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ANALYTICAL CHEMISTRY CHEM 3811 CHAPTER 12. DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university. CHAPTER 12 CHEMICAL EQUILIBRIUM CALCULATIONS. SOLUBILITY. - A measure of how much of a solute can be dissolved in a solvent - PowerPoint PPT Presentation
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ANALYTICAL CHEMISTRY CHEM 3811
CHAPTER 12
DR. AUGUSTINE OFORI AGYEMANAssistant professor of chemistryDepartment of natural sciences
Clayton state university
CHAPTER 12
CHEMICAL EQUILIBRIUM CALCULATIONS
- A measure of how much of a solute can be dissolved in a solvent
- Units: grams/100 mL
Three factors that affect solubility- Temperature
- Pressure- Polarity
SOLUBILITY
- Most nitrate (NO3-) salts are soluble
- Most salts of alkali metals (Group 1A) and ammonium (NH4
+) are soluble
- Most salts containing Cl-, Br-, and I- soluble Exceptions: salts of Ag+, Hg2
2+, Pb2+
SOLUBILITY OF SALTS
- Most sulfate salts are solubleExceptions: BaSO4, PbSO4, Hg2SO4
- Most hydroxides are slightly solubleHydroxides of Ba2+, Sr2+, and Ca2+ are marginally soluble
- Most salts containing S2-, CO32-, PO4
3-, CrO42- are insoluble
Exceptions: salts of alkali metals and NH4+
SOLUBILITY OF SALTS
- Solubility increases when soluble salts are addedto solutions of marginally soluble salts
- Cations are surrounded by anions to create a netnegative ionic atmosphere
- Anions are surrounded by cations to create a netpositive ionic atmosphere
- The net charges are less than those of the cation or anion alone
SOLUBILITY OF SALTS
- The attraction between ions in solution is decreasedwhich increases solubility
- Increasing the concentration of ions in solution decreasesthe attraction between ions and increases solubility
- Increasing concentration of ions increases ion dissociation
SOLUBILITY OF SALTS
IONIC STRENGTH
- A measure of the total concentration of ions in solution
.........zczczc21zc
21μ 2
ii2ii
2ii
i
2ii
µ = the ionic strengthci = the concentration of the ith species
zi = the charge on the ith species
IONIC STRENGTH
Find the ionic strength of 0.0250 M Na2SO4
Na2SO4 ↔ 2Na+ + SO42-
[Na+] = 2 x 0.0250 M = 0.0500 M
[SO42-] = 0.0250 M
0750.0)2)(0250.0(1)(0.0500)(21μ 22
IONIC STRENGTH
For 1:1 electrolytes (NaCl, NaNO3, KBr)
The ionic strength is equal to the molarity1:1 µ = molarity
For any other stoichiometryThe ionic strength is greater than the molarity
2:1 µ = 3 x molarity3:1 µ = 6 x molarity2:2 µ = 4 x molarity
ACTIVITY COEFFICIENT
Consider the equilibrium for the reaction
aA + bB ↔ cC + dD
The equilibrium constant (K) is given by
ba
dc
[B][A][D][C]K
K does not account for the effect of ionic strength
ACTIVITY COEFFICIENT- Activities (A) are used in place of concentrations
to account for ionic strength
A = [ ] x γ
where γ is the activity coefficient
- Activity coefficient depends on ionic strength
- Activity coefficient is 1 when there is no effect of ionic strength
- Activity coefficient decreases with increasing ionic strength
ACTIVITY COEFFICIENT
bB
baA
a
dD
dcC
c
bB
aA
dD
cC
γ[B]γ[A]γ[D]γ[C]
AAAAK
- K is generally expressed as follows
Debye-Hückel Equation
- Relates activity coefficients to ionic strength (at 25 oC)
/305)μ(α1μ0.51z
γlog2
γ = activity coefficientz = ion charge (±)
α = ion size in picometers (1 pm = 10-12 m)µ = ionic strength
ACTIVITY COEFFICIENT
ACTIVITY COEFFICIENT
Effects (limited to dilute aqueous solutions)
- Activity coefficient increases with decreasing ionic strength(approaches unity as ionic strength approaches zero)
- Activity coefficient depends on the magnitude of the chargebut not on the sign
(departs from unity as charge increases)
- Effect of activity on ions increases with decreasing ion size
ACTIVITY COEFFICIENT
Neutral Molecules
- Activity coefficient is assumed unity(no charge and no ionic atmosphere)
- Activity is assumed to be equal to its concentration
ACTIVITY COEFFICIENTGases
Activity (called fugacity) is written as
Agas = Pgas x γgas
P = pressure in bars
γgas = fugacity coefficient of a gas
For most gases at or below 1 barγgas ≈ 1
ACTIVITY COEFFICIENT
pH = negative logarithm of the hydrogen ion activitypH electrodes measure activity of hydrogen ions
HH]γ[HloglogApH
- Ionic strength of pure water is very low
- Activity coefficient of pure water is very close to unity
OHHw ]γ[OH]γ[HK
CHARGE BALANCE
- In a given solutionsum of positive charges = sum of negative charges
- The coefficient of each term equals the magnitude of thecharge on the respective ion
- 1 mole of an ion An+/n- contributes n moles of positive/negative charge
CHARGE BALANCE
n1[C1] + n2[C2] + ….. = m1[A1] + m2[A2] +…..
[C] = concentration of a cationn = magnitude of the charge on the cation
[A] = concentration of an anionm = magnitude of the charge on the anion
- Activity coefficient do not appear in charge balance
CHARGE BALANCE
Consider a solution containing the following speciesNa+, CO3
2-, HCO3-, H+, Ca2+, OH-, PO4
3-, HPO42-
total positive charge = total negative charge
[Na+] + [H+] + 2[Ca2+] =
2[CO32-] + [HCO3
-] + [OH-] + 3[PO43-] + 2[HPO4
2-]
MASS BALANCE
- Also called the material balance
- Conservation of matter
the quantity of a particular atom (or group of atoms)equals
the amount of that atom (or group of atoms) delivered
- Mass balance includes all products of compoundsthat dissociate in several ways
MASS BALANCE
Consider 0.0200 mol of H3AsO4 in 1.00 L of solution0.0200 M = [H3AsO4] + [H2AsO4
-] + [HAsO42-] + [AsO4
3-]
For KH2AsO4 in water[K+] = [H3AsO4] + [H2AsO4
-] + [HAsO42-] + [AsO4
3-]
For K2HAsO4 in water[K+] = 2 x {[H3AsO4] + [H2AsO4
-] + [HAsO42-] + [AsO4
3-]}
For K3AsO4 in water[K+] = 3 x {[H3AsO4] + [H2AsO4
-] + [HAsO42-] + [AsO4
3-]}
FRACTIONAL COMPOSITION
aHA K][H
][HF
[HA]α
a
a-
A K][H][K
F][Aα -
F = initial concentration of acid HA (formal concentration)
Fraction of species in the form HA
Fraction of species in the form A-
1ααAHA