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 solution of iron(III) chloride, what is observed?
Precipitation of a colored solid |
||
Precipitation of a colorless solid |
||
Evolution of a colorless gas |
||
Neither precipitation nor gas evolution |
What is the coefficient for H+(aq) when the equation is balanced
with whole number
coefficients?
__Mn2+(aq) + __BiO3-(aq) +
__H+ (aq) → __Bi3+(aq) +
__MnO4–(aq) + __H2O(l)
a 3
b 14
c 4
d 7
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Permanganate ion oxidizes hydrogen peroxide in acidic solution according to the following equation: 2 MnO4–(aq) +...
by titration with permanganate solution. The 13) Hydrogen peroxide, H2O2, can be determined by titration with permans reaction is: 2 MnO4 (aq) + 5 H2O2(aq) + 6 H+ + 502(g) + 2 Mn2(aq) + 8 H20 ate 5.0 mL of a H2Oz(aq) If it required 80.0 mL of 0.0220 molar MnO4 (aq) solution to titrate 5.0 m solution, what is the molarity of the H2O2(aq) solution?
Over time, hydrogen peroxide, H2O2, degrades into water and oxygen gas. A bottle of hydrogen peroxide is expired and you need to determine the concentration. A titration is performed using the following equation: 3 H2O2(aq) + 2 NaMnO4(aq) → 3 O2(g) + 2 MnO2(aq) + 2 NaOH(aq) + 2 H2O(l) Note that permanganate ion, MnO4-, is purple, while manganese (IV) ion, Mn4+, is colorless. A quantity of 683 mL of 3.44 M NaMnO4 was measured and placed in a beaker. The solution...
I can calculate molarity. But I don't know how to balance the acidic equation. Explain just about Balancing please. Thank you much! 3. The concentration of hydrogen peroxide, H2O2, in a solution is determined by titrating a 11.5 mL sample of the solution with permanganate ion, producing Mn2+ ion and oxygen gas. Balance the chemical equation for the redox reaction that occurs in acidic solution. H2O2 + MnO4 +H+ ► 02 + H2O + Mn2+ How will you able to...
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
5. (20pts) Consider the reaction between oxalate ion and permanganate ion in acidic solution: MnO4 (aq) + C202-(aq) → Mn2+ (aq) + CO2(9) a. Balance the reaction in acidic solution b. Determine the standard cell potential of the representative voltaic cell c. Determine the standard free energy change of this reaction d. Determine the cell potential if the pH = 4 and all other solute concentrations were standard.
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.
104 ' (aq). 2. Balance the following redox equation in a acidic solution: MnO4 (aq) + As406(s) → Asos (aq) + Mn2+ (aq)
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?
2. Balance the following redox equation in a acidic solution: MnO4 (aq) + As«O6(s) → AsO4 (aq) + Mn2+(aq)
The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the balanced equation H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l)H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l) The rate of formation of the red triiodide ion, Δ[I3−]/ΔtΔ[I3−]/Δt, can be determined by measuring the rate of appearance of the color. A sequence of photographs showing the progress of the reaction of hydrogen peroxide (H2O2)(H2O2) and iodide ion (I−)(I−). As time passes (left to right), the red color due to the triiodide ion (I3−)(I3−) increases in intensity. Initial rate data...