All of the following regarding Argentometric titration are correct except: a. Chromate indicator is used in Mohr method b. Greater values of Ksp give sharper break and inflection at end point c. Increasing reagent concentration makes the change in pAg larger. d. Volhard's method involves adding excess AgNO, to the analyte, then back titration with standard SCN solution. e. Fajan's method depends on adsorption of fluorescence indicator on the colloidal precipitate formed Please fill in the space with one of the following characters (a or b or c or d or e)
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- 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.one of the following is not correct about Volhard method: a. Ksp of silver thiocyanate is less than Ksp of silver chloride b. you can filtrate the precipitate before carrying out titration to the liquor c. relies on back titration d. silver chloride precipitate can be isolated by methanolDetermine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided Determination of water hardness using complexometric titration. During sample analysis (ppm CaCO3), the volume for blank correction was not subtracted to the volume of titrant. EX Blank 1 ET
- 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.A small amount of Mg-EDTA is often added in the titrimetric determination of water hardness. Why? A. Mg forms the most stable EDTA complex of all multivalent cations. B. It ensures that enough Mg ions are present for satisfactory indicator action. C. Mg-EDTA is inert and therefore does not influence the results, but it enhances indicator action.D. The Mg-EDTA dissociates after all the other cations have been titrated and therefore ensures that the end point is clearly visible.Which are TRUE for the use of indicators with dichromate? I Dichromate is orange and changes color to green when reduced. The color change is abrupt enough to serve as an indicator.II The equivalence point for dichromate can be determined using Pt and calomel electrodes.III Dichromate end points are determined using the distinct color changes of diphenylamine sulfonic acid or diphenylbenzidine sulfonic acid indicators.IV In basic solution, the orange dichromate solution changes color to yellow when reduced to chromate anion. The color change is abrupt enough to serve as an indicator. A. I and III B. II and III C. I and IV D. II and IV E. I, II, and IV
- 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 reagentYour 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?1. A process where impurity is precipitated along with the desired product. 2. Calculate the gravimetric factor for: Analyte: SiO2 Precipitate: KAlSi3O8
- Which of the following is a good description of a standard solution as a titrant? a) selectively reactive with the analyte b) only reacts with the matrix c) oxidize when exposed to air d) reacts very slowly but completelyThe Kjedahl procedure was used to analyze 256 µL of a solution containing 37.9 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.033 6 M HCl, and the remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the weight percent of nitrogen in the protein? wt%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.