Bromocresel Green v Volame of ratienPhenclphthalein vs Volume of titration 2EIS7.959.510.5Valume af titration 1 vellVolume of titratien 2 voFor which titration is phenolphthalein the best choice? Explain your reasoning and support withevidence from your graphs Be specific!- For which titration is bromocresol green the best choice? Explain your reasoning and support withevidence from your graphs Be specific!- Consider one of the graphs you made of the pH of a titration. The curve is less steep (flatter) at verylow volumes of titrant added and again at very high volumes of titrant added. Explain why.Bromocresol greenYellow to blue during weakacid to strong base(5 70 pH,9.8 mL), blue to yellow duringweak base to strong acid( 3.57Bromocresol GreVolume of titratiPhenolphthaleinVolume of titratiunitsvariablevolvariableunitsvariablevolvariable5.709.88.1510.4pt, 8.1 mL).3.578.17.787.43PhenolphthaleinClear to pink during weak acidto strong base (8.15 pH, 10.4ml), pink to clear during weakbase to strong acid (178pH,7.4 mL)45igun u udjouou42.

Titration is a technique in which a solution of known concentration is treated with a solution of…

For which titration is phenolphthalein the best choice? Explain your reasoning and support with evidence from your graphs Be specific! For which titration is bromocresol green the best choice? Explain your reasoning and support with evidence from your graphs Be specific!

For which titration is phenolphthalein the best choice? Explain your reasoning and support with evidence from your graphs Be specific! For which titration is bromocresol green the best choice? Explain your reasoning and support with evidence from your graphs Be specific!

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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Answer the following question. DRAW THE TITRIMETRIC PROFILE for better understanding
Which one of the following is NOT a source of error during a titration? Group of answer choices Adding too much sodium hydroxide solution to the analyte Refilling the buret during a titration trial Rinsing the buret with the analyte Adding indicator to the analyte
i) How many moles of hydrochloric acid were there in the volume of acid added in the titration? ii) How many moles of calcium hydroxide were there in the 25 cm sample of solution that the student used in the titration? iii) What was the concentration of the calcium hydroxide solution in mol/dm?
Incorrect Your answer is incorrect. • KC: Your answer is incorrect. • Cacl, Vour answer is incorrect. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll ind K, data in the ALEKS Data tab. Does enlubility change with pH? hiyhest solubility compound pll 5 pll 6 pll 8 yes O no yes Ba(OH), O no O yes Caci, e no
Hatsume Mei wanted to maintain the pH of a certain solution within a specified range. What should she use to accomplish this? Analyte Titrant Standard Buffer
1- Give the solubility class and the possible types of compounds for the solubilities listed below. a. The unknown compound was insoluble in water, 5% NaOH, and 5% HCI, but soluble in 96% H₂SO4, b. The unknown compound was soluble in water and ether and was unchanged with litmus. c. The unknown compound was insoluble in water and 5% NaHCO3, but soluble in 5% NaOH.
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
A local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 50.00 mL sample and found that you needed 33.20 ml NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) Purity NaOH (mL) used Determine the following: 0.8053 g Volume of sample 50.00 mL 99.80% NaOH (mL) used 33.20 mL 40.60 mL a. Molarity of NaOH b. % (w/v) acetic acid
30.0 mL of a 0.20 M solution of the weak base methylamine is titrated with 0.10 M nitric acid (HNO3). The Kb of methylamine can be found in Appendix I. Calculate the pH at each volume of base addition as listed below and report your answer to two decimal places The initial pH (after 0.0 mL of nitric acid addition) is The pH after 10.0 mL of nitric acid addition is The pH after 30.0 mL of nitric acid addition is The pH after 60.0 mL of nitric acid addition is The pH after 65.0 mL of nitric acid addition is
What is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. OKOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.
Standardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?
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…