Question
I got 20 and its wrong. and they gave me that hint,
For an aqueous solution of HF, determine the van't Hoff factor assuming... 0% ionization. 100% ionization. i= Number i = Number 2 solution is made by dissolving 0.0150 mol of HF in enough water to make 1.00 L of solution. At 22 degree , the osmotic pressure of the solution is 0.443 atm. What is the percent ionization of this acid? Incorrect. Consider the value of i. For example, i= 1.5 is halfway between 1 and 2, 1.25 would be 25% of the way between 1 and 2, and 1.75 would be 75% of the way between 1 and 2. Thus, we can generalize that for HF, the percent ionization is always (i -1)x 100%. First, find the apparent particle concentration using the osmotic pressure formula. Then calculate i by taking the ratio of the particle concentration to the HF concentration.
Explanation / Answer
P = iCRT i = 0.443 / (0.15* 0.0821*295) = 1.22 HF ------>> H+ + F- 1-x x x i = moles after/ moles before 1.22 = 1+x /1 x = .22 %age = 22
