Question

if eleanor starts with 25.00 ml of a weak acid (the concentration is 0.1084 m), then how many ml of 0.1817 m naoh has to be added to reach the equivalence point

Answer 1

Answer:

14.91 mL

Explanation:

Assuming the weak acid is monoprotic, we can solve this problem using the equation:

• C₁V₁=C₂V₂

Where subscript 1 stands for the Volume and Concentration of the weak acid, while 2 stands for those of NaOH.

We input the data:

• 25.00 mL * 0.1084 M = 0.1817 M * V₂

And solve for V₂:

• V₂ = 14.91 mL

Answer 2

The volume of 0.1817 M NaOH has to be added to reach the equivalence point is 14.91 mL.

How we calculate the volume?

Volume for the given solution will be calculated from the below equation:

M₁V₁ = M₂V₂, where

M₁ = Molarity of weak acid = 0.1084 M

V₁ = volume of weak acid = 25 mL

M₂ = molarity of NaOH = 0.1817 M

V₂ = volume of NaOH = to find?

On putting all these values on the above equation and calculate for V₂ as:
V₂ = (0.1084)(25) / (0.1817) = 14.91 mL

Hence required volume is 14.91 mL.

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