a. Given the titration curve above, is Malonic acid a mono-, di- or triprotic acid? Explain your answer. b. H many buffer regions and equivalence points are present? Indicate each with A-E. C. vvrite out the reactions and the equilibrium expressions associated with Kai and Kaz.

a. Given the titration curve above, is Malonic acid a mono-, di- or triprotic acid? Explain your answer. b. H many buffer regions and equivalence points are present? Indicate each with A-E. C. vvrite out the reactions and the equilibrium expressions associated with Kai and Kaz.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

10. When 100.0mL of 0.10 M malonic acid (H;CH;C;O.) is titrated with 0.10M NaOH the following
titration curve is observed:
pH
12-
10"
50
100
150
200
vol. of NaOH added (mL)
a. Given the titration curve above, is Malonic acid a mono-, di- or triprotic acid? Explain
your answer. a
b. H many buffer regions and equivalence points are present? Indicate each with A-E.
C.
vvrite out the reactions and the equilibrium expressions associated with Kai and Ka2.

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2. Calculate the grams of formic acid, HCOOH should be added to 25 ml of 0.1 M potassium formate, HCOOK solution if we want to prepare a buffer solution of pH= 5.50. Given pKa for formic acid is 3.75 .
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2. Calculate the volume of the salt preparation of 200 ml of the following buffer solutions. S BUFFER DESIRED NUMBER pH 5 Tale 6 7 8 210 6.90 7.18 9.45 8.25 0.1M SOLUTIONS TOT NaH₂PO4/Na₂HPO4 NaH₂PO4/Na₂HPO4 NH4CI/NH3 NH4CI/NH3 pka to be used in the 6.80 6.80 9.30 9.30 VOLUME OF SALT (ml)
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Please help.
At each stage of the titration: A. Determine the amount (mol) of weak acid, weak base, and strong acid present. B. Determine the total volume of the combined solutions. C. Determine [H;O*] or [OH], whichever predominates, using the total volume and the nature of the solution: weak base, buffer, weak acid, or strong acid. D. Calculate pH. Determine the pH during the titration of 37.3 mL of 0.336 M methylamine (CH3NH2, K, = 4.2x10-4) by 0.336 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI 12.067 (b) After the addition of 16.2 mL of HI 10.74 (c) At the titration midpoint 10.62 (d) At the equivalence point (e) After adding 56.0 mL of HI
the sodium acetate - acetic acid buffer keep the pH: a. =4.8 b. = 8.9 C. = 1.8 O d. = 7.7
25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the endpoint. e)Would the compound formed at the equivalence point be acidic, basic or neutral? Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration? g)Sketch a titration curve for this reaction. Label the x and y axes.