Ka = 10^(-pka)
if ka is 1.8E-5 then, solve for Pka for acetic acid.
a) The Ka for acetic acid (H3CCO2H) is 1.737 × 10–5. What is the pKa for this acid? b) Use the pKa calculated above to determine the pH at which [H3CCO2H]=[H3CCO2-].
(a) Calculate the percent ionization of 0.00710 M acetic acid (Ka = 1.8e-05). % ionization = ? % (b) Calculate the percent ionization of 0.00710 M acetic acid in a solution containing 0.0340 M sodium acetate. % ionization = ? %
nitrous acid pKa 4.5E10-4; HF 7.1E-4; Formic Acid 1.7E-4; Acetic Acid 1.8E-5; HCH 4.9E-10 1 Consider the titration of 40.0 mL of 0.0500 M NO2- with 0.100 M HBr a calculate the pH of the solution before the addition of any HBr b calculate the pH of the solution after the addition of 10.0 mL of HBr c calculate the pH of the solution after the addition of 20.0 mL of HBr
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)
For a buffer made from sodium acetate and acetic acid, the Ka of acetic acid is 1.8E-5. What mass of sodium acetate (NaCH3CO2) must be added to 2.50 L of 0.68 M acetic acid to make a buffer solution with pH = 5.75? The answer should be in two significant figures.
(a) Calculate the percent ionization of 0.00660 M acetic acid (Ka = 1.8e-05). % ionization = % (b) Calculate the percent ionization of 0.00660 M acetic acid in a solution containing 0.0220 M sodium acetate. % ionization = % + -10.1 points 0/4 Submissions Used A buffer solution contains 0.70 mol of hydrogen peroxide (HOOH) and 0.87 mol of sodium hydrogen peroxide (NaOH) in 5.80 L. The Ka of hydrogen peroxide (HOOH) is ka = 2.4e-12. (a) What is the...
Follow up questions 01. Find the accepted values for the pKa and Ka of acetic acid. How well do the accepted values compare with your calculated values? Explain. Lab 7 Determining Ka by the Half-Titration of a Weak Acid 1. Data table Titration Results NaOH volume at equivalence point NaOH volume at half equivalence point pH at the equivalence point pH at half equivalence point pKa of acetic acid Ka of acetic acid Trial 1 22.72 11.36 7.63 Trial2 23.26...
If acetic acid is the only acid that vinegar contains (Ka=1.8×10−5), calculate the concentration of acetic acid in the vinegar. the particular sample of vinegar has a PH of 3.15
At the equivalence point of a titration of HOAc (acetic acid, pKa = 1.76 x 10-5) with NaOH, the species present of OAc" and H20. If the concentration of OAc at the equivalence point is 0.50 M, what is the pH of the solution? Remember that Kb x Ka = 10-14 and that the OAc will react with water as follows: OAC- + H20 --> HOÀc + OH- . 1 4.77 2. 10.23 3 5.68 4. 9.23
Calculate the [H+] and pH of a 3.11×10^−4M acetic acid solution. The Ka of acetic acid is 1.76 × 10 ^−5.