A 150 mL sample of a 0.300 M solution of K2SO3 is titrated with a 1.00 M HCl solution. Ka1=1.39E10^-2, Ka2=6.73E10^-8 Wh...

Question

Question

A 150 mL sample of a 0.300 M solution of K2SO3 is titrated with a 1.00 M HCl solution. Ka1=1.39E10^-2, Ka2=6.73E10^-8

What is the initial pH (before titration) and the pH after 50.0 mL of the 1.00 M HCl has been added?

Answer 1

Answer #1

K2s03 0.3M, IS0 me 129,6-73 x lo pka,= 1.8S 69 pka, =7.1719 = (o.3 xSommole K2S03 K250 4S mmule jnih al pH dey to 1) + 7.1719

Answer 2

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