A 0.0250 LL sample of a solution of Cu+(aq)Cu+(aq) requires
0.0328 LL of 0.132 molL−1molL−1 KMnO4(aq)KMnO4(aq) solution to
reach the equivalence point. The products of the reaction are
Cu2+Cu2+ and Mn2+.
What is the concentration of the resulting Cu2+(aq)Cu2+(aq) solution?
A 0.0250 LL sample of a solution of Cu+(aq)Cu+(aq) requires 0.0328 LL of 0.132 molL−1molL−1 KMnO4(aq)KMnO4(aq)...
A 0.0254 L sample of a solution of Cu+(aq) requires 0.0326 L of 0.131 molL−1 KMnO4(aq) solution to reach the equivalence point. The products of the reaction are Cu2+ and Mn2+. Part A What is the concentration of the resulting Cu2+(aq) solution?
Review | Constants Periodic Table A 0.0252 L sample of a solution of Cu+ (aq) requires 0.0319 L of 0.129 mol L-KMnO4(aq) solution to reach the equivalence point. The products of the reaction are Cu²+ and Mn2+. Part A What is the concentration of the resulting Cu²+ (aq) solution? 10 ALQ * O ? (Cu?+) = mol L-1 Submit Previous Answers Request Answer
(b) If a 1.50−g sample of plant matter requires 39.0 mL of 0.0500 M KMnO4 solution to reach the equivalence point, what is the percent by mass of H2C2O4 in the sample
A 23.00 ?mL sample of an unknown HClO4 solution requires titration with 20.12 mL of 0.2000 M NaOH to reach the equivalence point. The neutralization reaction is: HClO4(aq)+NaOH(aq)?H2O(l)+NaClO4(aq) What is the concentration of the unknown HClO4 solution? express your answer using four Sig figs.
QUESTION 1 Minnie Mouse did the Ka by Titrimetry experiment last week. Minnie used 28.63 mL of 0.136 M sodium hydroxide to reach the equivalence point when she titrated 0.3062 g of an unknown monoprotic acid. What is the number of moles of acid that were used? QUESTION 2 The Iron in a sample of iron ore can be converted completely to Fe2+ in aqueous solution, and this solution can then be titrated with KMnO4, as shown: MnO4(q) + 6...
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H+(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2+(aq) in the sample. Express your answer to the appropriate number of significant figures.
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
6. A 25.00mL sample of an H2SO4 solution of unknown concentration requires 24.16mL of 0.106M sodium hydroxide for complete neutralization (to reach the equivalence point). What was the concentration of the H2SO4 solution?
An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and will be used in an experiment to determine the percentage of iron in a sample of ammonium iron (II) sulfate hexahydrate. The titration is self-indicating because at the equivalence point the products are a different colour than the original reactants. The two half reactions are: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) Fe^2+(aq) ---> Fe^3+(aq) + e- a) What is a redox...
The standardization of KMnO4 solution, if the magnetic stir bar was dropped into the flask, and some FAS solution splashed out, how would the calculation for the molarity of KMNO4 be affected? The calculated molarity of KMnO4 would be: Lower. Less FAS would need less MnO4-, therefore, the reduced volume would result in a smaller M. Unchanged. Lower. More FAS would need less MnO4-, therefore, the increased volume would result in a smaller M. Higher. Less FAS would need less MnO4-, therefore, the...