Which of the following statements regarding complexometric titrations is incorrect ? OIn the pH range 3-10 the predominant species are H2Y2 and HY3- O The higher the ammonia concentration, the less sharper the end point for the EDTA-Zn2* complex. O EDTA is a hexaprotic acid. O a4 value is proportional to the pH value. O The larger the formation constant for the EDTA-metal complex, the sharper the end point.

Which of the following statements regarding complexometric titrations is incorrect ? OIn the pH range 3-10 the predominant species are H2Y2 and HY3- O The higher the ammonia concentration, the less sharper the end point for the EDTA-Zn2* complex. O EDTA is a hexaprotic acid. O a4 value is proportional to the pH value. O The larger the formation constant for the EDTA-metal complex, the sharper the end point.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.25QAP

See similar textbooks

Similar questions

A 0.125-M solution of 0.075 Mn(NO3)2 is saturated with H2S([H2S]=0.10M). At what pH does Mns begin to precipitate?. MnS(s)Mn2+(aq)+S2(aq)Ksp=4.31022 H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
Calculate the equilibrium Ni2+ concentration of a solution that has beenprepared by mixing 50.0 ml of Ni2+ 0.030 mol / L with 50.0 ml of EDTA0.050 mol / L. The mixture was buffered to pH 3.0. Kf= 4.2 x 1018 , alfa4= 2.6x10-11
Calculate the molar solubility of Ni(OH)2 (Ksp = 2.0 × 10-15) in a solution which is buffered at pH = 9.75. Enter your answer as scientific notation with the correct number of sig figs. Use the #e# format.
Chloride in a brine solution is determined using Volhard method. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the (a) indicator (b) end point color (c) molarity of the Cl- in sample.
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.
Calculate the concentration of Fe2O3 in a mineral sample after solubilization of 0.4891g and availability of Fe as Fe2+. The released Fe2+ ions were titrated with a 0.02153 mol/L K2Cr2O7 solution requiring 36.92 mL to reach the end point of the titration. Show the calculations and express the concentration in % m/m. K2Cr2O7; + 6Fe2+ + 14H+ → 2Cr+3 + 2K+ + 6Fe3+ + 7H20
The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?
If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
A 1.000g sample of unknown Fe+2 content is titrated with potassium permanganate. The final color change is attained when 25.00 mL of 0.0300M potassium permanganate is added to the unknown Fe+2 sample. What is the mass percent of Fe in the sample?
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.
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?