40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 m naoh. after 20.0 ml of the base solution has been added, the ph in the titration flask is 5.10. what was the concentration of the original acetic acid solution? (ka(ch3cooh) = 1.8 × 10–5)

0.5 M

Explanation:

We have to start with the reaction between NaOH and CH3COOH:

We will have a 1:1 ratio between the acid and the base. The next step then would be the calculation of the moles of NaOH and his convertion to moles of CH3COOH.

The final step is the calculation of the concentration of the acid.

Due to the Ka value we can use the acetic acid as a strong acid.

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).