-14°C 5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change from red to pale blue. Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq). Trial Final burette reading (mL) Initial burette reading (mL) Volume of Ce4+ = 1 15.7 0.6 2 30.7 15.7 3 45.6 30.7 4 40.2 25.3 (Answer: 14.975) Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore analysis? (Answer: 7.49 x 10¹² M) ENG £ 1 0 + O E 5:42 PM

Hh.88.

Please don't provide handwritten solution ....

16,17, & 18

calculationS H= 1 Fe = 55.8; S = 32; O= 16; 10 10g of an impure iron(11) salt were dissolved in water and made un to 200 cm of solution. 20cm of this solution, acidified with dilute sulphuric acid, required 25 cm3 of 0.04 M KMNO4(aq) before a faint pink colour appeared. (a) Write a balanced ionic equation (or half-equations) for the reaction of acidified manganate(vII) (permanganate) ions with iron(11) ions. (b) How many moles of iron(1) ions react with one mole of MnO4 ions? (c) How many moles of Fe2 react with 25 cm' of 0.04 M KMNO4(aq)? (d) How many grams of Fe2 are there in the 200 cm' of original solution? (Fe 56) (e) Calculate the % by mass of iron in the impure iron(11) salt.

22. The following problem pertains to AgBr(s), Ksp = 5.0 x 10-13, Hg,Br2(s), Ksp = 1.3 x 10-22, and [Ag(S2O3)2]³-, Kf= 2.9 x 1013. A. (i) Include state symbols. Write the reaction for dissolving (dissolution) of AgBr(s) into its aqueous ions. Write the reaction for dissolving (dissolution) of Hg2Br2(s) into its aqueous ions. (ii) Include state symbols. Hint: recall mercury forms a Hg22* ion. (iii) Write the formation constant expression (Kr) for the complex ion [Ag(S2O3)2]3-

Write a balanced net ionic equation to show why the solubility of AgCN(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (s). K= + + +

Calculate AG° and K at 25°C for the reactions. 7H2O + 2 Cr+ + 3 Cl2 = Cr2 07²- + 6 Cl¯ + 14H = 0.03 V cel a. AG° = kJ K = Cu²+ (aq) + Ba(s) = Ba2+ (aq) + Cu(s) e° = 3.24 V b. AG° : kJ K = Cl2 (g) + 2 Br (aq) = Br2 (g) + 2 Cl¯ (ag) e° = 0.27 V C. AG° = kJ K = 3H2 O(1) + 5 IO4 (ag) + 2 Mn²+ (aq) = 5 IO3 (aq) + 2 MnO4¯(ag) + 6H† (ag) d. 0.09 V ´cell AG° = kJ K =