Question

To a flask, 15.0 mL of 1.25 M hydrofluoric acid is added. Then, 3.05 M KOH is used to titrate the acid sample. Write the balanced net ionic equation for the acid-base reaction.

Answer 1

H+ (aq) + OH-(aq) → H2O(l)

Step-by-step explanation:

Step 1: Data given

Volume of hydrofluoric acid = 15.0 mL = 0.015 L

Molarity = 1.25 M

Molarity of KOH = 3.05 M

Step 2: The unbalanced equation

HF(aq) + KOH(aq) → KF(aq) + H2O(l)

This equation is already balanced

Step 3: The net ionic equation

The net ionic equation shows only those elements, compounds, and ions that are directly involved in the chemical reaction.

The elements, compounds, and ions that do not take part in the chemical reaction are called spector ions.

H+ (aq) + F-(aq) + K+(aq) + OH-(aq)→ K+(aq) +F-(aq) + H2O(l)

We'll remove all the spector ions.

H+ (aq) + OH-(aq) → H2O(l)

Answer 2

HF + OH- = F- + H2O

Step-by-step explanation:

Since hydrofluoric acid does not ionize in aqueous solution, the fluoride ion is still present as part of the product