Calculate the pH at the equivalence point in titrating 0.100M solutions of each of the following with 0.080 M NaOH(a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2)(c) benzoic acid (C,H5COOH).

Given: Concentration of NaOH= 0.080M To find: The pH at the equivalence point

Answered: Calculate the pH at the equivalence…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.26QAP

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Similar questions

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
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?
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A plot of pH vs volume of 0.05 M NaOH solution was obtained for titrating 0.4055 g of a dried solid sample of a weak, monoprotic acid. Determine the molar mass of the acid in its solid, crystalline form.
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In another experiment, the student titrated 50.0mL of 0.100MHC2H3O2 with 0.100MNaOH(aq). Calculate the pH of the solution at the equivalence point.
Calculate the pH at the equivalence point in titration 0.100 M solutions of each of the following with 0.080 M NaOH: a. hydrobromic acid (HBr) b. chlorous acid (HClO2) c. benzoic acid (C6H5COOH)
A solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.
What volume of 0.500 M HNO2 should be added to 500 mL of 0.750 M KNO2, so that the pH of the resulting buffer is 3.23 .

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Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH (a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2) (c) benzoic acid (C,H5COOH).