2. Hydrazine (N,H) reacts with the bromate ion to produce nitrogen gas and the bromide ion. A 0.132 g sample of impure hydrazine was dissolved in acid and water and the appropriate indicator was added. This sample was then titrated with a 0.02060 M KBRO, solution. To reach the titration's endpoint 38.30 mL of KBrO, were required. Given this information, answer the following questions. a. Write the two half equations. b. Balance each half equation. Write the balanced redox equation. d. What is being reduced? e. What is being oxidized? f. C. o awolicl edd ebiano What is the oxidizing agent? g. What is the reducing agent? h. How many grams of pure hydrazine (MM = sample? i. What is the % N,H, in the sample? 32.06) were present in the

2. Hydrazine (N,H) reacts with the bromate ion to produce nitrogen gas and the bromide ion. A 0.132 g sample of impure hydrazine was dissolved in acid and water and the appropriate indicator was added. This sample was then titrated with a 0.02060 M KBRO, solution. To reach the titration's endpoint 38.30 mL of KBrO, were required. Given this information, answer the following questions. a. Write the two half equations. b. Balance each half equation. Write the balanced redox equation. d. What is being reduced? e. What is being oxidized? f. C. o awolicl edd ebiano What is the oxidizing agent? g. What is the reducing agent? h. How many grams of pure hydrazine (MM = sample? i. What is the % N,H, in the sample? 32.06) were present in the

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 74QAP: A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0...

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The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
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Illustrate the amphoteric nature of aluminum hydroxide by citing suitable equations.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0 ml, of M KMnO4, which oxidizes Fe2+ to Fe3+. The permanganate ion is reduced to manganese(ll) ion. The equation for this reaction is MnO4(aq)+8 H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+ +4H2OAnother 50.00-mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The equation for this reaction is 2Fe3+(aq)+Zn(s)2Fe2+(aq)+Zn2+(aq)The resulting solution is again titrated with 0.0280 M KMnO4; this time 48.0 ml, is required. What are the concentrations of Fe2+ and Fe3+ in the solution?
A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00- mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.