1)
concentration of HCl = 0.12 M
concentration of HF = 0.75 M
[H+] = sqrt (Ka x C) = sqrt (6.8 x 10^-4 x 0.75)
= 0.0226 M
total [H+] = 0.12 + 0.0226 M
= 0.14 M
pH = -log [H+] = -log (0.14)
pH = 0.846
% ionization = ([H+] / C ) x 100
= 0.14 / (0.12 + 0.75) x 100
% ionization = 16.4 %
PH of solution & degree ionization pls help What is the pH of the solution and...
d) ka-9.jj×10 Ka 1.45 x 104 P19. (Sec. 15.5) What is the pH of a 0.35 M solution of nitrous acid, HNO2? [Hint: ICE Table & Percent Ionization] & (Ka 4.5 x 104) HNO2(aq)H(aq)+ NO2 (aq)4.5 x 1o a) 4.11 b) 3.29 c) 12.70 d) 1.90 e) 9.10 P20. (Sec. 15.5) What is the pH of a 0.095 M solution of hydrofluoric acid, HF? [Hint: ICE Table & Percent Ionization] & (Ka = 6.8 × 10-4) 4
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...
Q3. If a solution of hydrofluoric acid (HF; Ka=6.8 x104) has a pH of 2.12, calculate the initial concentration of hydrofluoric acid. HF (aq) = H (aq) + F (aq)
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
If a solution of HF (Ka=6.8×10^−4) has a pH of 3.50, calculate the concentration of hydrofluoric acid. So far, I've made 5 incorrect attempts at the answer and have one attempt remaining. My answers were as follows: 0.00015, 1.5x10^-4, 1.5x10^-5, 0.001, and 0.00032 (This last answer prompted the website to tell me: "This value is the concentration of H+. This concentration and the Ka value can be used along with the equation for Ka to determine the initial concentration of...
What is the pH of a solution obtained by mixing: 10.0 mL of 2.00 M hydrofluoric acid (HF) solution and 20.0 mL of 1.00 M hydrochloric acid (HCI) solution The Ka of hydrofluoric acid (HF) is 6.6 X 104 Show all of your work, give a final answer with the correct amount of significant figures. Correct answer is (0.176)
46. What is the percent ionization of a 0.491 M aqueous solution of carbonic acid? Ka1= 4.2x10^-7; Ka2= 4.8x10^-11 47. What is the percent ionization of a 0.356 M aqueous solution of hydrosulfuric acid? Ka1= 9.5x10^-8; Ka2= 1x10^-19 48. What is the pH of a 0.387 M aqueous solution of acetic acid? Ka (CH3COOH) = 1.8x10^-5 49. What is the pH of a 0.0398 M aqueous solution of benzoic acid? Ka (C6H5COOH) = 6.5x10^-5 50. What is the pH of...
1. The weak base hydrazine, N2H4, has a Kb = 1.7 x 10-6. What is the percent ionization of a 0.15 M solution? 2. Hydrofluoric Acid has a Ka of 6.8 x 10-4. Calculate the [H+] in 0.25 M HF: 3. What is the pH of a 0.050 M solution of Acetic Acid, HC2H3O2? 4. A solution has a pOH of 10.25. Calculate the [H+].
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you! Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...