Question

What concentrations of SO3^2- is in equilibrium with Ag2SO3 and 8.7x10^-3 M of Ag+?

Answer #1

^{2}^{-}

The Ksp of Ag2SO3 is 1.50×10^–14

Ksp = [Ag+]^2 * [SO3 ^{2-} ]

if x moles of Ag2SO3(s) dissolve we have 2x moles of Ag+ and x
moles of SO3 2-

in .8.7 x 10 ^-3 M Ag + we have [Ag+ ] = 2x + 8.7 x 10 ^-3 moles /
liter

Ksp = (2x + 8.7 x 10 ^-3)^2 * x = 1.50×10^–14

we can solve the quadratic equation or assume (x <<< 8.7x
10 ^-3, use aprox)

we then have 1.50 x 10 ^-14 = x * (8.70 x 10 ^-3)^2

x = 1.50 x 10 ^-14 / (8.7 x 10 ^-3)^2

[SO3^{2-}]= **1.98 x 10 ^-10 moles per
liter**

What concentration of SO32– is in equilibrium with Ag2SO3(s) and
8.60 × 10-3 M Ag ? The Ksp of Ag2SO3 is 1.50×10–14.
[SO3^2-]=?
please show all work

What concentration of SO32– is in equilibrium with Ag2SO3(s) and
5.50 × 10-3 M Ag ? The Ksp of Ag2SO3 can be found here.

What concentration of SO32– is in equilibrium with Ag2SO3(s) and
5.20 × 10-3 M Ag ? The Ksp of Ag2SO3 can be found here.

Determine the concentration of SO3 in the following reaction
when it reaches equilibrium if the initial concentrations are 0.39
M So2, 0.14 M NO2, 0.11 M SO3 and 0.14 M NO.
SO2+NO2<=>SO3+NO
Kc=0.33
Please show all steps. Thank you!!

Calculate The concentration of Ag+ present
in solution at equilibrium when equilibrium concentration of
[NH3] =0.20 M. The initial
Ag(NH3)2+ concentration is 0.010M.
The Kf of Ag(NH3)2+ is
1.7 x 107.
Ag+(aq)+ 2NH3(aq)---
>Ag(NH3)2+(aq)

What is the approximate concentration of free
Ag+ ion at equilibrium when
1.42×10-2 mol silver
nitrate is added to 1.00 L of solution
that is 1.070 M in
S2O32-. For
[Ag(S2O3)2]3-,
Kf = 2.9×1013.
[Ag+] = ____M

For the following exothermic reaction at equilibrium: 2 SO2 + O2
------> 2 SO3 What is the effect of adding SO2?

a. The Ksp for Ag2SO3 = 1.50 X
10-14. What is the molar solubility of
Ag2SO3 in a 5 M solution of lithium
sulfite?
b.The Ksp for
Mg3(PO4)2 = 1.04 X
10-24. What is the molar solubility of
Mg3(PO4)2 in a 1.40 M solution of
sodium phosphate?
c.If the Ksp for Y(OH)3 = 1.00 X 10-22,
what is the molar solubility of Y(OH)3 in a buffer
solution composed of 1.60M trimethylamine (=
(CH3)3N) (Kb = 6.5 X
10-5) and 1.40M...

In the reaction below the equilibrium constant was found to be
2.80 x102. What is the concentration of SO3 at equilibrium if the
equilibrium concentrations of SO2 and O2 are 0.124 M and 0.031M
respectively? O2(g)+SO2(g)=SO3(g)

An equilibrium mixture of the following reaction was found to
have [SO3] = 0.401 M and [O2] = 0.205 M at 600 ∘C .
What is the concentration of SO2 ?
2SO2(g)+O2(g)⇌2SO3(g)
Keq = 4.84 at 600 ∘C

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