A permanganate solution is standardized by titrating it with a 0.1491 M hydrogen peroxide solution. The balanced net ionic equation for the reaction is: 2MnO4-(aq) + 5H2O2(aq)+6H3O+(aq)2Mn2+(aq) + 5O2(g)+14H2O(l) If 21.22 mL of the 0.1491 M hydrogen peroxide solution is required to react completely with 25.00 mL of the permanganate solution, calculate the concentration of the permanganate solution.
A permanganate solution is standardized by titrating it with a 0.1491 M hydrogen peroxide solution. The...
The redox reaction between hydrogen peroxide, H2O2, and permanganate ions, MnO4-, in acid solution are as follows: 5H2O2(aq) + 2MnO4-(aq) + 6H+(aq) → 5O2(g) + 2Mn2+(aq) + 8H2O (l) 5 mol of MnO4-was required to reach the equilibrium. How many moles of H2O2were required to reach the equilibrium? a) 2 mol b. 10 mol c) 12.5 mol d) 25 mol
The concentration of Cu+ in a solution is determined by titrating it with a 0.1621 M permanganate solution. The balanced net ionic equation for the reaction is: MnO4-(aq) + 5Cu+(aq) + 8H3O+(aq) Mn2+(aq) + 5Cu2+(aq) + 12H2O(l) In one experiment, 18.21 mL of the 0.1621-M permanganate solution is required to react completely with 25.00 mL of the Cu+ solution. Calculate the concentration of the Cu+ solution.
The concentration of hydrogen peroxide solution can be determined by titration against a standardized solution or potassium permanganate in acidic medium according to the following equation: 2MnO4 + 5H2O2 + 6H* -----> 502 + 2Mn+2 + 8H2O What is being oxidized? What is being reduced? What is the oxidizing agent? What is the reducing agent? If 36.44 mL of a 0.01652 M KMnO4 solution are required to oxidize 25.00 mL of a H2O2 solution, calculate the molarity of the H2O2...
The concentration of H3AsO3 in a solution is determined by titrating it with a 0.1807 M Ce4+ solution. The balanced net ionic equation for the reaction is: 2Ce4+(aq) + H3AsO3(aq) + 5H2O(l) 2Ce3+(aq) + H3AsO4(aq) + 2H3O+(aq) In one experiment, 22.27 mL of the 0.1807 M Ce4+ solution is required to react completely with 25.00 mL of the H3AsO3 solution. Calculate the concentration of the H3AsO3 solution?
The concentration of hydrogen peroxide, H2O2, in a solution is determined by titrating a 13.0 mL sample of the solution with permanganate ion, producing manganese(II) ion and oxygen gas. Part A Enter the balanced chemical equation for the redox reaction that occurs in acidic solution. Part B If it takes 16.6 mL of 0.127 M permanganate solution to reach the equivalence point, what is the molarity of the hydrogen peroxide solution?
The concentration of hydrogen peroxide in a solution is determined by titration with a 0.1258 M Ce++ solution. The balanced net ionic equation for the reaction is: 2ce4+ (aq) + H2O2(aq) + 2H20(1)— 2Ce3+ (aq) + O2(g) + 2H30+ (aq) (a) If 18.37 mL of the 0.1258 M Ce4+ solution are needed to react completely with 40.00 mL of the hydrogen peroxide solution, what is the concentration of the hydrogen peroxide solution? M (b) Which of the two solutions was...
The concentration of a Fe2+ solution is determined by titrating it with a 0.1462 M solution of Ce4+. The balanced net ionic equation for the reaction is shown below. Ce4+(aq) + Fe2+(aq) Ce3+(aq) + Fe3+(aq) In one experiment, 16.48 mL of the 0.1462 M Ce4+ solution is required to react completely with 25.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
can you please answer this one, the first one I posted the answer was wrong. Potassium permanganate in acidic solution is used to titrate a solution of hydrogen peroxide, with which it reacts according to 2MnO4 (aq) + 5H2O2(aq)+6H30+(aq)—>2Mn2+(aq) + 502(g)+14H2O(1) A potassium permanganate solution is prepared by dissolving 22.00 g of KMnO4 in water and diluting to a total volume of 1.000 L. A total of 20.27 mL of this solution is required to reach the endpoint in a...
Permanganate ion oxidizes hydrogen peroxide in acidic solution according to the following equation: 2 MnO4–(aq) + 5 H2O2(aq) + 6 H+(aq) 2 Mn2+(aq) + 5 O2(g) + 8 H2O(l) If 35.0 mL of an acidic 0.150 M KMnO4 solution is required to consume all the H2O2 in 50.0 mL of a disinfectant solution, what is the concentration of H2O2 in the disinfectant? 0.0420 M 0.105 M 0.263 M 0.368 M When a solution of barium hydroxide is mixed with a...
TUTOR Redox Titrations The concentration of Fe in a solution is determined by titrating it with a 0.1613 M Ce solution. The balanced net ionic equation for the reaction is: Ce (aq)+ Fe(aq)-- Ce"(aq)+ Fe"(aq) In one experiment, 18.89 mL of the 0.1613-M Ce solution. solution is required to react completely with 30.00 ml. of the Fe solution. Calculate the concentration of the Fe M Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 6 item attempts remaining