if the degree of dissociation of one molar monoprotic acid is 10 percent. calculate its Ka value?
1 M x 0.l0 = .1
.......HA ==> H^+ + A^-
I......1......0.....0
C.....0.1.....0.1...0.1
E.....0.9.....0.1...0.1
Substitute the E line into the Ka expresson and solve for K. Post your work if you get stuck.
Answer
To calculate the Ka (acid dissociation constant) value of a monoprotic acid from its degree of dissociation, we need to use the equation for degree of dissociation and the expression for Ka.
The degree of dissociation (α) is defined as the fraction of the acid that dissociates in a solution. In this case, α = 0.10 or 10%.
The equation for degree of dissociation is given by:
α = √(Ka * C)
Here, Ka is the acid dissociation constant and C is the initial concentration of the acid.
To find the Ka value, we need to rearrange the equation and solve for Ka:
Ka = (α^2) / C
Given that α = 0.10, we can substitute this value into the equation. However, we still need the initial concentration of the acid (C) to proceed.
If you provide the initial concentration of the monoprotic acid, I can help you calculate its Ka value.