If 0. 22 m aqueous solution of the weak acid hA at 25. 0 °C has a ph of 4. 15, the value of ka for HA is 2.27 × 10^(-8).
<h3>What is an aqueous solution?</h3>
The aqueous solution is simply defined as something which has been dissolved in water. The aqueous symbol is denoted as (aq).
Given,
pH = 4.15
Concentration of HA = 0.22 M
Firstly, we will calculate the concentration of H+ ion
pH=-log [H+]
4.15 =-log [H+]
= 7.08x 10^{-5}
Secondly we will calculate the value of Ka
for HA is
The equilibrium reaction will be:
HA----- (H+) + (A-)
Given,
Concentration of H+
= Concentration of A-
= 7.08 x 10^{-5} M
The expression of Ka for HA will be,
Ka = [A-] [H+]/[ HA]
= 2.27 × 10^(-8)
Thus we concluded that the value of ka for HA for weak acid HA is 2.27 × 10^(-8).
learn more about aqueous solution or Ka:
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