Unit 11: Solutions Day 3 – Solubility Curves. Objectives 1. I can define solubility, unsaturated, saturated and and supersaturated and determine if a.

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Unit 11: Solutions Day 3 – Solubility Curves

Objectives 1. I can define solubility, unsaturated, saturated and and supersaturated and determine if a solution either of the above by writing the definitions and reading a solubility graph. 1. I can define solubility, unsaturated, saturated and and supersaturated and determine if a solution either of the above by writing the definitions and reading a solubility graph. 2. I can distinguish and understand the factors that effect solubiltity. 2. I can distinguish and understand the factors that effect solubiltity. –Temp., surface area, and aggitation

Factors affecting solubility Solubility- the amount of a substance required to form a saturated solution with a specific amount of solvent at a specific temp. ex: the solubility of sugar in water is 204 g/100 ml of water at 20 o C. ex: the solubility of sugar in water is 204 g/100 ml of water at 20 o C.

The Solution Process Consider a sugar solute with a solubility (s) of 204 g per 100ml water. The volume in the diagram is 50 mL. Consider a sugar solute with a solubility (s) of 204 g per 100ml water. The volume in the diagram is 50 mL. 80g/50ml 102 g/50ml120g/50ml

The Solution Process 1) Unsaturated solution- a solution that contains less solute than a saturated solution (solubility=204g/100ml) 80g/50ml 102 g/50ml 120g/50ml 140g/100ml 204 g/100ml 240g/100ml

The Solution Process 2) Saturated solution- a solution that contains the maximum amount of dissolved solute (solubility=204g/100ml) 80g/50ml 102 g/50ml 120g/50ml 140g/100ml 204 g/100ml 240g/100ml

The Solution Process 3) Supersaturated solution- a solution that contains more solute than a saturated solution at the same conditions (solubility=204g/100ml) 80g/50ml 102 g/50ml 120g/50ml 140g/100ml 204 g/100ml 240g/100ml Supersaturated Solution - YouTube

Solubility Curve A graph that indicates how likely a solute is to dissolve in a solvent at any given temperature. #g solute/100 g solvent Label the Y axis with “solubility”

Factors affecting solubility 1. Nature of solute/solvent (polarity) 2. PRESSURE only affects the solubility of gases. only affects the solubility of gases. pressure, increased solubility (soda) pressure, increased solubility (soda) pressure, decreased solubility (fizz) pressure, decreased solubility (fizz) Solubility of liquids and solids is not changed by changes in pressure. Solubility of liquids and solids is not changed by changes in pressure.

FYI… Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid. When a soda fizzes and rapidly releases gas its called effervescence.

3. TEMPERATURE  Increased temp of solids solubility  Increased temp of gases solubility SOLIDS GASES

Label: Unsaturated NaNO 3 Saturated NaNO 3 Supersaturated NaNO 3 Where is solubility the same? Where is the gas?

Now you try!

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