The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4025 g sample of CaCO3 was transferred into a 250 mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4Cl buffer containing a small amount of Mg2+EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA requiring 42.36 mL to reach the end point. Report the molar concentration of the titrant.

A solution containing 60 mL of a 0.025 mol / L metal ion (Mn +) buffer buffered to pH 7.0 was titrated with a 0.05 mol / L EDTA solution. Data: Conditional formation constant (Kf)=10^15. Determine: i) The concentration of the free metal when ½ of the equivalence volume is added. ii) the concentration of free metal in the equivalence volume. iii) the concentration of free metal with an excess of 2 mL of EDTA? (Data - EDTA constants: K1=0.01; K2=2.19.10^-3; K3=6.92.10^-7; K4=5.75.10^-11)

A 50.0 mL solution of 0.100 M Zn2+ ion is titrated with 0.100 M NaOH. Calculate the pZn2+ after the addition of 100.0 mL of NaOH. Ksp for Zn(OH)2 = 3.0 x 10-16.

You are to prepare 100. mL of an acetate buffer of pH 5.00 using 1.0 M acetic acid (CH3CO2H, also written as HC2H3O2) and solid sodium acetate (NaC2H3O2). To prepare for the investigation, complete the following calculations. The pKa for HC2H3O2 is 4.74.     The Henderson-Hasselbach equation is pH = pKa + log ([conjugate base]/[acid])    (a) What ratio of [NaC2H3O2] to [CH3CO2H] is required for a pH = 5.00?  (b) You will want the concentrations relatively dilute, so use an acid concentration of 0.10 M. What volume of 1.0 M CH3CO2H would be needed to prepare 100. mL of buffer with the desired concentration of 0.10 M? Use M1V1 = M2V2  (c) Use the ratio from (a) and the concentration desired (discussed in (b)) to calculate how many grams of NaC2H3O2 · 3 H2O would be needed to prepare 100. mL of buffer if the acid concentration is 0.10 M?

Titration of 46.00 mL of 0.04726 M Na2 C2 04 required 39.26 mL of a potassium permanganate solution. 2Mn O4 + 5H2 C2O4 + 6H+ → 2MN²+ + 10CO2 (g) + 8H20 Calculate the molar concentration of the KMNO4 solution. Concentration

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