Figure 2:Re-arranging the expressions below, make a separate plot showingthe concentration of the protontated form and the de-protonatedform (both on the y-axis) for a total acid concentration of 0.01M forthe same pH values you used above (x-axis).αHA[HA][A] TOT[A-]αA-=[A] TOT

This code will generate a plot showing the concentration of the protonated form ([HA][HA]) and the…

Answered: Figure 2: Re-arranging the expressions…

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter20: Carboxylic Acids And Nitriles

Section20.3: Biological Acids And The Henderson–hasselbalch Equation

Problem 5P: Calculate the percentages of dissociated and undissociated forms present in the following solutions:...

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Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30
( Compare a to an acd with a large Ka Arswer the following questions about Ka and pka a What is Ka (b) Does a strong acid have a greater or lesser tendency to lese its proton than a weak acd na strong acid and a weak acid Who has a bigrer pa (d) Does the acid w (el Write the HHequation
I understand that Ka refers to the rate (constant) that HA acid dissociates into base A- and proton H+. I don't understand the pKa equation. What is the "p"? What does negative logarithm mean? Thank you.
For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid? Q.) chloroacetic acid, Ka = 1.38 X 10-3
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
+ 2) HA is a weak acid. HA is dissociated to H and A in water. At equilibria, if the pH of the solution is 3.24, then what is the concentration of A. [A [H*] At what condition, pH = pka? 3) pH = pKa + log
Determine the acetic acid concentration in a solution with [CH3CO2-] = 0.35 M and [OH-] = 1.5 x 10-5 M at equilibrium. The reaction equation is: CH3CO2- (aq) + H2O (l) ⇌ CH3CO2H (aq) + OH- (aq) (Acetic acid Ka = 1.8 x 10-8)
18). The formulas and the structures of two acids are shown below. Which acid is a stronger acid? If the acid strength of the two acids is equal, say so. Cl2CHCOOH CH3COOH но но CI-C-C-OH н-с-с-он ČI Ką = 0.0324 Ką = 1.82 x 10-5 %3D a. Cl¿CHCOOH is a stronger acid than CH;COOH. b. CH;COOH is a stronger acid than CI½CHCOOH c. The two have equal acid strength. d. none of the above
Q2-3:(a) Given that Kb for ammonia is 1.8 X 10 -5 and that for methylamine is 4.4 X 10 -4, which is the stronger base? (b) which is the stronger acid ,the ammonium ion or the methylammonium ion ? (c) calculate the Ka for NH,* and CH;NH;* + Q2-4: A particular sample of vinegar has a pH of 2.90, assuming that the vinegar contains only acetic acid (Ka acetic acid in vinegar . 1.8 X 10 -5), calculate the concentration of Q2-5: Calculate the molar concentration of OH-ions in an 0.85M solution of hypobromite ion , BrO- (Kp 4.0X10-6) .what the pH value of this solution?
The question is in the photo attatched. Additonal information: intial pH measurment: 3.30 inital volume: 0.0L weak acid concentration: 0.042M weak acid volume: 0.25L NaOH concentration: 0.1M NaOH volume at equilibrium: 0.105L HA (aq) + NaOH (aq) -> NaA (aq) + H2O(l) HA being the unknown acid.
Be sure to answer all parts. Which indicators that would be su ble for each of the following titrations: (a) CH;NH, with HBr thymol blue bromophenol blue methyl orange methyl red chlorophenol blue bromothymol blue O cresol red O phenolphthalein (b) HNO, with NaOH thymol blue bromophenol blue methyl orange methyl red chlorophenol blue bromothymol blue cresol red phenolphthalein (c) HNO, with KOH thymol blue O bromopbenol blue methyl orange methyl red chlorophenel blue
Which H is most acidic? Highlight this H. Ci: •S. H Which site is most basic? Highlight this site. H H H H ? 마 Ar

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Figure 2: Re-arranging the expressions below, make a separate plot showing the concentration of the protontated form and the de-protonated form (both on the y-axis) for a total acid concentration of 0.01M for the same pH values you used above (x-axis). αHA [HA] [A] TOT [A-] αA- = [A] TOT