A handbook lists the solubility of CaHPO 4 as 0.32g CaHPO 4 ⋅ 2H 2 O/L and lists K 10 1 × 10 − 7 CaHPO 4 ( s ) ⇌ Ca 2+ ( aq ) + HPO 4 2 − ( aq ) Are these date consistent? (That is, are the molar solubilities the same when derived in two different ways?) If there is a discrepancy, How do you account for it?
A handbook lists the solubility of CaHPO 4 as 0.32g CaHPO 4 ⋅ 2H 2 O/L and lists K 10 1 × 10 − 7 CaHPO 4 ( s ) ⇌ Ca 2+ ( aq ) + HPO 4 2 − ( aq ) Are these date consistent? (That is, are the molar solubilities the same when derived in two different ways?) If there is a discrepancy, How do you account for it?
Solution Summary: The author analyzes the solubility of CaHPO_Text4 in aqueous solution, and determines whether the data is consistent or not.
= 1.6 x 10-10
Given the reactions below, calculate the molar solubility of AgCl (s) in 0.566 M NH3 (aq) at 25 degrees C.
AgCl (s) →> Ag+ (aq) + Cl¯ (aq) K
sp
Ag+ (aq) + 2 NH3 (aq) →>
Ag (NH3)
+
(aq) K = 1.7 x 107
f
2
Report your answer rounded to two significant figures and do NOT include units. Use "e" for scientific notation. For example, 1.0 x
10-14 is 1.0e-14.
The solubility product constant for ruthenium perchlorate (RuClO4) is 3.0 x 10-3. What is the molar solubility (in mol/L)?
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is:
Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l)
A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant.
Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction:
B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq)
What is Ksp expression for the dissolution?
What is the tetraborate ions concentration in the filtrate?
What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
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