Answered: 7B. Write the chemical equation for the…

7B. Write the chemical equation for the acid/base equilibrium at the equivalence point of this titration and determine the pH of the solution at the equivalence point

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 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Question

Answer 7b

7. Kaydence titrated a 25.00 ml of 0.1250M oxoacetic acid (HA) solution with a 0.1080M NaOH solution
(in the buret). The Ka of oxoacetic acid is 1.8 x 105
7A Calculate the end point volume of NaOH,
I
7B. Write the chemical equation for the acid/base equilibrium at the equivalence point of this titration and
determine the pH of the solution at the equivalence point
7C. What is the pH of the solution after a total of 35.00ml of NaOH is added to the flask containing the acide
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Step 1: Given data

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Step 2: Calculation of volume at equivalence point

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Step 3: Calculation of total volume and moles of NaOH and acid

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Step 4: Determination of ICE table

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Step 5: Calculation of acetate molarity and new ICE table

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Step 6: Calculation of Kb value

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Step 7: Calculation of hydroxide ion concentration

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Step 8: Calculation of pOH and pH value

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A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
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