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)

Consider a buffer made by adding 132.8 g of NaC-H5O, to 300.0 mL of 1.97 M HC-H.O, (Ka = 6.3 x 10-5)   a. What is the pH of this buffer?   b. What is the pH of the buffer after 0.750 mol of H+ has been added?   c. What is the pH of the buffer after 0.250 mol of OH- has been added?

A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4).   A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?

Answer the following questions about a titration between 20.0 mL of a weak base (Kb= 4.7*10-6) and 0.150 M hydrochloric acid. A.What is the concentration of the weak base solution if it requires 26.67 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of bruhmophenol is ~ 4.9 and the pKa of thymol blue ~ 9.2. Which indicator would be best to use in the titration