Calculate pCd²+ at each of the following points in the titration of 55.00 mL of 0.0070 M Cd²+ with 0.0070 M EDTA in the presence of the auxiliary complexing agent NH3. The solution is buffered at a pH of 11.00. Take the NH3 concentration to be a constant 0.100 M. The formation constant for the Cd²+-EDTA complex is given by log K₁ = 16.5. (a) 0 mL (b) 2.00 mL (c) 50.00 mL (d) 55.00 mL (e) 60.00 mL ----- Number Number Number Number Number

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

Taking the Ksp of Zn(OH)2 as 4.0 x 10^-3 and the Kf of [Zn(NH3)6] as 1.0x 10^8, determine how many moles of Zn(OH)2 can dissolve in 0.6 L of 1.2M NH3.

A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction is 2Fe3+   +   Sn2+   ⇋   2Fe2+   +   Sn4+             and Fe3+   +   e−   ⇋   Fe2+                                        E° = +0.732 V Sn4+   +  2e−   ⇋   Sn2+                                       E° = +0.139 V   What is the volume of Sn2+ is added at the equivalence point?

1)Calculate the pH of 650. mL of a 0.439-M solution of hypochlorous acid before and after the addition of 0.196 mol of sodium hypochlorite.pH befor addition = pH after addition =  2)A 9.56×10-2-M aqueous solution of C2H5NH2 (ethylamine) has a pH of 11.8. Calculate the pH of a buffer solution that is 9.56×10-2 M in C2H5NH2 and 0.317 M in C2H5NH3+.pH =

A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value