2. 25.00 mL of 0.05600 M Fe" is made up in a solution that is buffered at pH 7.50. Oxalate is added as an auxiliary complexing agent to keep Fe(OH), from precipitating. The oxalate ion is adjusted so that it's free concentration is 0.250 M. The solution is titrated with a 0.02414 M solution of EDTA. How many mL of EDTA solution are required to reach the equivalence point in the titration? ve = 25,00 0.0 S600 58.00 mL O.02414 b. Calculate a„t- at this pH. Calculate a. for the solution. C.

2. 25.00 mL of 0.05600 M Fe" is made up in a solution that is buffered at pH 7.50. Oxalate is added as an auxiliary complexing agent to keep Fe(OH), from precipitating. The oxalate ion is adjusted so that it's free concentration is 0.250 M. The solution is titrated with a 0.02414 M solution of EDTA. How many mL of EDTA solution are required to reach the equivalence point in the titration? ve = 25,00 0.0 S600 58.00 mL O.02414 b. Calculate a„t- at this pH. Calculate a. for the solution. C.

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

Write an overall net ionic equation and calculate K for the reaction where Co(OH)2(Ksp=21016) is dissolved by HCI.
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?
Determine the molar solubility (?) of Ag2CO3 in a buffered solution with a pH of 5.887 using the systematic treatment of equilibrium. ?sp(Ag2CO3) = 8.46×10−12; ?a1(H2CO3) = 4.45×10−7; ?a2(H2CO3) = 4.69×10−11. S = ? M
A sample containing phosphorus weighs 4.2580g. The phosphorus in the sample is converted into phosphate ion and precipitated as silver phosphate through the addition of 50mL of 0.0820M of silver nitrate. The excess silver nitrate was back titrated with 4.06mL of 0.0625M of potassium thiocyanate. Calculate the % phosphorus pentoxide in the sample.
It is desired to determine the concentration of chlorides in a powdered milk following the method of Volhard, for such case 1.5g of milk is weighed, it is heated in a muffle until obtaining ashes, which are treated with acid water with some drops of HNO3, the solution is filtered and the obtained filtrate is collected in an Erlenmeyer and 20 mL of AgNO3 0 is added. 1M excess silver is titrated with 0.05M potassium thiocyanate, if 8 mL of KSCN has been used up at the time of the indicator turn. Calculate the % of chloride in the milk powder.
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.
0.3g of MBr is dissolved in distilled water to make 250mL in a standard flask. 25 mL ofthis is titrated with suitable indicator against 0.02 M silver nitrate solution and the end point was obtained at 12.8 mL of AgNO3 solution. Calculate the RMM of the metal bromide.
0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???
Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M NaHCO3
A 25.00 mL solution of 0.08960 M NaI is titrated with 0.05040 M AgNO3. Calculate pAg+ following the addition of the given volumes of AgNO3. The ?sp of AgI is 8.3×10−17 .35.20 mLpAg+= ?epAg+= 46.40 mLpAg+=
Aluminumcan form two complex ions with fluoride, AlF63–(Kf= 2.4x10^4), which forms in solutions with [F–] > 1.5M and AlF4–(Kf= 2.0x10^8), which forms when [F–] is between 0.5 M and 1.5M. 100 mL of 0.20 M Al(NO3)3is combined with 500 mL of a pH 4.25 HF/NaF buffer (total concentration of 2.0M). Given that the sodium salt of the complex ion has a solubility of 0.042 g/100 mL, will the sodium salt precipitate from the equilibrium mixture? Why or why not? If AlF63–forms, the sodium salt would be Na3AlF6; if AlF4–forms, the sodium salt would be NaAlF4.
A stainless steel alloy is to be analyzed for its chromium content. A 3.30 g sample of the steel is used to produce 250.0 mL of a solution containing Cr2O72−. A 10.0-mL portion of this solution is added to BaCl2(aq). When the pH of the solution is properly adjusted, 0.145 g BaCrO4(s) precipitates. A.) What is the percent Cr, by mass, in the steel sample? Express your answer numerically as a percentage.