suppose you perform a titration of an unknown weak acid solution. you start with 4.00 ml of the weak acid and find that it takes 18.3 ml of 0.0500 m naoh to reach the equivalence point. what is the concentration of the unknown weak acid solution? enter your answer to three significant figures in units of m.

Acid dissociation constant, K a K text a Ka, and weak acids. Acids that don't entirely dissociate in solution are referred to as weak acids. In other words, any acid that is not a strong acid qualifies as a weak acid. The amount of dissociation determines how strong an acid is; the more dissociation, the stronger the acid.

Equivalent point:

Since the volume is 4.00 mL of the weak acid, and it takes 18.3 mL of 0.0500 M NaOH to reach the equivalence point.

We know that

In the equivalence point, [H⁺] = [OH⁻].

here the given formula C₁V₁=C₂V₂ is used

Here

C₁ = 0.0500 M

V₁ = 18.3 mL

C₂ = ?

V₂ = 4.00 mL

So, the C₂ is

0.0500 M * 18.3mL = C₂ * 4.00 mL

C₂ = 0.228M

The concentration of the unknown weak acid solution is 0.228 M

To learn more about concentration refer to:

brainly.com/question/17206790

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