Hi,
I have a problem with some calculations on tartrate solubility and etc.
Substances dissolved (in this order):
-1.0 g/l potassium hydrogen tartrate (KHT)
- 843.2 mg/l KCl
- adjust pH = 3.2 with tartartic acid (H2T).
- fill up the solution until 1 L.
Reactions:1. KHT <---> K
+ + HT
-2. H
2T <---> HT
- + H
+3. HT
- <---> T
2- + H
+Reaction 2 and 3 are dependant on the pH. At pH=3.2 the relation is H2T : HT- : T2- = 43.7 : 54.0 : 2.3
pKa ( H
2T <---> HT
- + H
+)= 2.98
pKa (HT
- <---> T
2- + H
+)= 4.34
Data:MW (KHT) = 188.18 g/mol
MW (H2T) = 150.09 g/mol
MW (HT-) = 149.0 g/mol
MW (KCl) = 74.55 g/mol
Solubility (KHT, at T=20*C) = 2.77 g/L
Calculation:mol (KHT) = 2.77 / 188.18 = 1.47E-02 mol
mol (KHT) = mol (K+) = mol (HT-) = 1.47E-02 mol
Question A: HT- will react further according to reaction 2 and 3. When can I niggled that?
Ksp = [K+] x [HT-]
Ksp = 1.47E-02 x 1.47E-02 = 2.16E-04
Real content KHT = 1.0/188.18 = 5.31E-03 mol
KHT will dissolve completely. mol (KHT) = mol (K+) = mol (HT-) = 5.31E-03 mol
At the solution with KHT is KCl added.
mol (KCl) = mol (K+) = mol (Cl- ) = 0.8432/74.55=1.13E-02 mol
Question B: What are the new equilibrium concentrations?
I 'll tried it but there is something not right.
Reaction 1. KHT <---> K
+ + HT
-Start mol (KHT) = 0; mol (K+)= 5.31E-03 + 1.13E-02 = 1.66E-02; mol; mol (HT-) = 5.31E-03
Change +x; -x; -x;
Equilibrium 0 + x; 1.66E-02 – x; 5.31E-03 - x;
Complete formula Ksp = [K+] x [HT-]
Ksp = 2.16E-04 = (1.66E-02 – x) x (5.31E-03 - x)
x = 2.67E-02
This is impossible because both concentration, [K+] and [HT-], would turn out negative.
I 'll hope someone could help me out of this....