1 / 14

Solubility

Solubility. ~A measure of how soluble something is. Nothing is completely soluble or completely insoluble. Increasing the temperature normally increases the amount of a solid solute a solution can hold. Gases dissolved in a liquid. Colder solutions hold more of a gaseous solute.

kuper
Download Presentation

Solubility

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. Solubility • ~A measure of how soluble something is. • Nothing is completely soluble or completely insoluble. • Increasing the temperature normally increases the amount of a solid solute a solution can hold.

  2. Gases dissolved in a liquid • Colder solutions hold more of a gaseous solute. • Heating a solution forces gases to come out of solution (pre-boiling bubbles) • Higher pressure solutions can hold more gases. • ~Why a pop can fizzes when opened

  3. Decompression Sickness • If you dive deep into the ocean (submarine or scuba) the pressure increases • More gases will dissolve in the fluids of your body • If you rise too quickly, gases dissolved in the fluids of your body will come out of solution • This painful and deadly situation is called decompression sickness or “the bends”

  4. Saturation • Saturated solution- solution that has all the solute it can hold. If any more is added it will not dissolve. • Supersaturated solution- a soln. holding more solute than it should • Made by heating a solution to dissolve more solute and then cooling it. • If you disturb a supersaturated solution the solute will fall out of solution.

  5. Other units of concentration

  6. Dilution Equation • MV = MV • Molarity (volume) before dilution = molarity (volume) after dilution • How many liters of 12 M H2SO4 do you need to make 1.2 L of .75 M? • 12 M (V) = .75 M (1.2 L) • V = .075 L (75 mL)

  7. Mass Percent • Mass percent = mass of solute x 100 • mass of solution • Or = grams of solute x 100 • grams of solute + grams of solvent

  8. Problem • 35 g of NaCl is dissolved in 115 g of water, what is the mass percent? What is the molarity if the final solution has a density of 1.1 g/mL? • 35 g / (35g + 115g) x 100 • 23 % • 35 g x 1 mol/ 58.44 g= .5989 molNaCl • 150 g x 1mL / 1.1 g = 136.36 mL = .13636L • M = .5989 mol / .13636 L • M = 4.4 M

  9. Convert • Convert 1.2 M CuSO4 solution to mass percent, if the solution has a density 1.1 g/mL. • 1.2 M= 1.2 mol CuSO4 / 1 L solution • 1.2 mol x159.62 g / 1 mol =191.544 g • 1 L = 1000 mL x 1.1 g/1 mL = 1100 g of solution • Mass percent = 191.544 g / 1100 g x100 = 17 %

  10. Another 55 g of CaCl2 is dissolved in 115 g of water, what is the mass percent? What is the molarity if the final solution has a density of 1.1 g/mL?

  11. More Convert 1.9 M Ca(NO3)2 solution to mass percent, if the solution has a density 1.3 g/mL.

  12. Parts per thousand/million etc. • Mass percent can also be called parts per hundred (although it never is) • Parts per thousand is the same as mass percent except instead of multiplying by a 100 you multiply by 1000. • Parts per million is multiplied by 1,000,000 • Pollen counts are normally reported in this

More Related