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Ksp (Chapter 15)

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by: Mythri Partha

Ksp (Chapter 15) CHEM 1332

Mythri Partha

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About this Document

These notes cover Solubility product constant (Ksp)
Fundamentals of Chemistry 2
Simon Bott
Class Notes
chemistry 2
25 ?




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This 2 page Class Notes was uploaded by Mythri Partha on Thursday April 14, 2016. The Class Notes belongs to CHEM 1332 at University of Houston taught by Simon Bott in Spring 2016. Since its upload, it has received 44 views. For similar materials see Fundamentals of Chemistry 2 in Chemistry at University of Houston.


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Date Created: 04/14/16
K sp To begin:   Solubility (S)  K (Solubility product constant) sp  In a reaction: (Cation)  nAnion) (sm    n Cation(aq) + m Anion(aq): n m K sp Q =  [Cation] [Anion] At a certain temperature: All salts have a given constant K sp If: Q= K  : Solution is saturated sp Q> K  spA solid precipitate is formed in the reaction Q< K  spSolution is considered unsaturated Solubility – Measure of how to make saturated solution Either gram solubility (how many grams in a given volume) or MOLAR solubility (S, how many moles per liter of saturated solution) Relationships between S and K sp 1. Write an equation where the salt is dissolved and dissociated (review ions from previous  chapters) 2. Write an expression to help solve for K sp 3. Write out concentration in terms of S (you can get that by using stoichiometry) 4. Substitute the concentrations into the K exprsp ion Example: Say you are given AgCl (K valusp  1.8*10 ) Determine the molar solubility  + ­ 1) AgCl(s)   Ag (aq) + Cl(aq) 2) Ksp = [Ag ][Cl] ­ + ­ 3) [Ag ] = S, [Cl] = S 4) Ksp = S 2 1.8*10^(­10) = S  so, S=1.3*10 ­5 Solubility can also be expressed in g/L, but is mainly expressed in mol/L (M) K can also be used to predict whether or not a precipitate will form, but Q has to be greater than sp  K sp LeChatlier’s Principle  Ionic compounds become less soluble in solutions in which appropriate ions are present.   Effect of pH (acidic solutions): as you add acid the acidic solution gets neutralized (X  is  ­ removed from the solution). Reaction goes to completion to the right (products) For example: MX(s)  M (aq) + S(aq) ­  More MX can dissolve Ionic compounds can become more soluble in acidic solutions UNLESS the anion is ­ ­ ­ ­ ­ Cl, Br, NO , C3O , or4I REMEMBER K sp ONLY used for insoluble solutions/solids ALL OTHER SOLUTIONS ARE THERE TO GIVE IONS ONLY Watch for tricks: Think about where ions came from; do you multiply [] by stoichiometry of insoluble salt or not?  (usually yes when using S as molar solubility, NO  when ions comes from elsewhere) Remember, pH or pOH can give [H ] or [OH]  ­


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