Question

In: Chemistry

A 1.000 mL aliquot of a solution containing Cu 2 + and Ni 2 + is...

A 1.000 mL aliquot of a solution containing Cu 2 + and Ni 2 + is treated with 25.00 mL of a 0.05485 M EDTA solution. The solution is then back titrated with 0.02234 M Zn 2 + solution at a pH of 5. A volume of 21.46 mL of the Zn 2 + solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu 2 + and Ni 2 + solution is fed through an ion-exchange column that retains Ni 2 + . The Cu 2 + that passed through the column is treated with 25.00 mL of 0.05485 M EDTA . This solution required 15.70 mL of 0.02234 M Zn 2 + for back titration. The Ni 2 + extracted from the column was treated witn 25.00 mL of 0.05485 M EDTA .

How many milliliters of 0.02234 M Zn 2 + is required for the back titration of the Ni 2 + solution?

Solutions

Expert Solution


Related Solutions

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 0.03742 M EDTA solution. The solution is then back titrated with 0.02190 M Zn2 solution at a pH of 5. A volume of 20.48 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 0.05893 M EDTA solution. The solution is then back titrated with 0.02306 M Zn2 solution at a pH of 5. A volume of 19.89 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 0.04503 M EDTA solution. The solution is then back titrated with 0.02327 M Zn2 solution at a pH of 5. A volume of 22.80 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 0.05832 M EDTA solution. The solution is then back titrated with 0.02380 M Zn2 solution at a pH of 5. A volume of 18.49 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...
What is the concentration of Cu in a solution if a 25.00 mL aliquot reacted with...
What is the concentration of Cu in a solution if a 25.00 mL aliquot reacted with an excess of KI that requires 15.64 mL of 39.94 mM Na2S2O3 solution to titrate the liberated iodine?
What is the correct order of magnetic strength among the following elements? a) Fe > Co > Ni > Cu b) Fe > Ni > Co > Cu c) Cu > Ni > Co > Fe d) Cu > Fe > Ni > Co
What is the correct order of magnetic strength among the following elements? a) Fe > Co > Ni > Cu b) Fe > Ni > Co > Cu c) Cu > Ni > Co > Fe d) Cu > Fe > Ni > Co
A 23.33-mL solution containing 1.718 g Mg(NO3)2 is mixed with a 30.50-mL solution containing 1.467 g...
A 23.33-mL solution containing 1.718 g Mg(NO3)2 is mixed with a 30.50-mL solution containing 1.467 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive. If a species fully precipitates, type 0. a.) ______ M Mg2+ b.) ______ M NO3- c.) ______ M Na+ d.) ______ M OH-
A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of...
A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is then added to the mixture. Assume no change in volume. Ksp = 2.2 × 10-20 for Cu(OH)2, Ksp = 1.3 × 10-15 for Co(OH)2 The hydroxide concentration at which the first metal hydroxide will just begin to precipitate is __________M Using the integer designators, the metal hydroxide that precipitates first is {(1) Cu(OH)2 or (2) Co(OH)2 } _____________M...
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.
A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+...
A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O → HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60°C, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT