Question

A 50.0-mL solution containing Ni2+ and Zn2+ was treated with 25.0 mL of 0.0452 M EDTA...

A 50.0-mL solution containing Ni2+ and Zn2+ was treated with 25.0 mL of 0.0452 M EDTA to bind all the metal. The excess unreacted EDTA required 12.4 mL of 0.0123 M Mg2+ for complete reaction. An excess of the reagent 2,3-dimercapto-1-propanol was then added to displace the EDTA from zinc. Another 29.2 mL of Mg2+ were required for reaction with the liberated EDTA. Calculate the molarity of Ni2+ and Zn2+ in the original solution.

Homework Answers

Answer #1

Total moles of EDTA used initially to bind Ni2+ and Zn2+ = 0.0452 M x 25 ml = 1.13 mmol

Excess EDTA present = 0.0123 M x 12.4 ml = 0.15 mmol

Total moles of EDTA reacted with Ni2+ and Zn2+ = 1.13 mmol - 0.0123 M x 12.4 ml = 0.98 mmol

moles of EDTA complexed with Zn2+ = 0.0123 M x 29.2 ml = 0.36 mmol

moles of EDTA complexed with Ni2+ = 0.98 - 0.36 = 0.62 mmol

Molarity of Zn2+ in the original solution = 0.36 mmol/50 ml = 0.0072 M

Molarity of Ni2+ in the original solution = 0.62 mmol/50 ml = 0.0124 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.03828 M EDTA solution. The solution is then back titrated with 0.02192 M Zn2 solution at a pH of 5. A volume of 15.73 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.05231 M EDTA solution. The solution is then back titrated with 0.02324 M Zn2 solution at a pH of 5. A volume of 20.98 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.04127 M EDTA solution. The solution is then back titrated with 0.02003 M Zn2 solution at a pH of 5. A volume of 16.44 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.04728 M EDTA solution. The solution is then back titrated with 0.02103 M Zn2 solution at a pH of 5. A volume of 19.11 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...
A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.03146 M EDTA solution. The solution is then back titrated with 0.02115 M Zn2 solution at a pH of 5. A volume of 16.97 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...
A cyanide solution with a volume of 22.00 mL was treated with 25.00 mL of Ni2...
A cyanide solution with a volume of 22.00 mL was treated with 25.00 mL of Ni2 (containing excess Ni^2+) to convert the cyanide into tetracyanonickelate(II) ion: 4 CN- (aq) + Ni^2+ (aq) -> Ni(CN)4 ^2-(aq) The remaining unreacted Ni^2+ was reacted with 9.00 mL of 0.01500 M EDTA^4- (a reagent that forms 1:1 complexes with Ni2+ ion but does not react with Ni(CN)4^2- ). EDTA4- (aq) + Ni2+(aq) -> Ni(EDTA)^2- If 40.25 mL of the same EDTA titrant is needed...
Calculate the pZn of a solution prepared by mixing 25.0 mL of 0.0100 M EDTA with...
Calculate the pZn of a solution prepared by mixing 25.0 mL of 0.0100 M EDTA with 50.0 mL of 0.00500 M Zn2+. Assume that both the Zn2+ and EDTA solutions are buffered with 0.100 M NH3 and 0.176 M NH4Cl.
A 50.0 mL sample containing Cd2 and Mn2 was treated with 40.4 mL of 0.0500 M...
A 50.0 mL sample containing Cd2 and Mn2 was treated with 40.4 mL of 0.0500 M EDTA. Titration of the excess unreacted EDTA required 19.2 mL of 0.0300 M Ca2 . The Cd2 was displaced from EDTA by the addition of an excess of CN–. Titration of the newly freed EDTA required 18.2 mL of 0.0300 M Ca2 . What were the molarities of Cd2 and Mn2 in the original solution?
A 50.0 mL sample containing Cd2 and Mn2 was treated with 51.4 mL of 0.0600 M...
A 50.0 mL sample containing Cd2 and Mn2 was treated with 51.4 mL of 0.0600 M EDTA. Titration of the excess unreacted EDTA required 11.1 mL of 0.0190 M Ca2 . The Cd2 was displaced from EDTA by the addition of an excess of CN–. Titration of the newly freed EDTA required 11.3 mL of 0.0190 M Ca2 . What were the molarities of Cd2 and Mn2 in the original solution?
A 50.0 mL sample containing Cd2 and Mn2 was treated with 46.0 mL of 0.0700 M...
A 50.0 mL sample containing Cd2 and Mn2 was treated with 46.0 mL of 0.0700 M EDTA. Titration of the excess unreacted EDTA required 13.1 mL of 0.0230 M Ca2 . The Cd2 was displaced from EDTA by the addition of an excess of CN–. Titration of the newly freed EDTA required 19.3 mL of 0.0230 M Ca2 . What were the molarities of Cd2 and Mn2 in the original solution?