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Balance all by oxidation method
1) I2 + HNO3 => HIO3 + NO2 + H2O
2) Cu + H2SO4 => CuSO4 + H2O + SO2
3) Balance the following equations in acidic solutions
Cr2O7 ^-2(aq) + Cl^- (aq) => Cr^+3 (aq) + Cl2(aq)
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- 0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?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.1. What is the gravimetric factor of SO3 in BaSO4? 2. What is the normality of an oxidizing agent of a solution of potassium dichromate (K2Cr2O7) containing 8.906 g per 200 mL in the presence of acid? (Cr2O7-2 + 6Fe+3 + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O) NOTE: Present complete solution with corresponding units.
- 35.00 mL of a solution of KIO3 reacted with exactly 35.00 mL of a 0.1000 M solution of KI in acid medium according to the equation IO3 + I + H+ → I2 + H2O (a) Balance the equation and calculate the molarity of the KIO3 solution. (b) 50.00 mL of this KIO3 is treated with excess pure KI in acid solution and the liberated I, is titrated with 0.1000 N Na2S2O3. What volume of titrant is required?A solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. Calculate the %w/w Ag in the alloy. (Mwt of Ag = 107.87 g/mol)
- An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What volume (in mL) of 0.500 M HCl would be required to neutralize the resulting solution? (Hint: H2 is produced at the cathode and Cl2 at the anode.)A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co from a solution of ZnSO4 and CoSO4 . The mixture of Zn and Co that was deposited had a mass of 53.23 g. Calculate the masses of ZnSO4 and CoSO4 present in the original solution.Balance the following by redox reaction: Indicate the reducing agent and the oxidizing agent. 1. Cr2O72- + C2O42- ----> Cr+3 + CO2 (acidic solution) 2. Complete and balance the equation by redox Zn(s) + CuSO4 (aq)
- when the 35.0ml of KOH(2.0M) was added to the aluminum sample (1.430g), the student spilled some of the measured KOH on the bench and in the end, only 24.5ml of the KOH solution was added to the Aluminum pieces. Was there enough KOH added so that all the aluminum could reactA precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?For a redox analysis of iron, how do you calculate the % (weight/weight) with a mass of the K2Cr2O7 that was diulted to 250.00ml is 1.488 grams, mass of unknown is 0.2839g, and the vol. titrant given was 24.38 ml?