. (5 pts) The pKa of HF is 3.17. a) Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF. b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCI?
In a titration of 0.035 L of 0.44 M HF, a solution of 0.44 M NaOH was added. What is the pH after 33.0 mL of base is added? Ką of HF = 7.2 x 104
Estimating pH 1. If you combine 40.0 mL of a 0.80 M HF solution with 60.0 mL of a 0.60 M NaF solution, which of the following is correct? HF pKa = 3.17. a) pH will be > 3.17 b) pH will be < 3.17 c) pH will equal 3.17 2. If 1.50 mL of 1.0 M HNO3 is added to a solution containing 40.0 mL of 0.80 M HF and 60.0 mL of 0.60 M NaF, what will happen...
Find the pH and percent ionization for each HF solution. (Ka for HF is 6.8 x10-4.) Please use this Ka that is given to solve a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF
1) Find the pH of 0.200 M HF acid solution 2) Find the pH of a and [H3O+] of 0.100 M benzoic acid solution Explain how you got answer!
The pK, value for HF is 3.14. Would a buffer prepared from HF and KF with a pH of 2.64 be considered to be an effective buffer? A buffer in which the mole ratio of KF to HF is 0.42 has a pH of 2.76. Would this buffer solution have a greater capacity for added acid (H,0) or added base (OH)? added acid added base Submit Answer Retry Entire Group 1 more group attempt remaining A buffer solution that is...
Find the pH and percent ionization of each HF solution (Ka for HF is 6.8 X 10^-4) Please show your work, and explain. Thank you! Co < CHE180 Review Exercise 16.77 Find the pH and percent ionization of each HF solution (Ka for HF is 6.8 x 104) PartA Find the pH of a 0.240 M solution. Express your answer to two decimal places. pH Submit Previous Answers Request Answer X Incorrect; One attempt remaining: Try Agairn Part B Find...
Question 17 pK,(HF)-818. What is the pH after 2.00 ml of 0.25 M KOH is added to 10.00 ml of 0.50 M HF Answer numerically. Do not use scientific notation.
Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39, what is the K_a of the acid? K_a = Hydrofluoric Acid, A weak Acid with K_a = 7.1 times 10^-4 A. For a 0.50 M solution of HF, calculate the equilibrium concentrations of HF, H^+ and F^-. [HF] = [H^+] = [F^-] = % Dissociation =, pH = B. Now consider a 0.050 M solution of HF....
Ephedrine is a weak base. A 0.035 M solution of ephedrine has a pH of 11.33. What is the base ionization constant (Kb) for ephedrine? () 7.8 x 10-10 () 1.5 x 10-9 () 9.8 x 10-5 () 1.4 x 10-4