Order these steps for how you will determine pKa of a weak acid using a titration curve? (from 1 to 4)  ____ Identify the volume of base required to reach the equivalence point.  ____ Identify the pKa of the acid as the pH at the half-equivalence point.  ____ Calculate the volume of base required to reach the half-equivalence point.  ____ Identify the pH at the half-equivalence point.

Please step by step answer and current answer please

4. A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 \times 10-4) with 0.10 M NaOH.a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak base? (1 point) b. Estimate the pH at the equivalence point. Will it be equal to 7, greater than 7, or less than 7? Explain. (1 point) c. What is the pH after 20.0 mL of the 0.10 M NaOH is added? Show all calculations. (3 points)

acetic acid is a: ______ strong acid, strong base, weak acid, or weak base?? (Circle one) What should be the equivalence point pH be for this experiment? less than 7, equal to 7, pr greater than 7?? (Circle one) Why is the half-equivalence pH (and half-equivalence volume) important in this titration? Explain. From the graph, estimate the half-equivalence volume: ________________ mL From the graph, estimate the half-equivalence pH: ________________ Using these values, calculate the value of Ka for acetic acid: ________________ Acetic acid has a known Ka of 1.8 x 10-5 via the literature. Find the percent error for this experiment. Recall: Percent error = absolute value{(actual - experimental)/ actual}*100%