Na2CO3 here is Strong electrolyte
It will dissociate completely to give [CO32-] = 0.0044 M
At equilibrium:
Ag2CO3 <----> 2 Ag+ + CO32-
2s 4.4*10^-3 + s
Ksp = [Ag+]^2[CO32-]
8.6*10^-12=(2s)^2*(4.4*10^-3+ s)
Since Ksp is small, s can be ignored as compared to 4.4*10^-3
Above expression thus becomes:
8.6*10^-12=(2s)^2*(4.4*10^-3)
8.6*10^-12= 4(s)^2 * 4.4*10^-3
s = 2.211*10^-5 M
So,
[Ag+] = 2s
= 2*2.211*10^-5 M
= 4.422*10^-5 M
Answer: e
QUESTION 6 What is the concentration of silver ion in a saturated solution of silver carbonate...
What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0060 M Na2CO3? For Ag2CO3, Ksp = 8.6 × 10–12. a)3.8 × 10–5 M b)2.0 × 10–9 M c)8.0 × 10–9 M d)6.0 × 10–4 M e)8.0 × 10–4 M
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5. What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0030 M Na2CO3? For Ag2CO3, Ksp = 8.6 x 10-12. A) 6.0 x 10-4 M B) 2.0 x 10-'M C) 8.0 x 10-'M D) 5.4 x 10-5M E) 8.0 x 10-4M 6. Balance the following oxidation-reduction occurring in acidic solution. MnO4 (aq) + Co2+(aq) →Mn²+ (aq) + Co3+ (aq) A) B) C) D) E) MnO4 (aq) + 8 H+ (aq) + Co2+(aq) Mn²+ (aq)...
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