1 / 24

Molarity

Molarity. Molarity = grams / molar mass / Liters Liters = grams / molar mass/ Molarity Grams = Molarity x Liters x molar mass. Molarity. The higher the number the more concentrated Which solution is more concentrated? 1 M 3.5 M 0.5 M 2.0 M. Molarity Review.

schuyler
Download Presentation

Molarity

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Molarity • Molarity = grams / molar mass / Liters • Liters = grams / molar mass/ Molarity • Grams = Molarity x Liters x molar mass

  2. Molarity • The higher the number the more concentrated • Which solution is more concentrated? 1 M 3.5 M 0.5 M 2.0 M

  3. Molarity Review • What is the molarity of a solution containing 400 grams of lithium chloride in 500 mL of water?

  4. Molarity Review • If you a 4.5 M solution with 35 g of NaCl, how many liters do you have?

  5. Molarity Review • You need to prepare 800 mL of a 1.5 M solution of magnesium oxide. How many grams do you need?

  6. Dilutions Section 15.2 • Dilute = add more solvent • Moles of solute do not change. Therefore… moles of solute before = moles of solute after M1V1 = M2V2

  7. Dilutions • Volume does not have to be in Liters • Each side the equation must have the SAME VOLUME UNITS Molarity x mL = Molarity x mL or Molarity x L = Molarity x L

  8. Dilutions • Stock solution • The original solution that gets diluted to get the desired concentration of the new solution

  9. M1V1 = M2V2 1. How much stock solution do I need to prepare 500 mL of a new solution with a concentration of 4.5 M if the stock solution is 11.6 M?

  10. M1V1 = M2V2 2. What volume of a 3 M KI solution would you use to make 0.3 L of a 1.25 M KI solution?

  11. M1V1 = M2V2 3. How many milliliters of a 5 M H2SO4 solution would you need to prepare 100 mL of a 0.25 M solution?

  12. M1V1 = M2V2 4. If you dilute 20 mL of a 3.5 M solutions to make 100 mL solution, what is the molarity of the dilute solution?

  13. M1V1 = M2V2 5. What is the molarity if 1279 g of K3PO4 is dissolved in 4 L of water?

  14. 5. What is the molarity if 1279 g of K3PO4 is dissolved in 4 L of water?

  15. M1V1 = M2V2 6. If you dilute 50 mL of a 6 M solution to make 200 mL solution, what is the molarity of the new solution?

  16. 7. How many grams of magnesium sulfate would be dissolved in 1 L to make a 0.3 M solution?

  17. 8. If 0.65 g of a gas dissolves in 1 L of water at 2 atmospheres of pressure, how much will dissolve at 22 atmospheres of pressure?

  18. 15.3 Colligative Properties • Colligative = “depends on the collection” • Properties that depend on how many solute particles are present • Does NOT depend on identity of solute

  19. Pure solvent Solution Vapor Pressure Lowering • Vapor pressure = pressure created by particles going from liquid to gas inside a closed container • If you add solute, not as much solvent can escape into the gas phase

  20. Solution Boiling Point Elevation • Boiling = liquid to gas • The more solute added to a solution, the lower the vapor pressure and therefore the higher the boiling point

  21. A solvent has a boiling point of 200°C. When 10 grams of salt is dissolved in the solvent, what is the most likely new boiling point? a. 210°C b. 200°C c. 190°C

  22. Freezing Point Depression • Freezing = solvent particles moving into solid crystalline form • Solute gets in the way of making crystals preventing the solvent from freezing. Lower temperature is needed to freeze

  23. A solvent has a freezing point of 10°C. What is the most likely freezing point if 5 grams of salt is mixed with the solvent? a. 5°C b. 10°C c. 15°C

  24. Osmotic Pressure Increase • Osmosis-movement of water from low to high concentration. Goal is to balance the concentrations • Osmotic Pressure Increases

More Related