The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.540 moles of a monoprotic weak acid (Ka = 4.7 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.540 moles of a monoprotic weak acid (Ka = 4.7 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =

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 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

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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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The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other hall still remains unreacted if 0.360 moles of a monoprotic weak acid (K, = 4.8 x 10^-5 ) is titrated with NaOH, what is the pH of the solution at the half -equivalence point? pH =
The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka = 5.3 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.220moles of a monoprotic weak acid (?a=5.1×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (?a=5.3×10^−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted.If 0.340 moles of a monoprotic weak acid (Ka=6.3×10−5) is titrated with NaOH ,what is the pH of the solution at the half‑equivalence point?
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The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.320 moles of a monoprotic weak acid (Ka=1.7×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH=
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Similar to acetic acid, benzoic acid is a weak acid (HA) and is a commonly used as antimicrobial preservative in food and beverages, especially in carbonated beverages Suppose 10.00-mL of 0.5000 M benzoic acid (C6H5COOH) is titrated with 0.2000M NaOH. Ka for benzoic acid is 6.3 x 10-5 . What is the pH after addition of 35.00 mL of NaOH to the benzoic acid solution?
Calculate the pH for the titration of 50.00 mL of 0.0500 M NaCN with 0.1000 M HCl after addition of the following volumes of titrant. The reaction is CN⁻ + H₃O⁺ -> HCN + H₂O a) 0.00 mL (solution of the weak base) b) 10.00 mL (buffer solution of the weak base and conjugate acid) c) 25.00 mL (solution of the conjugate acid) d) 26.00 mL (solution of the excess acid titrant)