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12 Cards in this Set
- Front
- Back
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solution=
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solute (s, l, or g) + solvent (s, l, or g)
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typical solvent=
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H2O
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saturated solution=
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a solution that has the maximum concentration of solute possible
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unsaturated solution=
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can still dissolve more solute
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super saturated solution=
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has a higher concentration of solid solute (dissolved) than is supposed possible. prepared by heating a saturated solution (increases solubility of the solute, dissolving more) and letting it cool.
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conductivity
strong electrolytes weak electrolytes non electrolytes |
- solutes that, when dissolved, give a solution the ability to conduct electricity are called electrolytes
- soluble ionic compounds - strong acids - weak acids - low solubility ionic compounds - soluble molecules |
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Arrhenius theory
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ionic compounds must 'dissociate' to dissolve
NaCl(s) --> Na+(aq) + Cl-(aq) these ions are mobile in the water and charged so they can carry electrical current |
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low solubility
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AgCl(s) --> Ag+(aq) + Cl-(aq)
rxn is highly unsuccessful. these ions have very low concentration b/c AgCl doesn't dissolve well. poor conductivity. |
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solubility
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ionic compounds-solubility table
molecular compounds - polar solvents only dissolve polar solutes. non polar solvents only dissolve non polar solutes. ("like dissolves like") |
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molarity
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- concentration of a solution
- ratio of moles of solute per litre of SOLUTION - unit is mol/L or M |
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determine the [NaCl] if 1.75g of NaCl(s) is dissolved in water to make 375mL of solution
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1.75gNaCl * (1molNaCl/58.44gNaCl) * (1/375mL) * (1000mL/1L)= 0.0799M
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what mass of NaHCO3 (sodium bicarbonate) must be dissolved in water to make 1.50L of a 2.55M solution?
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1.50L * (2.55mol NaHCO3/ L) * (84.01gNaHCO3/ 1mol)= 321g NaHCO3
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