# Determining the Equivalent Mass and Dissociation Constant of an Unknown Weak Acid by Titrimetry

Topics: PH, Acid, Acid dissociation constant Pages: 6 (1365 words) Published: November 7, 2012
DETERMINING THE EQUIVALENT MASS AND DISSOCIATION CONSTANT OF AN UNKNOWN WEAK ACID BY TITRIMETRY

INTRODUCTION

Acids are substances that donate hydrogen ions and bases are substances that accept hydrogen ions. Acids and bases react with each other by transferring hydrogen ions. One way to distinguish an acid is by its equivalent mass, which is the number of grams of the acid needed to transfer one mole of hydrogen ion to a base. For a monoprotic acid, which only transfers one hydrogen ion, its equivalent mass equals its molar mass. For a diprotic acid, which transfers two hydrogen ions, its equivalent mass equals half its molar mass. The equivalent mass of a base is simply the number of grams required to accept one mole of hydrogen ion. The equivalent mass of an acid or base is also equal to the mass of the acid or base titrated divided by the number of equivalents of the acid or base.

Acid strength is measured by how much it dissociates. This is determined by the amount of hydronium ion formed in water. Most often, it is expressed by pH, which equals the –log[H3O+]. The equilibrium constant for an acid is represented by Ka = [H3O+] [A-] / [HA], where HA is the acid and A- is the dissociated acid. When comparing Ka’s, most commonly pKa is used, which is equal to –log Ka.

In this experiment, the pKa of an unknown acid is determined by titrating it with NaOH and graphing its pH levels versus volume of NaOH titrated. The inflection point found by graphing is the equivalence point, and at half that volume is the half-equivalence point. At half equivalence, the [A-] = [HA], so they cancel out in the equation Ka = [H3O+] [A-] / [HA], leaving Ka = [H3O+]. With pH being known, Ka is found by [H3O+] equaling 10-pH, and pKa = pH.

EXPERIMENTAL

First, about 2 g of an unknown weak acid was obtained. Then about 0.10 to 0.12 g of the acid was weighed out on an analytical scale. This mass was recorded to 4 decimal places. The acid was then transferred to a clean 125 mL Erlenmeyer flask. Distilled water was added to dissolve the acid, and then 3 drops of phenolphthalein indicator was added to the solution. Next, a buret was filled with NaOH solution and its initial reading was recorded to 2 decimal places. The acid solution was titrated with the NaOH solution until the acid solution turned and stayed pink. This final reading was recorded to 2 decimal places and the volume of NaOH used was calculated.

Another sample of unknown acid was weighed out using an analytical scale requiring about 25 mL of standardized NaOH solution. This mass was recorded to 4 decimal places. The acid was transferred into a clean 150 mL beaker, and was again dissolved using distilled water. A pH meter and electrode was then obtained. The electrode was rinsed with distilled water and put into the acid solution. Standardized NaOH solution was again used to titrate the acid. The initial buret reading was recorded to 2 decimal places and NaOH was added 0.5 mL at a time. After every portion added, the buret reading and pH meter reading were recorded to 2 decimal places. This was done until the pH spiked and stopped increasing significantly.

RESULTS

Identification code of weak unknown acidT
Mass of unknown acid, g0.1167
Volume of NaOH solution required, mL13.62
Concentration of NaOH solution used, M1.00 x 10-1
Mass of unknown acid requiring 25 mL of NaOH solution for titration, g0.2142 Mass of unknown acid used, g0.2152
0.502.95
0.993.07
1.503.22
2.003.38
2.493.50
3.003.60
3.493.70
4.003.78
4.503.86
4.993.92
5.493.99
6.014.04
6.504.09
6.994.14
7.504.19
7.994.23
8.504.28
8.984.32
9.504.36
10.004.40
10.484.43
11.004.47
11.484.51
12.004.55
12.504.59
13.004.62
13.494.66
13.984.69
14.494.73
15.004.77
15.504.80
15.994.84
16.504.88
17.004.92
17.494.96
17.995.00
18.505.05
19.005.09...