The reaction of a weak base and a strong acid goes to completion; that is one of the reactants is completely reacted away. The resulting solution contains theconjugate acid of the weak base, plus any weak base or strong acid that remains unreacted.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 [H3O*] 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 (CH3NH,, K, = 4.2x104) by 0.336 M HI at the following points. (Assume the titrationis done at 25 °C.)Note that state symbols are not shown for species in this problem.(a) Before the addition of any HI(b) After the addition of 16.2 mL of HI(c) At the titration midpoint(d) At the equivalence point(e) After adding 56.0 mL of HI

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Determine the pH during the titration of 37.3 mL of 0.336 M methylamine (CH3NH2, K = 4.2×10*) 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 (b) After the addition of 16.2 mL of HI (c) At the titration midpoint

Determine the pH during the titration of 37.3 mL of 0.336 M methylamine (CH3NH2, K = 4.2×10*) 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 (b) After the addition of 16.2 mL of HI (c) At the titration midpoint

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 65QAP: Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105)....

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Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Consider the following two acids: In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results. (See Exercise 113.)
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Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.