To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 46.0g sample in strong acid and titrates it to the endpoint with 130.mL of 0.1900M potassium permanganate KMnO4 solution. The balanced chemical equation for the reaction is: 8H+(aq) + 5Fe2+(aq) + MnO−4(aq) -> 5Fe3+(aq) + Mn2+(aq) 4H2O(l) What kind of reaction is this? 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 Fe in the sample. Be sure your answer has the correct number of significant digits

The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 5.43 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCI(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 28.0 mL of a 0.110 M aqueous solution of KBrO, (aq). The unbalanced equation for the reaction is Bro, (aq) + Sb³+(aq) → Br (aq) + Sb3+ *(aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: percentage of antimony: %

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In the following reaction, what ions (if any) are spectator ions? AgNO­3 (aq) + 2NaI (aq) -> AgI (s) + NaNO3 (aq)

The following reaction occurs in acidic solution. As, O6(s) + MnO, (ag)AsO (aq) + Mn²* (aq) What is the sum of the coefficients in the balanced equation?

25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction:                                K2S(aq)  + 2HNO3(aq)   →  2KNO3(aq)  + H2S(g) The concentration of sulphide ion in the final solution is

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 316.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 93.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.

The concentration of Sn²+ in a solution is determined by titrating it with a 0.1890 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnOq°(aq) + 5Sn²*(aq) + 16H3O*(aq) → 2Mn²+(aq) + 5Sn*(aq) + 24H,O(1) In one experiment, 24.99 mL of the 0.1890-M permanganate solution is required to react completely with 40.00 mL of the Sn2+ solution. Calculate the concentration of the Sn2+ solution. M

To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 41.0 g sample in strong acid and titrates it to the endpoint with 38.3 mL of 0.4700M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 3+ 2+ 8H (aq) + 5Fe²+ (aq) + MnO4(aq) → 5Fe³+ (aq) + Mn²+ (aq) + 4H₂O(1) What kind of reaction is this? 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 Fe in the sample. Be sure your answer has the correct number of significant digits. precipitation acid-base O redox 0 0 0 % X Ś x10

A CHM 125 student performed the "Redox Titration" procedure as given in the laboratory manual. In this experiment, the titrant solution of potassium permanganate (KMNO4) was used to determine the percentage of sodium oxalate (NazC2O4) in an unknown sample. The net ionic equation for the titration carried out was: 2MnO4 (aq) + 5C20,7(aq) + 16H*(aq) → 2MN²*(aq) + 10CO2(g) + 8H2O(£) The data provided in the table below was acquired. Complete the table and determine the percent of sodium oxalate in the unknown sample based on this one titration. Molarity of KMNO, Titrant Solution: 0.0203 M Trial 1 Weight of Oxalate 0.954 g Unknown Starting Buret Reading: 0.65 mL Ending Buret Reading: 34.85 mL of permanganate sl order to use 35.00 mL of Titrant Used: mmol of MnO4 mmol of 2- Weight of NazC204 in Unknown: Percent of Na,C204 in Unknown: You wer 4-