Thiosulfate ion,
a.
b.
c.
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General Chemistry: Principles and Modern Applications (11th Edition)
- Using Table 17.1, calculate E° for the reaction between (a) chromium(II) ions and tin(IV) ions to produce chromium(III) ions and tin(II) ions. (b) manganese(II) ions and hydrogen peroxide to produce solid manganese dioxide (MnO2)arrow_forwardUsing Table 17.1, calculate E° for the reaction between (a) lead and silver nitrate ion to produce lead(II) nitrate. (b) oxygen and iron(II) ions to produce water and iron(III) ions. (c) sulfur and nitrogen oxide gas in basic solution to form nitrate and sulfide ions.arrow_forwardWhat does it mean for a substance to be oxidized? The term “oxidation” originally came from substances reacting with oxygen gas. Explain why a substance that reacts with oxygen gas will always be oxidized.arrow_forward
- Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forwardWhen balancing reactions in Chapter 3, we did not mention that reactions must be charge balanced as well as mass balanced. What do charge balance and mass balance mean? What happens in a redox reaction that requires charge to be balanced?arrow_forwardIdentify each of the blowing substances as a likely oxidizing or reducing agent: HNO3, Na, C12, O2, KMnO4.arrow_forward
- Use Table 17.1 to select (a) a reducing agent in acidic solution that converts ClO3- to Cl2 but not Cr2O72- to Cr3+. (b) an oxidizing agent that converts Mg to Mg2+ but not Mn to Mn2+. (c) a reducing agent in basic solution that converts NO2- to NO3- but not OH- to O2.arrow_forwardA factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?arrow_forwardCopper can be plated onto a spoon by placing the spoon in an acidic solution of CuSO4(aq) and connecting it m a copper strip via a power source as illustrated below: a. Label the anode and cathode. and describe the direction of the electron now. b. Write out the chemical equations for the reactions that occur at each electrode.arrow_forward
- The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?arrow_forward. For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a.3Zn(s)+N2(g)Zn3N2(s)b.Co(s)+S(s)CoS(s)c.4K(s)+O2(g)2K2O(s)d.4Ag(s)+O(g)2Ag2O(s)arrow_forwardWrite balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.arrow_forward
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