Fe (s) | FESO4(0.30 M) || KIO3(0.50 M), 12(s), pH 4.0 | Pt(s) Given: Fe2+ +2 e Fe (s) EO - 0.44 %3D Fe +e ------ Fe2+ EO 0.771 V 103 + 6 H* + 5e V2 12(s) + 3 H20 (1) EO = 1.210 V

If, in the equilibrium constant lab, you measured a molar abosorptivity for Fe(SCN)2+ to be 5,000 M-¹, when it was actually 4,000 M-1, would this affect the value of your equilibrium constant? Explain your answer.

16,17, & 18

8 (a) Define in words the following: (i) Ka (ii) pKa

What is the concentration of S2- in equilibrium with MnS(s) (Ksp [S²] = M = 4.6 x 10-¹4) and 0.098 M Mn²+?

What is the value of the formation constant of the complex ion formed below? Equilibrium concentrations: [M3+] = 0.025 M; [L] = 0.015 M; [ML4] = 3.5 x 10-6 M %3D M3+ (aq) + 4L (aq) ML4 (aq) Select one: A. 2.8 x 103 B. 3.6 x 10-4 C. 6.0 x 102 D. 2.8 x 103

Please answer the following pertaining to analytical chemistry.

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