Q(2): Which of the following will affect the calculated molarity of phosphoric acid solution when its titrated with standard NaOH to be higher than the correct value? Select one: a. Rinsing the inner wall of the titration flask with distilled water during addition of NaOH b. Rinsing the titration flask with small amount of phosphoric acid c. Rinsing the buret with NaOH before filling it d. Presence of air bubble in the pipette that was used to deliver phosphoric acid Q(3): Which of the following statements is Correct Select one: a. Titrant should react completely with the analyte so that satisfactory end points are realized b. The reaction of the analyte with titrant should be slow to allow the detection of the end point c. Equivalence point and end point have the same physical meaning d. In titration of weak acid it is better to use weak base as titrant

Q(2): Which of the following will affect the calculated molarity of phosphoric acid solution when its titrated with standard NaOH to be higher than the correct value? Select one: a. Rinsing the inner wall of the titration flask with distilled water during addition of NaOH b. Rinsing the titration flask with small amount of phosphoric acid c. Rinsing the buret with NaOH before filling it d. Presence of air bubble in the pipette that was used to deliver phosphoric acid Q(3): Which of the following statements is Correct Select one: a. Titrant should react completely with the analyte so that satisfactory end points are realized b. The reaction of the analyte with titrant should be slow to allow the detection of the end point c. Equivalence point and end point have the same physical meaning d. In titration of weak acid it is better to use weak base as titrant

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 57P

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Similar questions

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?
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Sketch the titration curve for a weak base titrated by a strong acid. Weak basestrong acid titration problems also follow a two-step procedure. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong acid (HNO3, for example) reacts to completion with the weak base, B. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak basestrong acid titration? If pH = 6.0 at the halfway point to equivalence, what is the Kb value for the weak base titrated? Compare and contrast the titration curves for a strong basestrong acid titration and a weak basestrong acid titration.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
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
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
explain if this is true or false 1. in the potentiometric titration curve of salicylic acid, the dominating species from the post equivpt are salicylate and hydroxide anions.

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