I thought the high pH was strange too.
Alright, attempt 2.
Finding the pH of glycine in 20mL of water, by using its pka of 2.3 to find its Ka, and from its Ka finding its H+ concentration using an Ice Table
HA<-> H+ A-
.004 0 0
-x +x +x
Find x to be 0.0026. and find the pH to be 2.58.
Then, pH of 1M sulfuric acid is -log (1) = 0.
From this, we can find hte [H+] of both, and because we know the volume added, we can determine the amount moles of H+. Add the moles together, divide by sumated volume, and find new pH of acid.
10^-2.58 = .0026 M H+ from glycine x.02 L of water = .000052 moles of H
1M of H from sulfuric acid x .001 L = .001 moles of H
.001moles + .00052 = .001052 moles of H /0.021 L = .0500M H+
pH = - log (.0500) = 1.30
While I could believe this, you get a slightly different answer when you use the pKa2 for glycine--the H concentration is much smaller--but due to the large amount of moles from sulfuric acid, it doesn't make too much difference in the end pH roughly 1.32.
Thanks for the help