10. 0.01 mol of HCl were added to 1 Lofa buffer solution containing 0.08 mol of CH_(3)COOH and 0.04 mol of CH_(3)COONa. Calculate the pH of the resulting solution (forCH_(3)COOHpK_(a)=4.76) . (round up the number to the nearest tenth) square

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Answer 1

To calculate the pH of the resulting solution, we can use the Henderson-Hasselbalch equation, which is given by:

where:-

is the negative logarithm of the acid dissociation constant (

) of the acid.-

is the concentration of the conjugate base.-

is the concentration of the acid.Given:-

for

= 4.76- Initial concentration of

= 0.08 mol- Initial concentration of

(conjugate base) = 0.04 mol- Amount of

added = 0.01 molFirst, we need to determine the new concentrations of

and

after adding

.Since

is a strong acid, it will dissociate completely in water, providing

ions. The

ions will react with the conjugate base (

) to form more

:

The new concentrations will be:- New concentration of

= Initial concentration of

+ amount of

added

- New concentration of

= Initial concentration of

- amount of

added

Now, we can plug these values into the Henderson-Hasselbalch equation:

Calculate the ratio inside the logarithm:

Now, calculate the logarithm:

Finally, add this value to the

:

Rounding to the nearest tenth:

So, the pH of the resulting solution is approximately 4.3.

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