A solution containing 30.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was
ID: 943749 • Letter: A
Question
A solution containing 30.00 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 (Y4-) of free EDTA in the form Y4-. Keep 2 significant figures.
If the formation constant (Kf) is 1012.00. Calculate the value of the conditional formation constant Kf’ (=Y4- * Kf) and enter your result as scientific notation form.
Calculate the concentration (M) of free metal ion M+ at V = Ve. (Use the Kf' calculated above)
I'm stuck because theres no other information is provided nor given.
Explanation / Answer
Equivalence Volume = (Concentration of metal ion x Volume of metal ion)/concentration of EDTA
= (0.05 x 30)/0.04
= 37.5 ml
Volume of free metal ion at {V = 1/2 Ve = 18.75 ml} = 15 ml
Volume of total solution at {V = 1/2 Ve = 18.75 ml} = 30+18.75 = 48.75 ml
concentration (M) of free metal ion at {V = 1/2 Ve = 18.75 ml} = (0.05 x 15)/48.75
= 0.01538 M
fraction (Y4-) of free EDTA in the form Y4- = Y4- x concentration of EDTA
= 0.36(taken from literatute for pH = 10)x 0.04
= 0.0144 M
conditional formation constant Kf’ = 0.36 x 1012
= 364.32
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