Identify the type of titration method. Choose the best answer can be carried out at low pH or extremely acidic conditions makes use of adsorption indicators ✓the indicator reaction produces a reddish- brown precipitate forms complex with EDTA ✓requires a second titrant for back-titration indicator can either be potassium chromate or sodium chromate ✓ The indicator dye turns the sample into a greenish-yellow solution and turns pink when dye is adsorbed on ppt A. Fajan B. Volhard C. None of the above D. Mohr

Identify the type of titration method. Choose the best answer can be carried out at low pH or extremely acidic conditions makes use of adsorption indicators ✓the indicator reaction produces a reddish- brown precipitate forms complex with EDTA ✓requires a second titrant for back-titration indicator can either be potassium chromate or sodium chromate ✓ The indicator dye turns the sample into a greenish-yellow solution and turns pink when dye is adsorbed on ppt A. Fajan B. Volhard C. None of the above D. Mohr

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...

See similar textbooks

Similar questions

If a 25.00 ml aliquot of a solution containing sulfide ions was added to 25.00 ml of 0.0103 M Cu2+ solution. The CuS precipitate was washed and collected. The pH of the combined filtrate and washings was then adjusted by the addition of ammonia and the solution was titrated with 0.01453 M EDTA, using a suitable indicator. The endpoint volume was found to be 12.20ml. Find the molarity of the sulfide in the sample solution.
An aqueous solution of 0.2100 g of a mixture containing potassium cyanide and potassium chloride required 14.56 mL of 0.1000 M silver nitrate to produce a faint permanent turbidity; 30.00 mL more of the silver nitrate was added (an excess) and the precipitate of AgCl and AgCN filtered off from the solution. The filtrate and washings were titrated with 13.06 mL 0.1000 M thiocyanate solution. Calculate the percentages of KCl and KCN in the sample.
Your titration experiment included phosphoric acid, liqid starch, and Iodine-Potassium-Iodide (IKI) solution. The following information is given: iodine is too weakly colored to act as an effective primary indicator, but it is enhanced by its interaction with stach in a solution. The secondary indicator you will use in this experiment is iodine-starch complex. Iodine-potassium-iodide is the titrant. What acted as the primary indicator in this experiment? The secondary indicator? What was the role of the phosphoric acid? What would happen if you forgot to add it, or added a base instead?
An auxiliary competing agent is used in EDTA titrations to slow down the titration. keep some interfering component of the analyte mixture from complexing with the EDTA. speed up the titration. keep the metal ion from precipitating out of the solution.
A 2.054 g of macrogol monostearate (average molecular weight 706. 5) was added to a 200 ml flask and 25 ml of an ethanolic solution of potassium hydroxide (molecular weight 56.1, ca 0.5 M) was added. The sample was heated under a reflux condenser for 1 hour. The excess of alkali was then titrated with 0.5016 M hydrochloric acid using phenolphthalein solution as an indicator. The operation was repeated without the macrogol monostearate. Results Volume of HCI required to titrate the excess alkali = 18.35 ml Volume of HCI required to titrate the blank = 24.03 ml Calculate the saponification value for the macrogol stearate. Answer: Blank mg/g
Accurately weigh out about 6g copper(ii) sulfate crystals into a weighing boat. Use the copper(ii) sulfate crystals to make up 250cm3 of standardized copper (ii) sulfate solution Pipette 25cm3 of this solution into a conical flask Add 1.5g potassium iodide and swirl thoroughly Titrate this solution with standard 0.1 moldm-3 Na2S2O3 in a burette. When the iodine color fades, add 1 cm3 starch indicator. Use your titration data below to calculate the percentage by mass of copper in the copper(ii) sulfate crystals.
1. These are balances that have a maximum loading of 10 to 30 g with a precision of 60.01 mgA. semi-microanalyticalB. MicroanalyticalC. MacrobalancesD. Triple Beam Balance2. Which type of curve is normally produced when plotting the change in the concentration of a specie of some function and the amount of reagent added?A. Titration curveB. Sigmoidal CurveC. Phase Transition curveD. Calibration curve3. In the dead dear case study, silver diethyldithiocarbamateforms a colored solution when it binds with arsenic, what do we call substance like silver diethyldithiocarbamate?A. Secondary standard reagentB. Precipitating agentC. Chelating agentD. Primary standard reagent
10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)
The concentration of the sodium hydroxide titrant is determined with the use of KHP as primary standard because KHP is: a. is a low molecular weight substance b. readily absorbs atmosphere moisture c. comes in a highly concentrated form d. is non hygroscopic
A fish sample was analyzed for crude protein content using the Kjeldahl method. Thefollowing data were recorded: Moisture content 10.0%Weight of sample 2.15 gNormality of HCl used for titration 0.121 NHCl used for sample 28.5 mLHCl used for reagent blank 0.2 mL Calculate crude protein content on wet weight basis of the fish sample, assuming fishprotein contains 20% nitrogen.
I have gotten this wrong 8 times! Please help. See screenshot attached. Thank you! A solution containing a mixture of metal cations was treated as outlined. Dilute HClHCl was added and a precipitate formed. The precipitate was filtered off. H2SH2S was bubbled through the acidic solution. No precipitate formed. The pH was raised to about 9 and H2SH2S was again bubbled through the solution. A precipitate formed and was filtered off. Finally, sodium carbonate was added to the filtered solution and no precipitate formed. What can be said about the presence of each of these groups of cations in the original solution?
Which is CORRECT? a. EDTA has 2 oxygen sites and 2 nitrogen sites that are electron rich. b. At pH = 10, fraction of fully deprotonated form of EDTA approaches to 1. c. EDTA titrations that are carried out beyond pH 10 typically involves the use of auxiliary reagents. d. As long as EDTA titrations are carried out beyond pH 10, we are sure that all of the analyte will react completely with EDTA.