Asked by Catherine
Step 1: A 12.70mL sample of cyanide solution was mixed with 25.00mL of a solution of nickel ions at an appropriate pH to form the Ni-cyanide complex. The resulting solution was titrated cs 0.0130M EDTA and required 10.10mL to reach the end point.
Step 2: Then 30.00mL of the same nickel solution appropriatly titrated separately vs the same EDTA and required 39.30mL of EDTA
a) Suggest an appropriate pH for the step 1 (acid, base, neutral) and give your reason for eliminating the other two pH regions
b) Compare the relative stability of nickel-tetra cyanide and Ni-EDTA complexes
Step 2: Then 30.00mL of the same nickel solution appropriatly titrated separately vs the same EDTA and required 39.30mL of EDTA
a) Suggest an appropriate pH for the step 1 (acid, base, neutral) and give your reason for eliminating the other two pH regions
b) Compare the relative stability of nickel-tetra cyanide and Ni-EDTA complexes
Answers
Answered by
Catherine
I already figured out the answer for b) However, can anyone helps me with a)?
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