1. Determine the oxidation numbers of the elements indicated. a.* manganese in \( \mathrm{MnCl}_{2}, \mathrm{MnO}_{2}, \mathrm{MnO}_{4} \) b. nitrogen in nitrate, nitrogen dioxide, nitrite, nitrogen monoxide, dinitrogen monoxide, nitrogen and ammonia \( \overline{\text { nitrate }} \) \( \overline{\text { nitrogen }} \) nitrogen dioxide nitrite \( \overline{\text { nitrogen }} \) nitrogen \( \overline{\text { dinitrogent }} \) dinitrogent \( \overline{\text { nitrogen }} \) \( \overline{\operatorname{ammon} i a} \) c. arsenic in \( \mathrm{As}_{2} \mathrm{O}_{3}, \mathrm{As}_{2} \mathrm{O}_{5}, \mathrm{~K}, \mathrm{AsO} \) taitanty c. arsenic in \( \mathrm{As}_{2} \mathrm{O}_{3}, \mathrm{As}_{2} \mathrm{O}_{5}, \mathrm{~K}_{3} \mathrm{AsO}_{4} \) d. oxygen in \( \mathrm{H}_{2} \mathrm{O}, \mathrm{H}_{2} \mathrm{O}_{2} \) \( \mathrm{H}, \mathrm{O} \) \( \overline{\mathrm{H}_{2} \mathrm{O}_{2}} \) 2. Write balanced half reactions and complete reactions for the following oxidation-reduction reactions \[ \text { a.* aluminum(s) }+ \text { hydrogen ion(aq) } \rightarrow \text { aluminum ion(aq) }+ \text { hydrogen(g) } \] oxid. half rxn. red. half rxn: overall rxn: b. chloride + permanganate \( \rightarrow \) manganese(II) ion + chlorine(g) (aqueous acid) oxid. half rxn: red. half rxn:: overall rxn:: Scanned with CamScanner 362 c. tin(II) ion + dichromate \( \rightarrow \) tin(IV) ion + chromium(III) ion (aqueous acid) oxid. half rxn. red. half rxn: overall rxn: 3. For problem \( 2-c \), give answers to the following: What is oxidized? What is reduced? What is the oxidizing agent? What is the reducing agent? 4. Calculate the approximate amount of sodium thiosulfate pentahydrate needed to prepare 500 \( \mathrm{mL} \) of a \( 0.20 \mathrm{M} \) solution. \( \square \) \( \qquad \) \( \qquad \) \( \qquad \) 5.* A 0.800 gram sample of potassium ferricyanide is titrated with a sodium thiosulfate solution according to the procedure given above. \( 19.00 \mathrm{~mL} \) of the sodium thiosulfate solution are required to reach the starch end point. What was the concentration of the sodium thiosulfate solution? 6. For the titration in this experiment, explain how the indicator functions.
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Determine the oxidation numbers of the elements indicated. #### a. Manganese in \( \mathrm{MnCl}_{2}, \mathrm{MnO}_{2}, \mathrm{MnO}_{4}^{-} \) ** Show more…
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Procedure Overview: The oxidation number of an element in a selection of compounds and ions is determined by application of the rules in the Introduction. Your instructor will indicate the questions you are to complete. Answer them on a separate piece of paper. Be sure to indicate the date, your lab section, and your desk number on your Report Sheet. 1. Indicate the oxidation number of carbon and sulfur in the following compounds. a. CO b. CO2 c. Na2CO3 d. Na2C2O4 e. CH4 f. H2CO g. SO2 h. SO3 i. Na2SO4 j. Na2SO3 k. Na2S2O3 l. Na2S4O6 m. SCl2 n. Na2S2 o. SOCl2 2. Indicate the oxidation number of phosphorus, iodine, nitrogen, tellurium, and silicon in the following polyatomic ions. Remember that the sum of the oxidation numbers for a polyatomic ion must equal the charge of the ion. a. PO4^3- b. PO3^3- c. HPO4^2- d. P3O10^5- e. IO3^- f. IO2^- g. IO^- h. NH4^+ i. NO3^- j. NO2^- k. NO^+ l. NO2^+ m. N2O2^2- n. TeO4^2- o. SiO3^2- 3. Indicate the oxidation number of the metallic element(s) in the following compounds. None of the compounds listed are peroxides. a. Fe2O3 b. FeO c. CoS d. CoSO4 e. K3CoCl6 f. CrCl3 g. CrO3 h. K2CrO4 i. K2Cr2O7 j. KCrO2 k. K2MnO4 l. Mn2O7 m. MnO2 n. PbO2 o. Pb3O4 p. ZrI4 q. U3O8 r. UO2Cl2
Adi S.
1. In a reaction between copper metal and an aqueous iron (III) chloride, Fe3+(aq) is reduced to Fe2+(aq), while Cu(s) is oxidized to Cu2+(aq). Determine the mass of Cu(s) required to react with 18.3 ml of 1.88 M FeCl3(aq). 2. What is the mass, in grams, of Vitamin C, which contains 0.768 grams of carbon? (Vitamin C, C6H8O6.) 3. The color change from pink/violet to colorless is caused by: a. change from MnO4- to Mn2+ b. change from Fe2+ to Fe3+ c. change from H+ to H2O d. addition of indicator 4. When MnO4- reacts to form Mn2+ the manganese in MnO4- is: a. reduced as its oxidation number decreases b. oxidized as its oxidation number decreases c. oxidized as its oxidation number increases d. reduced as its oxidation number increases 5. What is the difference between the endpoint and equivalence point in a titration? a. the endpoint is when the pH is exactly 7 b. the equivalence point is when the pH is exactly 7 c. the endpoint and the equivalence point are the same thing d. none of these answers is correct
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What are the oxidation numbers of the metal atoms in the following compounds? Drag the appropriate items to their respective bins. CoO, PbCl2, CrO3, FeP, SnCl4 Assign an oxidation number to each atom in the reactants and products shown here to determine which of the following reactions are redox reactions. Assign an oxidation number to each atom in the reactants. Na2S(aq) + NiCl2(aq) → 2NaCl(aq) + NiS(s) Express your answers as signed integers separated by commas. For example: +1, +2, +3. Assign an oxidation number to each atom in the products. Na2S(aq) + NiCl2(aq) → 2NaCl(aq) + NiS(s) Express your answers as signed integers separated by commas. For example: +1, +2, +3. Assign an oxidation number to each atom in the reactants. 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) Express your answers as signed integers separated by commas. For example: +1, +2, +3.
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