Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12 11- 11- 10- 10- 9- 9- 8- 8- 7- 7- 6- 6- 5- 5- 4- 3- 3- 2- 2 1 10 15 20 25 30 35 40 45 50 10 15 20 25 30 35 40 45 50 Titrant.volume Cml). .Titrant.volume (mL). Answer Bank This graph does not represent a titration. a basic solution titrated with an acid an acidic solution titrated with a base Hd Hd

Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12 11- 11- 10- 10- 9- 9- 8- 8- 7- 7- 6- 6- 5- 5- 4- 3- 3- 2- 2 1 10 15 20 25 30 35 40 45 50 10 15 20 25 30 35 40 45 50 Titrant.volume Cml). .Titrant.volume (mL). Answer Bank This graph does not represent a titration. a basic solution titrated with an acid an acidic solution titrated with a base Hd Hd

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.13QAP

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Title: Potentiometric Acid Titration fitulo:Tabla de ph volumen NaOH (ml) ph Titulación NaOH 20 4.25 7.39 20.1 6.24 7.03 7.21 6.83 6.59 20.2 6.59 6.24 20.3 6.83 6 20.4 7.03 4.25 20.5 7.21 20.6 7.39 1 19.9 20 20.1 20.2 20.3 20.4 20.5 20.6 20.7 V NAOH (ml) With the previous graph determine the following: a. Determine the bufer zone on the graph b. Determine the volume at the stoichiometric point of the acid titration c. Determine the average volume d. Use the medium volume to get the pka e. From pka, get the value of ka
Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.55 49.43 49.99 Expected color at end point Volume of NaOH used (mL) Average Volume of NaOH used in liters Average moles of NaOH used (mol) Average moles of acetic acid (mol) Average molarity of acetic acid (M) Average mass of acetic acid (g) Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL) Average mass % of acetic acid in vinegar Known mass % of acetic acid in vinegar is 5.45% Percent Error
2. Below is a titration curve generated by a similar titration to the ones simulated, Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 * 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL) We can use this curve to estimate the pka of our weak acid by what is called the "half equivalence point method". The equivalence point is the middle of the steepest part of this graph. Estimate the volume of NaOH added to the titration at that point by using a rule or other straight edge to follow that point down to the x-axis. Divide that volume by 2 (half the equivalence point) and estimate the pH at that volume of NaOH using your straight edge again. pKa = pH at the half equivalence point. What do you estimate the pka to be? 3. The pka of acetic acid is 4.76. Calculate percent error between the true value and your estimated value from question 2.
A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm in a beaker. Add the solution of A to a burette. Titrate the solution of A with a standard solution of sodium hydroxide, NAOH. (a) What is meant by the term standard solution? (b) Sodium hydroxide is an alkali. What is meant by the term alkali? (c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 27
Reductant/ Analyte Standardizing Indicator reagent Titration Titrant Oxidant COD BOD INDIRECT TITRATION
Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (ml) Volume titration 2, (mL) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (mL) Standard deviation Unrounded value Rounded value
Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 49.32 49.06 49.93 Table 2. Titration data Table view List view Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 49.32 49.06 49.93 Expected color at end point Choose... Choose... Choose... Volume of NaOH used (mL) 1. Average Volume of NaOH used in liters 2. Average moles of NaOH used (mol) 3. Average moles of acetic acid (mol) 4. Average molarity of acetic acid (M) 5. Average mass of acetic acid (g)…
The titration of 5.00 mL of 0.4949 M NH3 with 0.2250 M HNO3. Kb = 1.8×10–5. Fill out chart and list possible indicator. Volume HNO3 (mL) Calculated pH 1 initial 0.00 2 ¼ way to eq. point 3 ½ way to eq. point 4 ¾ way to eq. point 5 0.5 mL before eq. point 6 equivalence point 7 0.5 mL after eq. point 8 well past eq. point 15.00
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
Make a potentiometric titration graph and the first and second derivatives to determine the equivalence point of the following data 1* derv Vavecage 2nd derv Vaverase. Vol titrant PH A pH AV. A² pH AV² (ml) 10.679 7.643 10.696 7.447 10.713 7.091 10.721 6.700 10.725 6.222 10.729 5.402 10.733 4.993 10.738 4.761 10.750 4.444 10.765 4.227
Titration is the addition of a chemically equivalent volume of a solution of known concentration called analyte titrant fluent None of them
You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Final Vol Delivered |(mL) Burette Burette Reading (mL) Reading (mL) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units. Answer: