Question

What is the solubility of AgBr in 0.05 M NaCN?

Ksp (AgBr)= 5.0x 10^-13 and Kf (Ag(CN)2-)= 1.0 x 10^21

Answer #1

What mass of AgBr will dissolve in 120 mL of 0.840 M NaCN?
Ag+ + 2CN- ↔ Ag(CN)2- B =
1.3*1021

The solubility of AgBr (Ksp =5.0 x 10-13 ) in 0.230
Molar CaBR2 is__________ (a number) Please show all
work

AgCl is very insoluble in water (Ksp= 1.6 x 10−10) but when
sodium cyanide (NaCN) is added, it dissolves readily. Propose a
reasoning for this. Hint: Use the following equation to find your
answer.Ag+(aq)+ 2 CN–(aq)↔[Ag(CN)2]–(aq)Keq = 5.6 x 1018

1. The Ksp for AgCl is 1.6 x 10-10
(a) What is the molar solubility of AgCl?
(b) What is the solubility in g/L solution?
2. The Ksp of Ag2CO3 is 8.1 x 10-12
(a) What is the molar solubility of Ag2CO3
(b) What is the molar solubility of [Ag+]?
(c) what is the solubility of Ag2CO3?

i just need work,
1. Calculate the Ksp for silver sulfite if the solubility in
pure water is (2.2x10^-3) g/L.
Answer :6.1 * 10^-16
2. What is the molar solubility of Mg(OH)2 in a basic solution
with a pH of (1.32x10^1)? Ksp for Mg(OH)2 is (1.8x10^-12)
Answer: 7.2x10^-11
3.
A (1.6x10^2) mL sample of a solution that is (3.000x10^-3) M in
AgNO3 is mixed with a (2.000x10^2) mL sample of a
solution that is (2.00x10^-1) M in NaCN. After the...

Calculate the solubility (in g·L–1) of CuBr(s) (Ksp = 6.3× 10–9)
in 0.90 M NH3(aq). Kf=6.3x10^10

What is the molar solubility of ArBr in 0.001 M NaBr? Ksp for
Arbr is 7.7*10^-13
Please explain :)

Question 1 :
The solubility product, Ksp, of
Cd3(PO4)2 is 2.5 x
10-33. What is the solubility (in g/L) of
Cd3(PO4)2 in pure water?
Question 2 :
The solubility product of Cu(OH)2 is 4.8 x
10-20. Calculate the value of pCu2+, or
-log[Cu2+], in an aqueous solution of NaOH which has a
pH of 12.89 and is saturated in Cu(OH)2.
Question 3 :
The equilibrium constant for the formation of
Cu(CN)42- is 2.0 x 1030. Calculate
the value of pCu2+,...

Which of the following has the greatest solubility in water?
(A) ZnCr2O4 ( Ksp = 2.7 x
10-8)
(B) BaCrO4 ( Ksp = 2.3 x 10-10
)
(C) CaF2 ( Ksp = 3.9 x
10-11)
(D) AgBr ( Ksp = 5.0 x 10-13 )

What is the molar solubility of BaF2 in .033M KF (aq)? The BaF2
Ksp is 1.8*10^-7.
I got 5.5*10^-6 which is incorrect. Please explain!

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