EQUALIBRIUM - Soluability, Precipitation and Complex Ion Equalibria

9 important questions on EQUALIBRIUM - Soluability, Precipitation and Complex Ion Equalibria

What is solubility product? Ksp?

It is the equilibrium constant for equilibrium established between a solid solute and its ions in saturated solution

What is a saturated solution?

A solution with the max concentration of dissolved ions with the solution in contact with extra undissolved solids.

How to determine the Ksp from solubility?

  1. Determine your concentrations
  2. Make an ICE Table (solid breaking down to its components)
  3. Solve for Ksp using solubility
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How to determine the solubility from the Ksp?

  1. Make an ICE table (solids break down to its components)
  2. Solve for the solubility using the Ksp value and the variables you used for the ICE table.

What units do soluability when determined from the Ksp?

ANS: mol/L unit

Which has a larger Ksp?
  1. AgI (2# of ions) Ksp = 8.5*10^-17 ; solubility = 9.2*10^-9
  2. CuI (2# on ions) Ksp = 1.3*10^-12 ; solubility = 1.1*10^-6

CuI would have the larger ksp

What is the Common Ion Effect?

  • It is when a weak acid is added to a salt which contains the same anion
  • EX: HNO2 and NaNO2

How to determine if the given initial ion will result in a precipitation of an insoluble solid?

You must use the reaction Quotient, Q
  • Q>Ksp reaction will proceed LEFT, Precipitation occurs
  • Q<Ksp reaction will proceed RIGHT, No precipitation
  • Q =Ksp solution is saturated, no precipitation occurs

What are examples of soluble?

  1. Nitrates (NO3-) salts
  2. Alkali metals (Group 1)
  3. Ammonium salts
  4. Cl, Br, I salts except with Ag+, Pb2+, Hg2+
  5. Sulfates salts except with Sr2+, Ba2+, Pb2+, Hg2+

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