1. Based on the shape of the curve, what is the nature of the analyte? Strong acid Strong base Weak acid None of the choices Weak base 2. What about the titrant used? Weak Base Strong Acid Strong Base Weak Acid None of the choices 3. At what pH would you expect the equivalence point to fall? Would it? At pH 10.50 Below 7.00 At 7.00 None of the choices Above 7.00 4. Which of the following can be said to be true of the concentrations of the species at some point before the equivalence point? None of the choices base = conjugate base acid = base acid = conjugate base conjugate acid < conjugate base

1. Based on the shape of the curve, what is the nature of the analyte? Strong acid Strong base Weak acid None of the choices Weak base 2. What about the titrant used? Weak Base Strong Acid Strong Base Weak Acid None of the choices 3. At what pH would you expect the equivalence point to fall? Would it? At pH 10.50 Below 7.00 At 7.00 None of the choices Above 7.00 4. Which of the following can be said to be true of the concentrations of the species at some point before the equivalence point? None of the choices base = conjugate base acid = base acid = conjugate base conjugate acid < conjugate base

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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3 a) The Ka value for phenolphthalein is 8 x 10-10. What is the concentration of hydrogen ton when this indicator changes colour? b) What is the pH at end paint? c) From your pH curve, why is the assumption that end point equals equivalence point valid for phenolphthalein?
At which point of a titration curve, is the pH value of the solution equal to the pKa of the weak acid? O at the quarter equivalence point O at the equivalence point O 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 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )
In the titration of HF with NaOH, which species are present at the equivalence point? O HF, NAOH, and H20 only O NaF, NAOH, and H20 only O NaF, HF, and H20 only O NaF and H20 only O HF and H20 only
From the standard properties of plotted titration curves, which one best represents the titration of a weak acid with a strong base? The curve is with a semi S orientation with the midpoint of the steep part at pH 7 The curve is with a semi Z orientation with the midpoint of the steep part at pH 7 The curve is with an "S' orientation with the midpoint of the steep part at pH > 7 The curve is with a "Z" orientation with the midpoint of the steep part at pH <7 Representative curve cannot be predicted
A student obtains the following data from the Determining the pKa of an Acid-Base Indicator experiment. Using this data, calculate the pKa of the indicator in the fourth solution. Solution Abs. pH 3.4 + HCI 0.054 pH 4.6 + NaOH 0.564 Sample # 1 2 345 actual pH 3.34 3.73 3.96 4.22 4.50 Abs. 0.135 0.214 0.295 0.382 0.460
Which of the following factors can affect the endpoint calculations in a titration? all of the choices can affect the calculations presence of an air bubbles on the nozzle of the buret not starting at exactly 0 reading O the amount of water used to dissolve the KHP
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically greater than the moles of the analyte? post-equivalence pre-equivalence equivalence end stage