Nonelectrolytes do not form ions in solution but dissolve as whole molecules

Nonelectrolytes do not form ions in solution but

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Nonelectrolytes do not form ions in solution but dissolve as whole molecules. Examples of strong electrolytes are ionic compounds such as NaCl, KBr, MgCl 2 , NaNO 3 ; weak electrolytes are HF, NH 3, H 2 CO 3 and CH 3 COOH; nonelectrolytes are
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mostly organic compounds such as CH 3 OH (Methanol), C 2 H 5 OH (Ethanol), and C 12 H 22 O 11 (Sucrose). Not all ions have the same charge. An equivalent measures the electrical charge (+ or -) carried by one mole of the ions. 1 mole Na + = 1 mole Cl - =1 Eq 1 mole Ca 2+ = 2 Eq 1 mole Al 3+ =3Eq 9.3 Solubility Solubility is the maximum ratio of the amount of solute soluble in 100 g of solvent at a given temperature. Solubility is often expressed in numbers of grams of solute/100 g of H 2 O. Saturated solution contains the maximum amount of dissolved solute at a certain temperature or its solute and solvent ratio equal or greater than the solubility. If a solute readily dissolves when added to the solvent, the solution doesn't contain the maximum amount of solute. We call the solution unsaturated solution, more solute can be dissolved in the solvent in the set conditions (temperature and pressure). Supersaturated solution contains more than the amount of solute that can be dissolved. It is actually possible under controlled circumstances to create a supersaturated solution where more solute is dissolved than the maximum. For example, a saturated sugar solution at room temperature can be made into a supersaturated solution: by 1) increase its temperature to dissolve all the sugar crystals, 2) let the solution slowly cool down to room temperature. This solution is extremely unstable but if it is carefully and slowly cooled, it is possible to retain its supersaturated status for a short while. If however it is agitated or an additional crystal of sugar is added, the excess solute crystallizes again.
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