Suggested Data Table (Partially completed) 1 2 3 4 5 6 7 8 9 10 11...

Question

Question

THE DETERMINATION OF THE IONIZATION CONSTANT OF A WEAK ACID Unknown number: Complete the data table with the measured and cal

Suggested Data Table

(Partially completed)

	1	2	3	4	5	6	7	8	9	10	11
	Vol HX Init., mL	Vol OH^– added for this increment, mL	Total Vol OH^–, mL	Total Vol Soln, mL	[HX]_i	[X^–]_eq	[HX]_eq	[X^–]/[HX]	log $begin mathsize 12px style fraction numerator left square bracket straight X to the power of – right square bracket over denominator left square bracket HX right square bracket end fraction end style$	Meas'd pH	Calc'd pK_a
0	50.0	0.0	0.0	50.0	---	---	---	---	---	---	---
1	50.0	10.0	10.0	60.0
2	50.0	5.0	15.0	65.0
3	50.0	5.0	20.0	70.0
4	50.0	10.0
5	50.0
6	50.0

please help

Answer 1

Answer #1

Solution 1.

pH = 2.15

i.e. -Log[H⁺] = 2.15, i.e. [H⁺] = 10^-2.15 = 7.08*10^-3 M

i.e. [X^-]_eq = 7.08*10^-3 M

Now, [HX]_eq = 0.1 M - 7.08*10^-3 M = 0.093 M

Now, Ka = [H⁺][X^-]_eq/[HX]_eq = (7.08*10^-3)*(7.08*10^-3)/0.093 = 5.394*10^-4

Now, pKa = -Log(Ka) = -Log(5.394*10^-4) = 3.268

Log[X^-_eq/HX_eq] = Log(7.08*10^-3/0.093) = -1.118

Answer 2

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