Which of the followingstatements regardingcomplexometric titrations isincorrect ?O The larger the formationconstant for the EDTA-metal complex, thesharperthe end point.O a4 value is proportional tothe pH value.O EDTA is a hexaprotic acid.O In the pH range 3-10 thepredominant species areH2Y2- and HY3-O The higher the ammoniaconcentration, the lesssharper the end point fortheEDTA-Zn2+ complex.

Titration is of 4 types :- 1) acid -base titration 2) redox titration 3) precipitation titration 4)…

Which of the following statements regarding complexometric titrations is incorrect ? O The larger the formation constant for the EDTA- metal complex, the sharper the end point. a4 value is proportional to the pH value. O EDTA is a hexaprotic acid. O In 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.

Which of the following statements regarding complexometric titrations is incorrect ? O The larger the formation constant for the EDTA- metal complex, the sharper the end point. a4 value is proportional to the pH value. O EDTA is a hexaprotic acid. O In 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.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter11: Solving Equilibrium Problems For Complex Systems

Section: Chapter Questions

Problem 11.16QAP

See similar textbooks

Similar questions

If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint
If 175 mL of a 0.0208 M AgNO3 solution is added to a 250 mL 0.0380 M K2CrO4, will Ag+ precipitiate completely?
Calculate the ratio of [Ca2+ ] to [Fe2+ ] in a lake in whichthe water is in equilibrium with deposits of both CaCO3 and FeCO3. Assume that the water is slightly basic andthat the hydrolysis of the carbonate ion can, therefore, beignored.
The ksp of NiCO3 is 6.6x10-9 @ a certain temperature. If 5.0 mL of1.7x10-5M Ni2+ ions were added to 5.0 mL of 0.0010M CO32 ions, will a precipitateform?
If 175ml of a 0.00550 M KCI solution is mixed with 145ml of a 0.00150M AgNO3 solution,will AgCl (Ksp=1.77 x 10-10) precipitate?
Consider the reaction Agl <-> Ag+ + I- What will happen to the solubility of the salt if the solvent is at pH 4.5? (It will increase, decrease, or not change?) What will happem to the solubility of the salt if Ag+ forms a complex with NH3 in the solution? (It will increase, decrease, or not change?)
Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch equation to provide a recommendation for a suitable acete/acetic acid buffer under the following reaction conditions. a) If a checial reaction produces hydroxide ion, OH-, what would be the range for the target pH of a buffer soution that would favor pH stabilizatoin under these conditions? Explain.
Silver chromate, AgCrO has a K = 9.010. When added to a 3.14E0 M KCrO(aq) solution, what molar concentration of Ag ions are necessary to reach the saturation point for AgCrO?
10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
We received 15000 Ci of 28Mg, present as Mg(NO3)2 and want to dissolve is in 10 mL water at pH 8. Will we form a precipitate or will the solid entirely dissolve?
A solution contains three anions with the followingconcentra t i o n s : 0.20 M CrO42 - , 0.10 M CO32 - , and0.010 M Cl-. If a dilute AgNO3 solution is slowly added tothe solution, what is the first compound to precipitate:Ag2CrO4 (Ksp = 1.2 x 10-122, Ag2CO3 (Ksp = 8.1 x 10-12 ),or AgCl (Ksp = 1.8 x 10-10 )?
If a solution contained Fe3+ ions at a concentration of 0.1 M, what pH would have to be reached toprecipitate 99% of the Fe3+ as Fe(OH)3?Hint: Determine [Fe3+] after precipitation and use it and the Ksp todetermine [OH-]