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Solubility

Solubility. Chemistry 11 Mrs. Gerber 2009-2010. “Snow Globes”. Please describe what happened as the solution in the snow globe cooled. Use pictures as well as words. After you have described what you saw and felt, tell me why you think this happened (come up with a hypothesis).

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Solubility

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  1. Solubility Chemistry 11 Mrs. Gerber 2009-2010

  2. “Snow Globes” Please describe what happened as the solution in the snow globe cooled. Use pictures as well as words. After you have described what you saw and felt, tell me why you think this happened (come up with a hypothesis). Your pictures, description and hypothesis should be approximately one typewritten page.

  3. Vocabulary Solute Solvent Solution Saturated Dilute Saturated Dissolve Concentration

  4. Key Concepts Solubility g/100mL g/L moles/L (M) C6H5CO2H (benzoic acid) 1g/75mL = g/100mL = g/L = moles/L = M

  5. Ksp Solubility product • Because the concentration of a pure solid is fairly constant it is not included in the equilibrium constant expression. • AgBr Ag+ + Br- • Ksp = [Ag+][Br-]

  6. Key concepts Equilibrium constant Concentrations are measured in M K describes what happens at equilibrium – when no more solute can be dissolved • When a slightly soluble ionic compound is added to water, some of it dissolves to form a solution. • AgBr Ag+ + Br- • This means the solid AgBr is in dynamic equilibrium with the Ag+ and Br- • K= [Ag+][Br-]/[AgBr]

  7. Ion Product (Q) The ion product of a salt is the product of the concentrations of the ions in solution. • Ksp describes equilibrium concentrations, but the ion product describes concentrations that are not necessarily equilibrium concentrations. • Q< Kspsolution is unsaturated. • Q= Kspsolution is saturated. • Q> Kspsolution is supersaturated.

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