E-Storeliquid solutions
SOLUTIONS
- homogenous mixture of 2 or more pure substances
- solution = solvent + solute
- solvent = present in large amount
= decides physical state of solution
| type | solute | solvent | example |
| gaseous | gas | gas | O2 + N2 |
| liquid | gas | ChCl3 + N2 | |
| solid | gas | camphor + N2 | |
| liquid | gas | liquid | O2 + water |
| liquid | liquid | alcohol + water | |
| solid | liquid | sugar + water | |
| solid | gas | solid | H2 + Pd |
| liquid | solid | Hg + Na | |
| solid | solid | Cu + Au |
- solubility : max. amount of solute that can be dissolved in a given amount of solvent at given temperature and pressure
- like dissolves like
- vapour pressure : pressure exerted by the vapors of liquid which are in equilibrium with it at a given temperature
- v.p. depends on temperature and nature of liquid.
- Raoult's law : P ∝ Xsolvent or P = P0 Xsolvent (for non volatile solute)
- Ideal solution: (i) obey this law over entire range of concentration (ii) ΔHmix = 0 ; ΔVmix = 0
- for volatile solute, P = P0A Xa + P0B XB
- for binary solution : Xa + XB = 1
- yA = PAo/ P (yA = mole fraction of A in vapor state when immiscible liquids)
- vapor pressure ↑boiling point ↓
- vapor pressure of 2 immiscible liquids(i) yA / yB = P0A / P0B = nA / nB
- (ii) Xa + XB ≠ 1
- non ideal solutions: don't obey Raoult's law
| s.n. | + ve deviation | -ve deviation |
| 1. | PA > P0A Xa PB > P0B XB | PA < P0A Xa PB < P0B XB |
| 2. | A--B < A--A / B--B | A--B > A--A/B--B |
| 3. | ΔHmix > 0 ΔVmix > 0 | ΔHmix < 0 ΔVmix < 0 |
| 4. |
| |
| e.g. | ethanol + cyclohexane | chloroform + acetone |
- Azeotropes = constant boiling mixtures. Components cannot be separated by fractional distillation
- Min. boiling aze. = b.p. < b.p. of A & B (large +ve deviation)
- Max. boiling aze. = b.p. > b.p. of A & B (large –ve deviation)
moles of solute
1. Molarity (M) = ------------------
volume of solution (L)
moles of solute
2. Molality (m) = ------------------------
mass of solvent (kg)
moles of solute
3. Mole fraction (Ca) = ------------------------
moles of solute + solvent
Mass of solute
4. Mass (w/w) % = ------------------------ x 100
Mass of solution
Volume of solute
5. Volume (v/v) % = ------------------------ x 100
Volume of solution
Mass (volume) of solute
6. ppm (w/w or v/v) = ---------------------------- x 106
Mass (volume) of solution
Mass (volume) of solute
7. ppb (w/w or v/v) = ------------------------------ x 109
Mass (volume) of solution
hey its original. not copy pasted.
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