Question

At the equivalence point in an acid - base titration, the:

a. [H+] = [OH¯]

b. [H+] > [OH¯]

c. [H+] < [OH¯]

d. [OH-] is zero

Answer 1

Answer: At the equivalence point in an acid-base titration, the
`[H^+]=[OH^-]`

Step-by-step explanation:

An acid is defined as the substance which released hydrogen ions when dissolved in water.

A base is defined as the substance which released hydroxide ions when dissolved in water.

At equivalence point, then number of moles of hydrogen ions is equal to the number of moles of hydroxide ions.

There are 3 types of solution:

• If the solution has high hydrogen ion concentration than hydroxide ion concentration
  `([H^+]>[OH^-])`, then the solution will be acidic.
• If the solution has low hydrogen ion concentration than hydroxide ion concentration
  `([H^+]<[OH^-])`, then the solution will be basic.
• If the solution has equal hydrogen ion concentration and hydroxide ion concentration
  `([H^+]=[OH^-])`, then the solution will be neutral.

Hence, at the equivalence point in an acid-base titration, the
`[H^+]=[OH^-]`

Answer 2

Option A, [H+]= [OH-]

Step-by-step explanation:

Equivalence point is the one at which the amount of acid is equal to the amount of base in Acid-Base titration

Here concentration of Acid (H+)= [OH-] in option A.

If H+> OH-, acidic solution

OH->H+, basic solution.

Hence A is correct