In simple words we can say that,
Equilibrium is a dynamic process. Removing some solid would cause the equilibrium of the solution to shift to the left and produce more solid from the dissolved solution to reestablish equilibrium.
Lets look at a simple example with say, silver chloride
The equilibrium we are talking about is AgCl(s) <---> Ag+(aq) + Cl-(aq)
At equilibria these will be at a certain balance, controlled by the equilibrium constant Kc
But what would happen if you removed the solid AgCl? The condition for Kc would not longer be true and silver ions and chloride ions would have to react to form AgCl solid. This is why solid must be present.
The other reason is that temperatures rarely remain constant, and the presence of solid also allows the equilibria to adjust to the small temperatures changes. {Kc varies with temperature]
Why must some solid remain in contact with a solution of a sparingly soluble salt in...
Dat Determination of the Solubility-Produet Constant for Sparingly Seluble Selt Distinguish between the equilibrium constant expression and K for the disolution of a on and K, for the dissolution of a sparingly soluble salt List as many experimental techniques as you can that may be used to determine K, for a sparingly soluble salt. 7. 8. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? 9. In general, when...
Answer QUESTION 5 Describe what happens at the molecular level once equilibrium is reached--that is, once the solution is saturated with Cu(IO_3)_2. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? Describe how you are going to calculate the [Cu^2+] for the saturated solution of copper iodate once you know the absorbance value of the copper ion. How will you use this concentration to find the K_sp value for...
AgBr is sparingly soluble in water and has a Ksp of 5.0 x 10-13. What will be the effect of adding solid NaBr to an aqueous solution of in equilibrium with solid AgBr? Some additional AgBr will precipitate. The Ksp of AgBr will increase. The Agt concentration will remain constant. Additional AgBr will dissolve.
A student sets out to determine the Ksp of the sparingly soluble salt, M2X3. This salt dissociates into the ions M3+ (aq) and X2- (aq). A sample of a 0.00300M M(NO3)3 (aq) solution is titrated by a 0.00200M solution of K2X (aq). A precipitate starts to form when 4.50mL of K2X (aq) have been added. Based on this data, determine the Ksp of M2X3. As usual, assume that aqueous solution volumes are additive.
PbI2 is a sparingly soluble salt with Ksp= 1.39x10-8 What is the molar solubility of PbI2?
What is likely to happen when PbI2 , a sparingly soluble salt, is placed in a 0.050 M KNO3 solution: a. The amount of Pb2+ ions in solution will increase b. K+ and NO3- ions will co-precipitate with PbI2 c. More PbI2 will be formed d. The amount of I- in solution will be unchanged
Question 6 (Extra Credit Challenge): When the sparingly soluble salt lead fluoride, PbF2, is added to an acidic solution with [H+] = 1.6 x 10–4 M, the resulting concentration of [Pb2+] after the salt dissolves is determined to be 7.75 x 10–5 M. (a) Determine the equilibrium constant for the dissolving of PbF2 in an acidic solution of H3O+ and (b) given Ka = 6.8 x 10–4, use the value determined in part a to calculate the Ksp for PbF2...
6. Enough of a sparingly soluble salt AB(s) dissolved in a certain amount of water to bring it into equilibrium with the ions A" (aq) and B (aq). If the equilibrium concentration of A*? is 4.9 x 10 mol kg"', and the Debye Hückel Limiting Law (DHLL) is obeyed at this concentration, K sp for the salt is: A) 2.11e-9 B) 4.90e-9 C) 4.86e-10 D) 8.46e-9 E) 3.91e-10
Question 4: Given the Ksp = 2.0 x 10-29 for the sparingly soluble salt, calcium phosphate (Ca3(PO4)2), determine the molar solubility of the salt in a solution that is 0.20 Min calcium perchlorate, Ca(CIO4)2.
AgBr is a sparingly soluble salt with a molar solublity of about 7x107 Min pure water. How would you expect the solubility to change if AgBr is dissolved into a solution of 1.0M AgNO3? O Solubility will be the same Solubility will be decreased O Solubility will be increased