1) before addition of any KOH :
H3PO3 ---------------------> H+ + H2PO3-
2.1 0 0
2.1- x x x
Ka1 = [H+][H2PO3-] / [H3PO3]
0.05 = x^2 / 2.1 - x
x^2 + 0.05 x - 0.105 = 0
x = 0.30
[H+] = 0.30 M
pH = -log [H+] = -log [0.30]
= 0.523
pH = 0.523
b) after addition of 25.0 mL KOH
it is first equivaelce point
pH = pKa1 = 1.30
pH = 1.30
c) addition of 50.0 mL KOH
it is first equivalence point
pH = 1/2 (pKa1 + pKa2)
pH =1/2 (1.30 + 6.70)
pH = 4.0
d) 75.0 mL KOH
it is seond half equivalece point
pH = pKa2
pH = 6.70
e) 100.0 mL KOH
it is second equivalece point
HPO3^-2 millimoles = 100 x 2.1 = 210
HPO3^-2 molarity = 210 / (50 +100) = 1.4M
HPO3^-2 + H2O ------------------> H2PO4- + OH-
1.4 -x x x
Kb2 = x^2 / 1.4-x
5.01 x 10^-8 = x^2 / 1.4-x
x^2 + 5.01 x 10^-8 - 7.017 x 10^-8 = 0
x = 2.65 x 10^-4
[OH-] = 2.65 x 10^-4 M
pOH = -log[OH-] = -log (2.65 x 10^-4 )
pOH = 3.58
pH + pOH = 14
pH = 10.42
Phosphorous acid, H, PO, (aq), is a diprotic oxyacid that is an important compound in industry...
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