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- Write a balanced equation for the reaction scheme belowWrite a balanced net-ionic equations to describe a. reduction of Fe3+ to fe2+ by SO2b. reaction of H2MoO4 in a Jones reductorc. oxidation of HNO2 by a solution of MnO4-d. reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solutione. air oxidation of HAsO3(2-) to HAsO4(2-)f. reaction of KI with HNO2 in acidic solutionAssuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and a value of 3.5 × 10−11 for the solubility product of FeCO3, what would you expect to be the stable iron species at pH 9.5 and pE −8.0, as shown in Figure 3.4?
- Dry hydrogen chloride gas does not turn blue litmus red whereas dilute hydrochloric acid does. State the reason ?Percentage purity of a sample of 0.1350 g of As2O3 assayed iodometrically using 23.5 mL of 0.1055N iodine solutionBleach (sodium hypochlorite, NaOCl, a strong oxidizing agent) neutralizes and inactivates mustard gas. Bleach is also effective on organic stains because it oxidizes coloredcompounds to colorless compounds. Propose products that might be formed by thereaction of mustard gas with bleach
- Provide detailed solutions.What wt. of impure calcite (CaCO3) should be taken for analysis so that no. of milliliters of CO2 obtained by treating with acid, and measured dry at 18°C and 763 mm pressure, will equal the percentage of CaO in the sample?Calculate the pH of an aqueous solution prepared by dissolving 5.61 g of KOH pellets in water and diluting to a final volume of 0.500 L. (At. wts: K = 39.10, O = 16.00, H = 1.008)
- A sample known to consist of NaOH orNaHCO3, or Na2CO3 or possible compatible mixtures of these, together with inert matter. With methyl orange, a 1.10 g sample requires 31.40 mL of HCl (of which 1.00 mL ≈ 0.0140 g CaO). With phenolphthalein, the same weight of sample requires 13.30 mL of the acid. Calculate the percentage of inert matter in the sample.if we use KMnO4 and H3Po4 and MnSO4 for tritation of fecl3 and calculation of. Fe2+ what suitable ratio for tritationWrite balanced net-ionic equations to describe: (a) the reduction of Fe3+ to Fe2+ by SO2 (b) the reaction of H2MoO4 in a Jones reductor (c) the oxidation of HNO2 by a solution of MnO-4. (d) The reaction of aniline (C6H4NH2) with a mixture of KBrO3 and KBr in acidic solution (e) the air oxidation of HAsO2-3 to HasO2-4 (f) the reaction of KI with HNO2 in acidic solution Please answer letters d, e, and f
