To measure the concentration of an aqueous solution of H₂O,, an analytical chemist adds strong acid to a 34.00 g sample of the solution and titrates it to the endpoint with 61.3 ml. of 0.450M potassium permanganate (KMnO,) solution. The balanced chemical equation for the reaction is: 6H (aq) SH₂O₂ (aq) 2MBO (og) + What kind of reaction is this? - 50,(eg) + 2Mn (aq) + SH₂O(0) If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of H₂O, in the sample. Be sure your answer has the correct number of significant digits. O precipitation O acid-base redox 0 0 O 0% q X 8 3

A sample of iron ore is dissolved in acid, and the iron is converted to Fe2*. The sample is then titrated with 47.20 mL of 0.02240 M MnO4 solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) + 4H2O How many moles of MnO4¯ were added to the solution? Blank 1 2+ How many moles of Fe were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer Blank 4 Add your answer

The quantity of antimony in a sample can be determined by an oxidation–reduction titration with an oxidizing agent. A 6.19 g6.19 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+⁢(aq). The Sb3+⁢(aq) is completely oxidized by 30.5 mL of a 0.115 M aqueous solution of KBrO3⁢(aq). The unbalanced equation for the reaction is   BrO^−  3(aq) + Sb^3+(aq)⟶Br^−(aq)+Sb^5+(aq)(unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony in grams:     percentage of antimony:

The following chemical reaction takes place in aqueous solution: SnBr₂(aq) +2 KOH(aq) → Sn(OH)₂(s)+2 KBr(aq) Write the net ionic equation for this reaction.