For the reactionCaCO3 s+ H+ aq Ca2+ aq+ HCO3-aq Find the K constant to 2 d.p given the followingCaCO3 s ⇌ Ca2+ aq+ CO32-aq K1 = 2.48HCO3-aq ⇌ H+ aq + CO32-aq K2 = 8.6
Question
For the reactionCaCO3 s+ H+ aq Ca2+ aq+ HCO3-aq Find the K constant to 2 d.p given the followingCaCO3 s ⇌ Ca2+ aq+ CO32-aq K1 = 2.48HCO3-aq ⇌ H+ aq + CO32-aq K2 = 8.6
Solution
The reaction given can be broken down into two steps:
- CaCO3(s) ⇌ Ca2+(aq) + CO32-(aq) with K1 = 2.48
- HCO3-(aq) ⇌ H+(aq) + CO32-(aq) with K2 = 8.6
The overall reaction is the sum of these two reactions:
CaCO3(s) + H+(aq) ⇌ Ca2+(aq) + HCO3-(aq)
According to the law of mass action, the equilibrium constant for the overall reaction (K) is the product of the equilibrium constants of the individual reactions. Therefore, K = K1 * K2.
K = 2.48 * 8.6 = 21.33
So, the equilibrium constant for the overall reaction to 2 decimal places is 21.33.
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