What is the percent ionization of 0.2 M of acetic acid (K = 1.8 x 10-5)? O 0.17 % o 1.7 x 10-3 % O 0.0134 % O 0.0087 % O 0.87%
a) The degree of ionization of acetic acid (CH3COOH) in a 0.1 M aqueous solution at 25 oC is 0.013. Ka 1.7 X 10-5. What is the ph of this solution? What is the deg of ionization b) A solution is prepared to be 0.1 M acetic acid CH,COOH and 0.2 M CHCOONa. What is the pH of this solution at 25°C ? K, for acetic acid at this temperature -1.7 X10
A weak acid has a K, of 1.8 x 10-7. What is the value of pK, for the acid? PK, -
on 2 of 5 > If the K of a monoprotic weak acid is 1.7 x 10-6, what is the pH of a 0.38 M solution of this acid? pH= TOOLS *10 about s c contac reen privacy policy terms of use
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2. Which species is the conjugate base of HPO 2-? Refresher of Acid/Base Equilibria, Ka, and pK., and buffer solutions: 1. The (H30') in a cabernet Sauvignon wine is 5.9 x 10 M. What is the (-OH) in this wine? 2. The pH of a lime is 1.90. What is the [H30*]? 3. What is the pH of a cleaning solution with a [H3O+] =...
calculate Ka and pKa
PR, ANALYSIS Units Trial 1 pk, of acetic acid unitless ♡ 4.85 Trial 2 4.70 ♡ € Average experimental pk, of acetic acid (Intermediate value) unitless 4.775000 (Final value) unitless 4.78 Calculate experimental K, of acetic acid (use average experimental pk (Intermediate value) unitless (Final value) unitless Calculated pk, of acetic acid (from literature value, K. = 1.8e-5) (Intermediate value) unitless (Final value) unitless Calculate % error in experimental pK (Intermediate value) (Final value)
3. Consider the following weak acids and their K, values, calculate the pK, for each acid. HC,H,O, - Acetic acid K. = 1.8 x 105 PK,= H,PO, - Phosphoric acid K = 7.1 x 10 PK, HCIO - Hypochlorous acid K = 3.5 x 10 pk = You want to prepare buffers at pH 2.8, 4.5 and 7.5. Which weak acid-conjugate base buffer system is the best choice for each pH from the acids listed? Write the reaction and indicate...
If a solution of acetic acid (K = 1.8 x 10-5) has a pH of 2.90, calculate the original (initial) concentration of acetic acid (HC,H,O) (Report your answer in 1 sig. fig. Example: .03942 would be reported as 0.04) Be sure to include a zero in front of the decimal point. QUESTION 37 5 points Save Answer The K, for benzoic acid C.H.COOH is 6.3 x 106. Calculate the equilibrium concentrations of H,0* in the solution if the initial concentration...
pH of solution of acetic acid (K, - 1.8 10-5) is 3. What is concentration of the acid? 0.018 M 0.056 M 0.006 M O 1.8 M
Concentration is not given.
Acetic acid (CH, COOH, K, = 5.62 x 10-5) is a weak acid, so the salt sodium acetate (CH, COONa) acts as a weak base. Calculate the pH of a 0.563 M solution of sodium acetate. pH =