(a)
Interpretation: Advantages and/or disadvantages of using sodium hypochlorite for oxidation over
Concept introduction:
(b)
Interpretation: Advantages and/or disadvantages of using sodium hypochlorite for oxidation over
Concept introduction: Sodium hypochlorite is a green chemistry reagent for oxidation of alcohols as it avoids the usage of strong acids and also no carcinogenic metals are used. Sodium hypochlorite is also a green chemistry reagent for oxidation of alcohols as no carcinogenic metals are used.
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Organic Chemistry
- In an analytical determination of arsenic, a solution containing arsenious acid, H3AsO3, potassium iodide, and a small amount of starch is electrolyzed. The electrolysis produces free iodine from iodide ion, and the iodine immediately oxidizes the arsenious acid to hydrogen arsenate ion, HAsO42. I2(aq)+H3AsO3(aq)+H2O(l)2I(aq)+HAsO42(aq)+4H+(aq) When the oxidation of arsenic is complete, the free iodine combines with the starch to give a deep blue color. If, during a particular run, it takes 65.4 s for a current of 10.5 mA to give an endpoint (indicated by the blue color), how many grams of arsenic are present in the solution?arrow_forwardCalcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?arrow_forward3NHA + BiN (s) → Bi3+ + 4NH3 The reaction above occurs in liquid ammonia. In this reaction, the ammonium ion behaves as: a base a reducing agent an oxidizing an acidarrow_forward
- please explain how to balance and predict the reaction: (CH2)2 (CH)4(L) + O(G)=?arrow_forwardCalculate the mass of Na2S2O3•5H2O needed to prepare a 1.00-liter solution of 0.0700 M concentration. Write the net ionic balanced equation for the redox reaction of iodate and iodide in acidic medium forming iodine and water. This is the pre-titration reaction. Write the net ionic balanced equation of iodine and thiosulfate forming iodide and tetrathionate, S4O62-. This is the titration reaction. Write the overall balanced equation for reactions 2 and 3. What is the expected color at this endpoint? Write the balanced net ionic equation when ascorbic acid, C6H8O6, reacts with iodine to form dehydroascorbic acid, C6H6O6 and iodide in acidic medium. This is second pre-titration reaction for the analysis of Vitamin C.arrow_forwardComplete and balance the following equation:(acid - base) H2SO4 + KOHarrow_forward
- Write a balanced chemical equation for the acid-base reaction of oxalic acid, H2C2O4, with sodium hydroxide.arrow_forwardBalance the following chemical equation (if necessary): V₂O₅(s)+HCl(aq)→VOCl₃(s)+H₂O(l)arrow_forwardWrite the balanced NET ionic equation for the reaction when aqueous KBr and aqueous AGC2H3O2 are mixed in solution to form aqueous KC:H3O2 and solid AgBr.arrow_forward
- What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the Kp for CH3NH2 is 4.4 x 104 and the Ka for HNO3 is 2.4.arrow_forwardHow do I find the oxidation numbers for I2O5 ? what are they and how did you get there?arrow_forwardbalance the equation and indicate the type of reaction C6H6 (l) + O2 (g) → CO2 (g) + H2O (l)arrow_forward
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