A solution of 0.0100 moles of pure Na_2H_2EDTA is prepared in 1.00 L of aqueous

Question

A solution of 0.0100 moles of pure Na_2H_2EDTA is prepared in 1.00 L of aqueous solution. Calculate the molarity of this solution. Suppose EDTA is of unknown purity, and this solution needs to be standardized. In one or two complete sentences, maximum 50 words, describe a titration procedure (naming specific reagent(s)) that could be used to establish the concentration of the solution. Calculate the conditional formation constant for the titration of Tl^3+ (aq) at pH = 2.50; use data from Tables in Harris, and you may interpolate a Table for alpha_Y4- Write an appropriate algebraic expression that could be used for calculating alpha_Y4- at pH = 2.50, defining all terms clearly; include the appropriate value of [H_3O^+].

Explanation / Answer

A) Molarity = moles / volume in Litres

Therefore,

Molarity of Na2H2EDTA = 0.01 moles/ 1.0 L = 0.01 M

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