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Ionic solids generally dissolve better in Polar solvents like water
whereas a molecular compound usually favors non-polar solvents.
moleculues with OH- groups in its structure will dissolve in water due to hydrogen bonding with water enhancing solubility |
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(g of solute/ g of solute + g of solvent) * 100%
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| (Moles of solute/ volume of solution in (L)) |
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pure solvent vs. solution |
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Pure solvent Solution
vapor pressure- higher lower
boiling point- lower higher
frezzing point- higher lower |
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| =( mole of solute/ mass of solvent) |
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ΔT= difference of two frezzing points or the differnce of two boiling points
K= the constant
m=molality (mole of solute/kg of solvent) |
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solvent-solute interations > solvent-solvent and solute- solute interations |
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Solvent- solute interations= solvent-solvent and solute-solute interations |
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solvent-solute interations< solvent-solvent and solute-solute interations |
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| solution may or may not form, depending on relative disparity |
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| The movement of wayer from low solute concentration to hight solute concentration through a semipermiable membrane, thus generating osmotic pressure |
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| ionic compounds dissociate in soulution thus doubleing the concentration |
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a mixture in which a dispersed substance is finely divided in a dispersing medium.
size between 1nm-1000nm |
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| concentration changes and the rate also changes at the same magnitude |
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| concentration changes however rate remains unchanged |
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| when concentration changes and rate change at a greater magnitude |
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