A 0.21-mol sample of a diprotic acid, H 2A, is dissolved in 250 mL of water. The K a1 of this acid is 1.0 × 10 –5 and K a2 is 1.0 × 10 –10. Calculate the concentration of A 2– in this solution. a.
0.84 M
b.
1.0 × 10–5 M
c.
1.4 × 10–3 M
d.
1.0 × 10–10 M
e.
2.9 × 10–3 M

it should be all of them because it asks if you included all of those in your answer

explanation:

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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