Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. adding titrant past the color change of the analyte solution recording the molarity of titrant as 0.1 M rather than its actual value of 0.01 M spilling some analyte out of the flask during the titration starting the titration with air bubbles in the buret filling the buret above the 0.0 mL volume mark Answer Bank no effect too low too high 7

Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. adding titrant past the color change of the analyte solution recording the molarity of titrant as 0.1 M rather than its actual value of 0.01 M spilling some analyte out of the flask during the titration starting the titration with air bubbles in the buret filling the buret above the 0.0 mL volume mark Answer Bank no effect too low too high 7

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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Using the letters on the image, identify each component of the titration set-up. Buret clamped to a ring stand with a beaker underneath. The letter A appears at the top of the buret, the letter B appears midway down the buret, the letter C appears at the bottom of the buret, the letter D appears next to the beaker, and the letter E appears on the other side of the buret, near the ring stand.
• An unknown acid (HA) was titrated with NaOH(aq). • The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 2. 4 9. 8. 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Which of the following net ionic equations explains the pH of the analyte solution before any titrant is added? A (aq) + H20(1) HA(aq) + OH (aq) A (aq) + H3O*(aq) --> HA(aq) + H20(1) O H*(aq) + OH (aq) H20(1) --> O HA(aq) + OH (aq) --> H2O(aq) + A (aq) HA(aq) + H20() H3O*(aq) + A (aq)
A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0345 Trial 2 0.0334 Trial 3 0.0381 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.
Volumetric Analysis In Part A, a drop of the NaOH titrant adheres to the side of the buret (because of a dirty buret) between the initial and final readings for the titration. As a result of the “clean glass” error, how will the calculated molar concentration of the NaOH solution be affected?
Analytical Chemistry. Identify the most appropriate class (based on purity) of chemical/reagent that will be used in the following.
Four millimoles of pure sodium chloride was dissolved in 100 ml water and analyzed according to the Mohr method. Calculate the ionic strength at the endpoint, the solubility products of silver chloride and silver chromate at this ionic strength, and the titration error. (The answers are respectively: 0.0350, 2.6 x 10−10, 1.2 x 10−11, +0.10 ml)
30. Indicate the FALSE statement about pH indicators and their use in titrations: A) A pH indicator suitable for titrations of strong bases with strong acids cannot be used for titrations of strong acids with strong bases. B) pH indicators should be used sparingly (in small amounts) as they are weak acids/ bases, and thus could affect the volume of titrant used. C) An indicator should be selected such that its pKits value matches the equivalence point pH. D) pH indicators all contain at least one acidic group that can be deprotonated to form a differently colored conjugate base. E) The colours of the acid and base forms of a given pH indicator depend on their chemical structures.
Data for the titration of 100.00 mL of a weak acid by NaOH are given in the table. Find the end point by preparing a Gran plot, using the last 10% of the volume prior to Ve. mL NaOH 0.00 1.31 2.34 3.91 5.93 7.90 11.35 13.46 15.50 16.92 18.00 18.35 18.95 19.43 19.93 20.48 V₂ = pH 4.14 4.30 4.44 4.61 4.79 4.95 5.19 5.35 5.50 5.63 5.71 5.77 5.82 5.89 5.95 6.04 mL NaOH 20.75 21.01 21.10 21.13 21.20 21.30 21.41 21.51 21.61 21.77 21.93 22.10 22.27 22.37 22.48 22.57 pH 6.09 6.14 6.15 6.16 6.17 6.19 6.22 6.25 6.27 6.32 6.37 6.42 6.48 6.53 6.58 6.63 mL NaOH 22.70 22.76 22.80 22.85 22.91 22.97 23.01 23.11 23.17 23.21 23.30 23.32 23.40 23.46 23.55 pH 6.70 6.74 6.78 6.82 6.86 6.92 6.98 7.11 7.20 7.30 7.49 7.74 8.30 9.21 9.86 mL
Explain how the calculation of the molar solubility will be affected if a small amount of the sample adhering to the side of the flask was left unreacted when the end point was thought to have been reached. Procedure: Pipet 25 mL of the saturated Ca(OH)2 solution (without added CaCl2) into a 125 mL flask and add 2 drops of methyl orange indicator. Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Titrate two additional 25 mL aliquots of the saturated Ca(OH)2 solution
2b
Thank you! Data included in pictures! No hand drawn graphs!! Determine the equivalence point and the endpoint of the sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 3: Titration of Sudsy Ammonia with 0.25 M Citric Acid Data with the Chosen Indicator. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Draw a blue arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your endpoint. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration data in Question 9. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental…
A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.200 + x] [0.175 + x] [0.200] [0.200 -x] [0.175 -x] 0 1.70 Kb 4.77 x 10-1⁰ = 12.3 [0.0200] [0.100] [0.0200 + x] [0.0200 -x] 10.8 [0.140] 2 [0.100 + x] 2.10 x 10-² A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the…