A buffer solution based upon sulfurous acid (H2SO3) was created by treating 1.00 L of a 1.00 M sulfurous acid solution with NaOH until a pH of 1.135 was achieved (assuming no volume change). To this buffer 1.180 moles of NaOH were added (assume no volume change). What is the final pH of this solution

The final pH of this solution is 7.69

Explanation:

having the chemical reaction:

H2SO3 = HSO3- + H

Ka = 1.5x10^-5

pKa = 1.82

H2SO3 + OH- = H2O + HSO3-

1                  ?                      0

1-x               0                      +x

the pH is equal to:

pH = pKa + log([HSO3-]/[H2SO3])

1.135 = 1.82 + log(x/(1-x))

Clearing x:

x = 0.17

Having the reaction:

H2SO3 + OH- = H2O + HSO3-

0.83         1.180                 0.17

0                 0.83                1

HSO3- = SO3-2   +   H+

Ka2 = 1x10^-7

pKa2 = 7

HSO3-  + OH- = SO3-2 + H2O

1              0.83       0

0.17            0          0.83

pH = pKa2 + log([SO32-]/[HSO3-]) = 7 + log(0.83/0.17) = 7.69

they include patterns; cause and effect; scale, proportion, and quantity; systems and system models; energy and matter; structure and function; and stability and change.

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i answered it first

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.