Answered: 16. A 50.0 mL sample of 0.20 M HNO3 is…

16. A 50.0 mL sample of 0.20 M HNO3 is titrated with 0.10 M NaOH. What is the [H*] in the sample after 25.0 mL of NaOH titrant have been added? а. 0.10 М b. О.20 М с. 0.05 М d. 0.005 M

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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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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In an acid-base neutralisation titration, equivalent quantities of hydronium and hydroxide ions are present Select one: a. At the beginning of the titration b. When the indicator changes colour c. Half way through the titration d. At the equivalence point
SET-1 1. Acids produce; when dissolved in water. a. Na+ ions b. OH ions c. H+ ions d. Cl ions 2. A solution with a pH of 4 is; a. Neutral b. Acidic c. Basic d. Salty 3. H2SO4 is added to the oxalic acid solution before titration with KMnO4 solution to: Speed up reaction a. b. Slow down reaction c. d. Dissolve formed ions Help produce a color at the endpoint. 1. A solution with a pH of 7 is SET-2 a. Neutral b. Acidic c. Basic d. Salty 2. Bases produce;. when dissolved in water. a. Na+ ions b. OH- ions c. H+ ions d. Clions 3. For bases, the following is true. a. [H+] = [OH] b. [H+] > [OH] c. [H+] < [OH] d. [OH-] is zero
Which of the following statements about the equivalence point of an acid-base titration is true? a. The equivalence point of an acid-base titration is the average value of the dissociation constants b. The equivalence point of an acid-base titration is the point where there is an equivalent amount of titrant and analyte c. The equivalence point of an acid-base titration is the same as the indicator endpoint. d. The equivalence point of an acid-base titration is where the pH = 7.0 (neutral).
A 100 mL sample of a 0.300 M solution of a weak monoprotic acid is titrated with 0.150 M KOH. After 100 mL of the KOH solution is added, the pH is 5.24. What will be the pH after another 100 mL of the KOH solution is added? A. 8.82 B. 10.48 C. 8.62 D. 9.12 E. 9.01
According to the titration curve attached, the equivalence point can be found at the following volume of KOH: 14 12 10 8. 9. 4. 0. 10 15 20 25 30 Volume of KOH added (mL) A. 8.00 mL B. 25.00 mL C. None of the above OD. 16.00 mL
17. For each slightly soluble salt, how will the addition of hydrochloric acid affect its solubility? How will the addition of sodium hydroxide affect its solubility? a. AgBr b. Al(OH) c. Ca(OH)₂ d. PbF₂
25). One of your classmates, Chem 109 student said, “I can make a perchlorate buffer using equal amount of 0.1 M HCIO4 and 0.1 M NaCIO4." Will the solution prepared properly by this student functions as a buffer? Another word, can this solution be a buffer? а. yes d. need only ClIO, to make the buffer. c. need only HCIO, to make a perchlorate buffer. e. none of the above b. no
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14 Given the hypothetical titration curves below, determine what curve has a stronger acid. 14 a. b. C. d. 12 10 8 6 4 () 0 Curve A Curve B Curve C Cannot be determined A B and C 10 20 30 40 50 60 Volume of 0.1000 M NaOH, mL
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ANSWER D and how would the rankings change if...
Moving to another question will save this response. uestion 5 In the titration of 0.100 M HNO3 with the titrant 0.100 M KOH, what species are present at any point after KOH has been added but before the equivalence point? a. KOH only b. KNOJ only c. HNOJ and KNO d. HNO3 only e. HNO3 and KOH