A.CALCULATE THE CRYOSCOPIC CONSTANT OF H2O. USE IT TO ANSWER THE FOLLOWING: a WEAK ACID HX is dissolved in water. A 0.250 molal solution has a freezing point of 0.5 C. calculate the value of ka for the acid, where Ka is the equilibrium constant for

Question

A.CALCULATE THE CRYOSCOPIC CONSTANT OF H2O. USE IT TO ANSWER THE FOLLOWING: a WEAK ACID HX is dissolved in water. A 0.250 molal solution has a freezing point of 0.5 C. calculate the value of ka for the acid, where Ka is the equilibrium constant for HX<--=-->H+ + X- Ka = [X-][H+]/[HX] I assume you have the cryoscopic constant for water. I will assume, further, that it is 1.86 degrees C/m. (delta T)=i*k_f*m delta T is 0.5^o C solve for i k_f=1.86^{oC/m.
m is molality = 0.250 mol/kg

i*m(ideal)=m(effective)
where m(ideal) is 0.250.

HX <===>H^+ + X^-
When HX ionizes,
(H^+) = Y
(X^-) = Y
(HX) = 0.250 - Y
The sum of HX + H^+ + X^- =
0.250-Y+Y+Y=m(effective).
m(effective is from above).
Solve for Y and then for Ka.
Post your work if you get stuck.
Check my thinking. Check my work carefully.

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