Answer:
X = 2
Explanation:
As you know, the rate of a first-order reaction depends linearly on the concentration of a single reactant. The rate of a first-order reaction that takes the form
Answer:
Le Chatelier's principle predicts that equilibrium will shift to decrease the concentration of reactants. Increasing the rate of the forward reaction will mean a decrease in reactants. ... When the concentration of reactants is increased, the equilibrium shifts to the right and there will be more product than before.
Explanation:
We have to calculate
value.
It is known that at the equivalence point concentration of acid is equal to the concentration of anion formed.
Hence, [HA] = ![[A^{-}]](https://tex.z-dn.net/?f=%5BA%5E%7B-%7D%5D)
Now, relation between
and pH is as follows.
pH = ![pK_{a} + log \frac{[A^{-}]}{[HA]}](https://tex.z-dn.net/?f=pK_%7Ba%7D%20%2B%20log%20%5Cfrac%7B%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D)
Putting the values into the above formula as follows.
pH = ![pK_{a} + log \frac{[A^{-}]}{[HA]}](https://tex.z-dn.net/?f=pK_%7Ba%7D%20%2B%20log%20%5Cfrac%7B%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D)
4.23 =
(as [HA] =
)
= 4.23 (as log (1) = 0)
or,
= 4
Thus, we can conclude that
of given weak acid is 4.