does alcohol evaporate faster than water? 3. Alcohol's boiling point is 78.4ºC. What is the boiling point of water? Why is this? Answers 1. Nonpolar compounds, because water uses its polarity to help break up other polar compounds. You would need another nonpolar solvent.
2. Hydrogen bonding. (the answer to everything in Ch 15)
3. 100 ºC. Again, hydrogen bonding makes the water molecules "want to stay" in the water. 4. Bonus points! If the solute in question 3 is a strong electrolyte and an inorganic acid, can you guess what it is? Questions