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13 Dec 2019

Calculate the pH of a buffer solution containing 0.25 moles sodium acetate and 0.30 moles acetic acid (HOAc) to which 0.20 moles HCl are added. pKa (HOAc) = 4.74

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Related questions

Calculate the pH of the following buffer solutions: (anwers given in bold)

1) A solution obtained by adding 30 mL of 0.20 M HOAc to 25 mL of 0.10 M NaOH. R = 4.61

2) A solution that is 0.050 M in formic acid and 0.10 M in sodium form. R = 4.0

3) A buffer solution of acetic acid-sodium acetate of pH 5.00 (initial) whose concentration in NaOAc is 0.100 M, after the addition of 10 mL of 0.1 M NaOH to 100 mL of the buffer. R = 5.12

What volume of 0.20 M NaOH is required to reach the equivalence point if you start with 10-mL of an acetic acid/acetate buffer with pH 4.74? NOTE: The pKa of acetic acid is 4.74

What volume of 0.20 M HCl is required to fully protonate all of the acetate in 10-mL of an acetic acid/acetate buffer with a pH of 4.74?

How will the volumes differ from your answers in Questions 3 and 4 if the buffer has a pH greater than 4.74?

How will the volumes differ from your answers in Questions 3 and 4 if the buffer has a pH less than 4.74?

Can i please get help with all these questions ?

these are two previous questions but i already answer them hopefully they help out with the ones i need help on.

Calculate the molarity of a 5% (w/v) solution of acetic acid (household vinegar).

Calculate the equivalence point volume for the titration of 10-mL of 5.0% acetic acid titrated with 0.20 M NaOH.


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