Which of the following statements regarding complexometric titrations is Incorrect?O EDTA is a tetroprotic acidO The larger the formation constant for the EDTA-metal complex, the sharper the endpointO Q, value is proportional to the pH valueO In the pH range 3-10 the predominant species is YO The higher the ammonia concentration, the less shorper the end point for theEDTA-Zn complex

Complexometric titrations are used for the determination of various metals like Ca, Mg, Pb, Zn, Al,…

Which of the following statements regarding complexometric titrations is Incorrect? O EDTA is a tetraprotic acid O The larger the formation constant for the EDTA-metal complex, the sharper the endpoint O Q4 value is proportional to the pH value O In the pH roange 3-10 the predominant species is Y O The higher the am menia concentration the less sharnar the and point for th

Which of the following statements regarding complexometric titrations is Incorrect? O EDTA is a tetraprotic acid O The larger the formation constant for the EDTA-metal complex, the sharper the endpoint O Q4 value is proportional to the pH value O In the pH roange 3-10 the predominant species is Y O The higher the am menia concentration the less sharnar the and point for th

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.25QAP

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0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). At what volume (in mL) of EDTA added will the equivalence point be reached?
Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.
Determinethe concentration of an EDTA solution given that a 20.00 mLsample of 0.02491M Zn2+was titrated with37.84mL of EDTA
Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of these
Determine the molar solubility ( ? ) of Ag2CO3 in a buffered solution with a pH of 5.835 using the systematic treatment of equilibrium. ?sp(Ag2CO3)=8.46×10−12 ; ?a1(H2CO3)=4.45×10−7 ; ?a2(H2CO3)=4.69×10−11 .
A 0.2420 g sample cntg. Calcium is dissolver and the metal precipitated as CaC2O4. The ppt. is filtered, washed and redissolved in acid. The pH is adjusted, 25 ml of 0.0400 M EDTA added and the xcss EDTA titrated with 33.28 ml of 0.012102 M MG2+. Calculate the % Ca (40.078) in the sample.
A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.
The phosphate in a 3.00 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO₃ (169.87 g/mol). The solution was filtered and the filtrate, upon addition of 1.00 mL of 0.01 M FeCl₃, required 18.23 mL of 0.1377 M KSCN for titration to the endpoint. Identify (a) what type of precipitation titrimetry was used (b) which served as the indicator (c) the color at the end point Calculate (d) the weight percent of phosphate (94.97 g/mol) in the detergent.
For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g, necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 27.4mL of 0.0097 M EDTA solution. Calculate the amount of calcium in the sample in terms of% CaCO3. (Ca = 40 g / mol, CaCO3 = 100g / mol)
Calculate [Cr3 + ] in equilibrium with Cr(OH)4-(aq) when0.010 mol of Cr(NO3)3 is dissolved in 1 L of solution bufferedat pH 10.0.
In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?
What is the molar solubility of Ag2CO3 in an aqueous solution that is buffered to a pH of 2.37? Relevant constants: Ksp for Ag2CO3 = 8.1 x 10-12; K1 H2CO3 = 4.45x10-7; K2 for HCO3- = 4.69x10-11; Kw = 1.00x10-14.