In a titration, the equivalence point occurs when the amount of titrant added is sufficient to neutralize the analyte solution. At this point, the number of moles of titrant (standard solution) equals the number of moles of the unknown concentration solution.
What will be the pH at the equivalence point of strong base weak acid titration?
In the titration of a weak acid with a strong base, protons are transferred directly from the weak acid to the hydroxide ion.
In a titration of a weak acid with a strong base, the endpoint point is shifted from neutralization to the pH of the strong reagent (base). The equivalence point is reached when the moles of acid added stoichiometrically balances the moles of base added. In a titration of a weak acid with a strong base, the pH of the solution at the equivalence point is greater than 7.
For example, the reaction of the weak acid, acetic acid (CH3COOH) with a strong base, sodium hydroxide (NaOH).
What will be the pH at the equivalence point during the titration of a 1000 ml of 0.2 M solution of CH3COONa with 0.2 M solution of HCl?
- A: 3+log√2
- B: 3−log2
- C: 3−log√2
- D: 3+log2
The correct answer is option C: 3−log√2
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