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11 Nov 2019

1)25.0 ml of 0.600M hypobromous acid, HBrO, is titrated with 0.400M sodium hydroxide, NaOH. Calculate the pH of the solution after the addition of 20.0 ml of NaOH solution.

2)15.0 ml of 0.750M propanoic acid, HC₃H₠O₂, is titrated with 0.500M sodium hydroxide, NaOH. Calculate the pH of the solution at the equivalence point of the titration.

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Trinidad Tremblay
Trinidad TremblayLv2
25 Jan 2019

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Related questions

Calculate the pH when 15.0 mL of 0.20 M Benzoic Acid (HC7H5O2 Ka = 6.5x10-5) is titrated with 20.0 mL of 0.15 M sodium hydroxide (NaOH)

Can you exaplain how to solve this question?

1)How many grams of solid potassium hypobromite, KBrO must be added to 200.0 ml of 0.100M hypobromous acid in order to form a buffer with a pH = 8.75?

2)A buffer solution is formed by adding 0.200 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.500 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.

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Calculate the pH of the buffer solution after the addition of 10.00 ml of 2.50 M KOH.
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Propionic acid is a weak organic acid. A 0.123 M propionic solution is titrated by a 0.123 M sodium hydroxide solution. The initial volume of the propionic solution is 65.0 mL.

The Ka of propionic acid is 1.34 x 10-5.

A. Calculate the pH before any sodium hydroxide has been added (initial solution)

B. Calculate the pH after 20.0 mL of sodium hydroxide has been added.

C. Calculate the pH after 50.0 mL of sodium hydroxide has been added.

D. Calculate the pH at the equivalence point

E. Calculate the pH after 80.0 mL of sodium hydroxide has been added.

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