How can I calculate dissociation of a weak acid?
To do this you'll need to use the Ka value of the acid and determine the equilibrium expression of the dissociation of that acid. Using the quadratic equation allows you to solve for the hydrogen ion concentration if you are given the initial concentration of the acid and the Ka value.
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To calculate the dissociation of a weak acid, you can use the equilibrium constant expression for acid dissociation, known as the acid dissociation constant ((K_a)). For a weak acid (HA) dissociating into (H^+) and (A^-), the equilibrium expression is:
[K_a = \frac{[H^+][A^-]}{[HA]}]
Where:
- (K_a) is the acid dissociation constant.
- ([H^+]) is the concentration of hydronium ions.
- ([A^-]) is the concentration of the conjugate base.
- ([HA]) is the initial concentration of the weak acid.
Given the initial concentration of the weak acid, and assuming the initial concentrations of hydronium ions and the conjugate base are both zero, you can use the equilibrium constant expression to calculate the concentrations of (H^+) and (A^-), and hence determine the extent of dissociation.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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