Final answer:
To calculate the pH of the solution resulting from mixing 150.0 mL of 0.25 M HF with 225.0 mL of 0.30 M NaF, you need to consider the dissociation reactions of both HF and NaF in water. The pH of the resulting solution is 1.85.
Step-by-step explanation:
To calculate the pH of the solution resulting from mixing 150.0 mL of 0.25 M HF with 225.0 mL of 0.30 M NaF, we need to consider the dissociation reactions of both HF and NaF in water.
HF is a weak acid and will partially dissociate, while NaF is a salt that will dissociate completely.
The dissociation of HF can be represented by the equation: HF (aq) → H+ (aq) + F- (aq).
The dissociation of NaF can be represented by the equation: NaF (aq) → Na+ (aq) + F- (aq).
Since NaF dissociates completely, we can consider the F- ion concentration to be equal to the NaF concentration.
The HF concentration will decrease slightly due to dissociation.
We can set up an ICE table to calculate the concentrations of H+ and F- after mixing the solutions.
Using the ICE table, we find that the concentration of H+ is 0.014 M and the concentration of F- is 0.285 M.
To calculate the pH, we can use the formula: pH = -log[H+].
Substituting the concentration of H+ into the formula, we get a pH of 1.85.