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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.

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Solubility

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  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

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