Which of the following would decrease the Ksp for AgCl? Which of the following would decrease solubility of AgCl?
A. Increasing the pH of the solution
B. Adding a solution of AgNO3
C. Adding a solution of KCl
D. Adding a solution of KI
E. None of the above
Select one:
a. Only E; Only B and C
b. Only B and C; Only A
c. Only A; Only B and C
d. Only B and C; E
e. Only A; Only B, C and D
Hi there,
Correct option: a. Only E; Only B and C
Q: Which of the following would decrease the Ksp for AgCl?
Answer: E. None of the above, the Ksp of a compound is constant at constant temperature.
Q: Which of the following would decrease solubility of AgCl?
AgCl <==> Ag+ + Cl-
Adding AgNO3 increases the Ag+ concentration and also adding NaCl increases the Cl- concentration will shift equilibrium towards left hence solubility decreases.
Answer:
B. Adding a solution of AgNO3
C. Adding a solution of KC
Hope this helped you!
Thank You So Much!
Please Rate this answer as you wish.("Thumbs Up")
Which of the following would decrease the Ksp for AgCl? Which of the following would decrease...
5. Which of the following would decrease the K for PbCl2? 2. Lower the pH of the solution b. Add a solution of Pb(NO3)2 c. Add a solution of KCI d. Both band e. None of the above the Ky of a compound is constant at constant tempera mperature, 6. In which of the following aqueous solutions would you expect AgBr to have the HIGHES solubility? a. 0.10 M LIBE b. 0.10 M AgNO3 c. 0.20 M NaBr d. 0.15...
Select all that apply. The molar solubility of AgCl in 6.5 × 10−3 M AgNO3 is 2.5 × 10−8 M. In deriving Ksp from these data, which of the following assumptions is (are) reasonable? Ksp is the same as solubility. The molar solubility of AgCl is the same in 6.5 × 10−8 M AgNO3 as in pure water. Solubility of AgCl is independent of the concentration of AgNO3. [Ag+] does not change significantly upon addition of AgCl to 6.5 ×...
If x = molar solubility, Ksp = solubility product, which of the following compounds would have the relationship: 27x4 = Ksp? a) Bi2S3 b) Ag2CO3 c) AgCl d) PbI2 e) Ag3PO4
. Which of the following would be more soluble if the pH of the solution was decreased? A. AgNO3 B. AgCl C. PbBr2 D. MgCO3 E. pH would have no effect on all of the above. Please explain how you answer this question.
very urgent !
(4 points) The KSP for AgCl is 1.8 x 10-10 in which of the following would you expect AgCl to have the lowest solubility? (Circle one). д) 0,025 M Baci, b) 0.040 M AgNo, c) 0.040 MKCI d10050 MKCN e) 0.075 M HCIf pure water
What is the molar solubility of AgCl in 0.025 M CaCl2? For AgCl, Ksp = 1.6 x 10-10. You can assume that molar solubility, s, is very small. Select one: a. 1.6 x 10-11 M b. 3.2 x 10-9 M c. 8.5 x 10-12 M d. 2.5 x 10-10 M e. 6.2 x 10-13 M
Complete Table 1:
Ksp data
Salt
[cation] (M)
[anion] (M)
molar solubility (M)
Ksp
AgCl
SrSO4
Ag2CO3
Sr(IO3)2
1) Rank the salts in order of increasing molar solubility.
2) Rank the salts in order of increasing Ksp
(remember 10–10 < 10–5)
3) If these rankings are not in the same order, why might
Ksp not always scale directly with molar solubility?
Design experiments in the virtual lab to answer the follow questions, 1). Use the virtual lab to determine the...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except that they have the following pH values: Hint: Common ion effect. Which two ions dictate acidity and basicity? a. 3 b. 7 c. 9 d. 11 2. Potassium perchlorate has a solubility product constant of 10-2. Which is true about the following solution of KClO4: [K+] = 0.01 M, [ClO4 −] = 0.01 M a. Ksp < Q and no precipitation occurs b....
A. Choose all the species that could increase the molar solubility of AgCl. NaCl, HCl, NaOH, NH3 B. Choose all the species that could increase the molar solubility of Mg(OH)2. HCl, MgCl2, NaOH, KBr C. Which of the following compounds would be more soluble in an acidic solution than in water? Select all that apply. CuS, AgCl, PbSO4, KI
Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 1.94 x 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 6.24 x 10-6 M. (a) What is the concentration of chloride ions, [CI – ], in the resulting solution? XM (b) What is the molar solubility of silver chloride, AgCl, in 1.94 x 10-5 M NaCl? 4.9 6.24e-6...