EDTA titration-(Analytical Chem.)

[tipton12]

EDTA titration--(Analytical Chem.)

A mixture of Mn2+, Mg2+, and Zn2+ was analyzed as follows: The 25.00mL sample was treated with 0.25g of NH3OHCl (hydroxylammonium chloride)--a reducing agent that maintains manganese in the 2+ state. 10 mL of ammonia buffer (pH10) and a few drops of eriochrome black T indicator and then diluted to 100 mL. It was warmed to 40 degrees (C) and titrated with 39.98 mL of 0.04500 M EDTA to the blue end point. Then 2.5g of NaF was added to displace Mg2+ from its EDTA complex. The liberated EDTA required 10.26 mL of standard 0.02065 M Mn2+ for complete titration. After this second end point was reached, 5 mL of 15 wt% aqueous KCN was added to displace Zn2+ from its EDTA complex. This time the liberated EDTA required 15.47 mL of standard 0.02065 M Mn2+. Calculate the number of milligrams of each metal (Mn2+, Zn2+, and Mg2+) in the 25.00 mL sample of unknown. (note: EDTA reacts 1:1 with metal ions).

--ok, I seriously have no idea where to start. I definitely need a starting point. Am I right to assume since EDTA reacts 1:1, that I do not need to do redox for each metal ion? ---Please help!

 

[chem_tr]

Yes, EDTA reacts with almost all metal ions in 1:1 stoichiometric molar ratio, as it has six donor atoms to bind to metal ions. Multiply all the volumes in mL with their corresponding concentrations in mol/L to convert to their millimoles. This may help you fro the beginning.

 

[tipton12]

I did that already to get:

(10.26mL)(0.02065mmol/mL)=0.2112 mmol Mn2+
(15.47mL)(0.02065mmol/mL)=0.3195 mmol Mn2+

Then, I subtracted the two, to get 0.1083mmol Mn2+
I then took that number and multiplied it with the weight:
(.1083mmol Mn2+)(54.938mg/mmol Mn2+)=5.95mg Mn2+

Is this correct for the Mn2+? Or do I need to do something different? When I got to that point, I didn't know where else to go to get the Zn2+ and the Mg2+. Any suggestions?

 

[chem_tr]

It seems okay with Mn²⁺ ion.

In the beginning, you know that

39.98 mL of 0.04500 M EDTA

is the total of three ions.

MgF₂ precipitate is formed by the action of fluoride to magnesium, if I am not wrong. So one mole of EDTA is released to the medium, and this is treated with the given amount of standard Mg²⁺ solution.

Zinc ion forms a tetracyanozincate(II) complex, as shown with the formula [Zn(CN)₄]^2-.

What you need to do is simply write the formation reactions of the compounds I mentioned, and find how many moles of reactants (fluoride or cyanide) is required.

 

[tipton12]

I got 7.035mg Zn2+ , 2.14x10^3 mg Mg2+, and 5.95mg Mn 2+. I hope these values are correct,but if they are not then it is only an error in my math. thanks a lot for all your help! tipton12

 

[tipton12]

I changed my answer last minute to get the actual correct answers:
mmoles Mg2+= (10.26)(.02065M)=.2119
mmoles Zn2+=(15.47mL)(.02065M)=.3195
mmoles Mn2+=1.799-.2119-.3195=1.278

(.2119mmolesMg2+)(24.3051mg/mmole)=5.150mg Mg2+
(.3195mmolesZn2+)(65.392mg/mmole)=20.89mg Zn2+
(1.278mmolesMn2+)(54.9380mg/mmole)=70.21mgMn2+

 

[tipton12]

the 1.799 comes from (39.98mL)(.04500mmoles/mL EDTA)=1.799