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- (a) Identify the species that was reduced in the titration reaction. Justify your answer in terms of oxidation numbers. (c) Given that the concentration of KMnO4(aq) was 0.0235M, calculate the number of moles of MnO4− ions that completely reacted with the H2C2O4. d) The student proposes to perform another titration using a 0.139g sample of H2C2O4, but this time using 0.00143MKMnO4(aq) in the buret. Would this titrant concentration be a reasonable choice to use if the student followed the same procedure and used the same equipment as before? Justify your responsAccounts for the following(i) Rusting of iron is quicker in saline water than in ordinary water.(ii) Blocks of magnesium are straped to the steel hubs of ocean going ships.Explain the term electrolysis. Discuss briefly the electrolysis of (i) moltenNaCl (ii) aqueous sodium chloride solution (iii) molten lead bromide (iv)water.
- State whether each of the following statements is true orfalse. Justify your answer in each case.(a) NH3 contains no OH- ions, and yet its aqueous solutionsare basic.(b) HF is a strong acid.(c) Although sulfuric acid is a strong electrolyte, an aqueoussolution of H2SO4 contains more HSO4- ions than SO42-ions.The following oxidation-reduction reactions take place in basic medium. For each reaction, (i) Assign oxidation state for each atom in the equation; (ii) Indicate oxidation half-equation and reduction half-equation; (iii) Balance the equation by half-equation method; (iv) Indicate which reactant is oxidizing agent and which reducing agent. (v) State and verify whether the pH of the medium decreases, increases, or remains constant as the reaction proceeds.17) The number of Faraday of charge needed to deposit 3.54 x 10-4 moles of Cr+3 ion from its solution is
- What is the purpose of a “salt bridge?The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?(a) Determine the mass of Na,S2O3.5H20 required to prepare 0.1N solution in 50 ml volume. (b) Compare combustion of Anthracene and Xylene in sufficient supply of air. Which one will produce more carbon rich sooty flame and why? (c) Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination will give maximum potential. Provide justification. (d) Explain two industrial applications of acidic buffer solutions. (e) Discuss the importance of Hess law with suitable example.
- Complete and balance the following equations for reac- tions taking place in basic solution. (a) Cr(OH);(s) + Brz (aq) - (b) ZrO(OH)2(s) + SO3 (aq) → (c) HP6O5(aq) + Re(s) - (d) HXeO, (aq)· (e) N,H4(aq)+ CO; (aq) → N2(g)+ CO(g) - Cro (aq) + Br (aq) Zr(s) + SO¯ (aq) → Pb(s) + ReO, (aq) → XeO-(aq) + Xe(g) -Magnesium, the element, is produced commercially by electrolysis from a molten salt (the “electrolyte”) using a cell similar to the one shown here. (a) What is the most common oxidation number for Mg when it is part of a salt?Balance the following redox reactions: (a) In acidic solution, xenon trioxide reacts with iodide ion toproduce xenon gas, triiodide ion (I₃⁻), and water. (b) In basic solution, the hydrogen xenate ion (HXeO₄⁻) dispro-portionates to xenon gas, perxenate ion (XeO₆⁴⁻), water, andoxygen gas.(c) In basic solution, bismuthate ion (BiO₃⁻) reacts with man-ganese(II) ion to produce bismuth(III) and permanganate ions. (d) In basic solution, oxygen difluoride reacts to produce fluo-ride ion, oxygen gas, and water. (e) In acidic solution, manganese(IV) oxide reacts with sulfiteion to form manganese(II) ion, water, and dithionate ion(S₂O₆²⁻).(f) In one of the few reactions known for a statine, the oxidationof astinide ion by chlorine gas in acid solution produces astinateion (AtO₃⁻) and chloride ion.