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Equilibrium shifts towards the higher Ka

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βˆ™ 11y ago
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βˆ™ 8mo ago

Ka is the equilibrium constant for the dissociation of a weak acid. A higher Ka value indicates a stronger acid and therefore more products are formed during dissociation, pushing the equilibrium position to the right. Conversely, a lower Ka value indicates a weaker acid and less products are formed during dissociation, shifting the equilibrium position to the left.

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Q: How does Ka affect equilibrium position?
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Enzymes do not affect the equilibrium constant of a reaction. They only speed up the rate at which the reaction reaches equilibrium, but do not change the position of the equilibrium itself.


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How are the equilibrium constants Ka and Kb related in a chemical reaction?

In a chemical reaction, the equilibrium constants Ka and Kb are related by the equation Ka x Kb Kw, where Kw is the equilibrium constant for water. This relationship shows that the product of the acid dissociation constant (Ka) and the base dissociation constant (Kb) is equal to the equilibrium constant for water.


What is the relationship between the equilibrium constants Kb and Ka in a chemical reaction?

The equilibrium constants Kb and Ka in a chemical reaction are related by the equation Ka Kb Kw, where Kw is the equilibrium constant for water. This relationship shows that the product of the acid dissociation constant (Ka) and the base dissociation constant (Kb) is equal to the equilibrium constant for water.


What is the relationship between the equilibrium constants Ka and Kb in a chemical reaction?

The equilibrium constants Ka and Kb are related by the equation Ka x Kb Kw, where Kw is the equilibrium constant for water. This relationship shows that as one equilibrium constant increases, the other decreases in order to maintain a constant value for Kw.