A 10.00 mL sample of a solution containing Fe3+ and Co2+ are added to 100 mL...

A 10.00 mL sample of a solution containing Fe3+ and Co2+ are added to 100 mL of pH 4.5 buffer and then titrated to a Cu-PAN endpoint with 17.62 mL of 0.05106 M EDTA. A 25.00 mL sample of the same solution are added to 100 mL of pH 4.5 buffer and then 10 mL of 1 M potassium fluoride are added to mask the Fe3+. This solution was titrated to a Cu-PAN endpoint with 12.44 mL of 0.05106 M EDTA. Calculate the molarity of Fe3+ and Co2+ in the solution.

Expert Solution

queen_honey_blossom answered 2 years ago

A 30.00 mL sample of 0.0100M MgEDTA2- solution was added to a 30.00 mL sample containing...

A 30.00 mL sample of 0.0100M MgEDTA2- solution was added to a 30.00 mL sample containing Fe3+. The solution was then buffered to pH 10 and titrated with 12.83 mL of 0.0152 M EDTA to an Eriochrome Black-T endpoint. What was the [Fe3+] in the original sample? Please show work.

In the experiement, each flask containing a water sample, pipette 10.00 mL of the AgNO3 solution....

In the experiement, each flask containing a water sample, pipette 10.00 mL of the AgNO3 solution. Using a small graduated cylinder, carefully add 3.0 mL of Fe(NO3)3 solution and 2.0 mL of 6M HNO3 to each water sample. the trial is now ready for titration. Obtain approximately 120 mL of stock KSCN solution. Rinse out a clean buret with about 10 mL of KSCN at least twice, and discard the washing solution into a waste beaker. From the calculation , number...

A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was...

A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Calculate the fraction (αY4-) of free EDTA in the form Y4−. Keep 2 significant figures.

For the titration, 10.00 mL of a 2.00 M hydroiodic acid solution was added to a...

For the titration, 10.00 mL of a 2.00 M hydroiodic acid solution was added to a beaker. The buret was filled with a 0.500 M barium hydroxide solution. What is the pH of the solution if 10.00 mL of the base were added? (0.301 but why?) What is the pH of the solution if 20.00 mL of the base were added? What is the pH of the solution if 30.00 mL of the base were added?

How many milliliters of 1.27 M KOH should be added to 100. mL of solution containing...

How many milliliters of 1.27 M KOH should be added to 100. mL of solution containing 10.0 g of histidine hydrochloride (His·HCl, FM 191.62) to get a pH of 9.30?

Consider the titration of a 50.00 mL aliquot of a water sample containing Fe3++ and Pb2++...

Consider the titration of a 50.00 mL aliquot of a water sample containing Fe3++ and Pb2++ with 19.62 mL of 0.00243 M EDTA to reach the end point. Excess CN- was added to a separate 20.00 mL aliquot of the same water sample, causing Fe(CN)3 to precipitate. This aliquot was titrated with 2.01 mL of 0.00243 M EDTA to reach the end point. What is the molarity of Fe3+ in the water sample? Please explain every step. Thank you.

21.83 mL of a Pb2 solution, containing excess Pb2 , was added to 10.75 mL of...

21.83 mL of a Pb2 solution, containing excess Pb2 , was added to 10.75 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2 –BAL complex. The excess Pb2 was titrated with 0.0141 M EDTA, requiring 8.86 mL to reach the equivalence point. Separately, 40.70 mL of the EDTA solution was required to titrate 31.00 mL of the Pb2 solution. Calculate the BAL concentration, in molarity, of the original 10.75-mL solution.

A solution containing 45.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was...

A solution containing 45.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Answer the following questions and enter your results with numerical value only. Calculate the equivalence volume, Ve, in milliliters. Calculate the concentration (M) of free metal ion at V = 1/2 Ve. Calculate the fraction (αY4-) of free EDTA in the form Y4-. Keep 2 significant figures. If the formation constant (Kf) is 1012.00. Calculate the value of the...

10.00 ml of seawater containing Mg2+ ions is determined by precipitation with an oxalate (C2O42-) solution....

10.00 ml of seawater containing Mg2+ ions is determined by precipitation with an oxalate (C2O42-) solution. Mg2+ + C2O42- <> MgC2O4 The precipitate was filtered, redissolved, and titrated to endpoint requiring 18.21 ml of a standard MnO4-. Beforehand, the MnO4- solution was standardized with 10.00 ml of a 2.00 * (10)-3 M oxalate solution and required 32.10 ml of MnO4- solution. Calculate the concentration of Mg2+ in the seawater sample. 2 MnO4- + 5 C2O42- + 6H+ ==> 10 CO2...

If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which...

If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which is 0.20M in NH3 and 0.18M in NH4Cl, what will be the pH of the new solution? The Kb of NH3 is 1.8x10^-5. Please explain how the answer was obtained. Thank you!

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