Question

The thermodynamic solubility product of Ag2CrO4 is 1.1x10^-12. What is the [Ag+] in a saturated Ag2CrO4 solution that is also 30 mM NaNO3?

Answer #1

Given that

Ksp for Ag2CrO4 = 1.1*10^-12

i.e. [Ag+]^2 [CrO4-] = 1.1*10^-12

Let's say, [Ag+] = 2s and [CrO4-] = s M

Therefore, (2s)^2 * s, i.e. 4s^3 = 1.1*10^-12

i.e. s = {(1.1*10^-12)/4}^(1/3) = 0.65*10^-4 M

**[Ag+] (in solution of Ag2CrO4) = 2*0.65*10^-4 M, i.e.
1.3*10^-4 M**

Therefore, [Ag+] in saturated Ag2CrO4 solution having [NaNO3] as 30 mM, i.e. 30*10-^3 M is

**[Ag+] (in solution of Ag2CrO4 + NaNO3) = 1.3*10-^4 M
(since there is no common ion, [NaNO3] can't hamper the solubility
of Ag2CrO4)**

3a. Write the balanced reaction and solubility product
expression (KSP) for dissolving
silver chromate:
Ag2CrO4(s).
Include all charges, stoichiometric coefficients, and phase
subscripts. (4 pts)
c. Determine [Ag+1]
and [CrO4−2] fo
a saturated solution of
Ag2CrO4
if KSP = 1.1 ×
10−12. Also, determine the molar
solubility. (8 pts)
d. Use the KSP above
to determine
[CrO4−2] for a
solution that is saturated with
Ag2CrO4,
and also has a common ion effect where
[Ag+1] = 0.495 M. (4
pts)

Ksp for Ag2CrO4=5.4x10^-12. Calc molar solubility of Ag2CrO4 in
0.0050M K2CrO4

Calculate the molar solubility of Ag2CrO4 (Ksp = 1.1 × 10-12) at
25 °C in various aqueous solutions.
Calculate the solubility in 0.249 M
AgNO3
Calculate the solubility in 0.134 M
Na2CrO4

Calculate the molar solubility of Ag2CrO4
(Ksp = 1.1 × 10-12) at 25 °C in
various aqueous solutions.
A)Calculate the solubility in 0.200 M
AgNO3
B)Calculate the solubility in 0.200 M
Na2CrO4

The solubility product of silver chromate is 1.12*10^-12 at 25
degrees Celsius. What are the concentrations of Ag+ and CrO4^2- at
equilibrium? What is the solubility of silver chromate in g/L? What
is one way that you could increase the solubility of this slightly
soluble salt?

What is the pH of a saturated solution of Ni(OH)2
?
pH=
What is the solubility in grams of Ni(OH)2 /100 mL of
solution?
Solubility = g/100 mL

The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the
same initial set up of 10mL of 1M silver nitrate is combined with
25mL of 0.1M sodium chromate, what is the reaction quotient (Q) of
the silver chromate? (Is a precipitate going to form?)

What is the pH of a saturated solution of Ca(OH)2 if the
solubility of calcium hydroxide is 1.50 g/L?

find the concentration of Ag+ (silver ion) and CO3 2-
(carbonate ion) in a saturated silver carbonate solution with 0.01
M of KNO3 (potassium nitrate). The equilibrium constant for silver
carbonate is 8.1 X 10 -12 .

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...

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