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Published byAleksander Bogumił Rutkowski Modified over 5 years ago
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Ksp Values that indicate how soluble a solute is.
Leads us to calculate the molarity of ions in solution.
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Solubility Equilibrium
All compounds ionize to some extent: PbCl2(s) ↔ Pb+2(aq) + 2Cl-1(aq) NaCl(s) ↔Na+(aq) + Cl-(aq) Solubility constants are known values for the relative solubility in room temp Ksp for PbCl2 = 1.6 x 10-5 Ksp for NaCl = 36 smaller number = less soluble
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Which substance is more soluble?
CaCO3 Ksp = 4.7 x10-9 Mg(OH)2 Ksp = 8.8 x 10-12 The larger the number the more soluble the substance is
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Solubility Product Expression
Is written from the ionization of the compound PbCl2(s) ↔ Pb+2(aq) + 2Cl-1(aq) Ksp = [Pb+2][Cl-1]2 multiply
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Practice problem The solubility product constant of lead II chloride is 1.6 x 10-5 at 25oC. Calculate concentrations of the lead & chloride ions in solution. Step 1: write ionization reaction Step 2: assign Xs Step 3: solubility product expression Step 4: substitute using Xs & solve [Pb+2] = 1.6x10-2 [Cl-] = 3.2x10-2
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How did you get those answers??????
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The [Ni2+] in a saturated solution of nickel II hydroxide is 2
The [Ni2+] in a saturated solution of nickel II hydroxide is 2.2x10-12 M. What is the Ksp? 4.26x10-35
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How did you get THAT??????
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The Ksp of aluminum sulfate is 1. 42 x 10-12 at 25oC
The Ksp of aluminum sulfate is 1.42 x at 25oC. Calculate the concentrations of the aluminum ions and sulfate ions in a saturated solution. [Al+3] = 3.3x10-3 M or mol/L [SO4 -2] = 5.0x10-3 M or mol/L
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How did you get THAT??????
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The ENd
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