Solubility

# Solubility - Chapter17(Continued Ksp Solubility 1...

This preview shows pages 1–8. Sign up to view the full content.

Chapter 17 (Continued) Solubility equilibrium K sp Factors affecting solubility 1 Solubility

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
SOLUBILITY l bilit tit f bt th t di l t f Solubility: quantity of a substance that dissolves to form a saturated solution Solubility: g/L Molar solubility: mole/L Some salts are very soluble (> 0.1 M). Some salts are sparingly soluble (< 0.1 M) sometimes referred to as soluble’. Recall solubility rules (Chapter 4.2). insoluble . Precipitation and Solubility of ionic salts and their equilibrium in water MA(s) M + (aq) + A (aq) 2 Solubility
SOLUBILITY EQUILIBRIA Precipitation i l ti Dissolution hen forward rate = backward te: equilibrium When forward rate backward rate: equilibrium AgCl (s) Ag + (aq) + Cl (aq) K eq = [Ag + (aq) ][Cl (aq) ] [AgCl (s) ] K eq [AgCl (s) ] = [ Ag + ][Cl ] The concentration of solid does not change at equilibrium 3 Solubility K sp = [Ag + ][Cl ]

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
K SP - SOLUBILITY PRODUCT CONSTANT The solubility product is equal to the product of the concentrations of the ions involved in the quilibrium each raised to the power of it’s co equilibrium, each raised to the power of it s co efficient. sp constant for a given solid at a given Ksp is constant for a given solid at a given Temp. olubility = amount of CaF issociated Solubility amount of CaF 2 dissociated s= 2.14 x 10 4 mol/lit aF ) a +2 q 2F q CaF 2 (s) Ca (aq) + 2F (aq) -s + s +2 s sp = [Ca 2+ F - 2 = s (2s) 2 =4s 3 = 9 x 10 11 Ksp [Ca ][F ] s.(2s) 4 s 3.9 x 10 Ksp of CaF 2 =3.9 x 10 11 at 25 o C
Solubility Products Solubility Product: K sp AgCl 1.8 × 10 10 AgBr 5.0 × 10 13 AgI 8.3 × 10 17 CdS 8.0 × 10 27 ZnS 1.1 × 10 21 Mg(OH) 2 1.8 × 10 11 6 Ca(OH) 2 5.5 × 10 CaF 2 3.9 × 10 BaCO 3 5.1 × 10 9 aSO 1 0 1 BaSO 4 1.1 × 10 0 5

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
SOLUBILITY CALCULATION Calculate [Ca 2+ ], [F ] for a saturated CaF 2 sol’n. F ) + ) + 2F ) CaF 2 (s) Ca 2+ (aq) + 2F (aq) x2 x K sp = [Ca 2+ ][F ] 2 = x(2x) 2 = 4x 3 = 3.9 x 10 11 = [Ca 2+ = 2.14 x 10 4 x [Ca ] 2.14 x 10 M [F ] = 2x = 4.3 x 10 4 M CaF 2 solubility = 2.14 x 10 4 moles/liter
Ksp of PbI 2 (4 x 10 8 ) PbI 2 (s) = Pb 2+ + 2 I Start with I lit. of 0.01 M Pb 2+ Add I (1M KI) to cause ppt.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

## This note was uploaded on 10/04/2011 for the course CHEM 437623 taught by Professor Sherylrummel during the Spring '10 term at Penn State.

### Page1 / 27

Solubility - Chapter17(Continued Ksp Solubility 1...

This preview shows document pages 1 - 8. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online