Determine the pH during the titration of 14.8 mL of 0.286 M hydrobromic acid by 0.110...

Determine the pH during the titration of 14.8 mL of 0.286 M hydrobromic acid by 0.110 M sodium hydroxide at the following points:

(1) Before the addition of any sodium hydroxide

(2) After the addition of 19.3 mL of sodium hydroxide

(3) At the equivalence point

(4) After adding 47.7 mL of sodium hydroxide

Solutions

Expert Solution

HBr is a strong acid

so it dissociates completely to produce H⁺ and Br^- in solution

1) before addition of sodium hydroxide

the concentration of HBr = 0.286M

so HBr H⁺ + Br^-

so concentration of H⁺ = 0.286M

pH = -log[H⁺]

pH = -log(0.286) = 0.544

2) after addition of 19.3mL of sodium hydroxide

now the real acid-base chemistry comes into play

Acid + base salt + H₂O

HBr + NaOH NaBr + H₂O

but now the concentration changes as the volume is change

the concentration of HBr in 14.8mL is 0.286

after addition of 19.3mL of NaOH total volume changes to = 14.8+19.3 = 34.1

we solve question using mole concept (means 1mole of acid reacts with 1 mole of base )

queen_honey_blossom answered 1 year ago

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