please help me asner this question correctly and how all your steps asap! A student prepares a 0.40 mM aqueous solution of acetic acid (CH,CO,H). Calculate the fraction of acetic acid that is in the dissociated form in his solution.Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource.Round your answer to 2 significant digits.||%х10 oh DataFor example, the potentials you'll need to calculate the voltage of a battery.[-] pka of weak acids at 25°CnameformulapKa1pKa2pKa3аcetic acidCH3CO2H4.756acetylsalicylic acidC9H8O43.52ascorbic acidC6H8O64.04benzoic acidC6H5CO2H4.204butanoic acidC3H,CO2H4.83carbonic acidH2CO36.3510.334-chlorobutanoic acidC3H6CICO2H4.52chlorous acidHCIO21.94crotonic acidC3H5CO2H4.69formic acidHCO2H3.75hypochlorous acidHCIO7.40hydrocyanic acidHCN9.21hydrofluoric acidHF3.20

To can fraction of dissociated form , we need to be the concentration of ions after dissociation of…

A student prepares a 0.40 mM aqueous solution of acetic acid (CH,CO,H). Calculate the fraction of acetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.

A student prepares a 0.40 mM aqueous solution of acetic acid (CH,CO,H). Calculate the fraction of acetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 82AP

See similar textbooks

Similar questions

An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 104) and 0.150 M CH3CH2COOH (Ka = 1.34 105). Calculate the pH of this solution. Because both acids are of comparable strength, the H+ contribution from both acids must be considered.
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
. Calculate the pOH value corresponding to each of the pH values listed, and tell whether each solution is acidic or basic. a. pH = 10.75 b. pH = 3.66 c. p1-I = 1.98 d. pH = 12.47
Calculate the acid dissociation constant, Ka, for hydrogen cyanide, HCN, based on the given information. (CN),(g) + 2 H*(aq)+2 e¯= 2 HCN(aq) E° = 0.373 V Eº! = -0.041 V -10 Ka = 1 x10
Calculate the acid dissociation constant, Ka, for hydrogen cyanide, HCN, based on the given information. (CN),(g) + 2 H (aq) + 2 e= 2 HCN(aq) E° = 0.373 V Eo! = -0.041 V Ka = 1 x10-10
when chlorine gas is added to water during the disinfection of drinking water, it hydrolyzes with the water to form HOCL. The disinfection power of the acid HOCL is 88 times better than its conjugate base, OCl-. The pKa for HOCl is 7.5. (a) what percentage of the total disinfection power exists in the acid form at pH of 6?
For a 0.15 M H3PO4(aq) solution, determine pH [H3PO4], [H2PO4-], [HPO42-], and [PO43-]
Calculate the acid dissociation constant, Ka, for hydrogen cyanide, HCN, based on the given information. (CN), (g) +2H+ (aq) + 2 e= 2 HCN(aq) E° = 0.373 V E = -0.041 V
(2) ibäi The pOH for 0.2 M sulfuric -2 acid solution is
Which statement is correct regarding the acid-base equilibrium system below? OH HN spontaneous in forward direction, because H3CCH»NH;" is a weaker acid than HạCCH-OH spontaneous in forward direction because H3CCH2NH3\» a stronger acid than III. spontaneQUs InTeverse directon, because #H3CCH2NH3¯ is = stionger ad the HICCH OH. IV. spontanecIS in reverse direction, becauseH CH NHT zensetacid than H O Suggestion: Look up the pka valties for the acids invalved in the above reaction to best support your response! Table provided below. Keywords cher tal egol boun pra the moynamaltlelabe cs Fre+ Enertatharige weakest acid stronceaddi weakest tase s une fehw teictidENE Jeren Concepts Impicanions of pra farithemical eguabrn
Initial pH: 1.55 Molarity: 0.081158