Which of the following could be the equilibrium constant for the dissociation of

Question

Which of the following could be the equilibrium constant for the dissociation of HNO2 in water?
circle one: K= 1.5 K = 3.8 × 106 K = 4.6 × 10-4
Explain why you chose that equilibrium constant Which of the following could be the equilibrium constant for the dissociation of HNO2 in water?
circle one: K= 1.5 K = 3.8 × 106 K = 4.6 × 10-4
Explain why you chose that equilibrium constant Which of the following could be the equilibrium constant for the dissociation of HNO2 in water?
circle one: K= 1.5 K = 3.8 × 106 K = 4.6 × 10-4
Explain why you chose that equilibrium constant

Explanation / Answer

HNO2 is a weak acid . So it is partialy ionisable in water. So it has low disociation constant.

HNO2 --------------> H+ + No2^-

Ka = [H+][No2^-]/HNO2]

Ka is acid disociation constant or equilibrium constant

HNo2 has K = 4.6 × 10-4

K= 1.5, K = 3.8 × 106 two value are high . so they are not disociation constants of weak HNO2

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