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27 Nov 2019

Add 2 mL of sodium hydroxide to 1 mL of potassium permanganate. Then add hydrogen peroxide until the color change is complete. From the change in color, identify the manganese product. What is the formula? [Is it MnO2??]What evidence indicates the product from hydrogen peroxide? [is it bubbles that indicated the product is O2???]Complete the redox reaction and balance it under acidic conditions:MnO4- + H2O2-->

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Casey DurganLv2

14 Feb 2019

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H₂O₂+MnO_4^1-=Mn^₂₊+O₂inan acidic solution

Withthe above balanced chemical reaction and the stoichiometricrelationship between hydrogen peroxide and permanganate ion, 1.900grams of a hydrogen peroxide solution requires 14.65 mL of a0.02500 M solution of potassium permanganate solution to reach theequivalence point.

1.How many moles of potassium permanganate or permanganate ion areneeded to reach the equivalence point?

2.After calculation of the moles of permanganate ion used to reachthe equivalence point; how many moles of hydrogen peroxide weretitrated?

3.From the moles of hydrogen peroxide titrated, use the molar mass ofhydrogen peroxide to determine the mass of hydrogen peroxidetitrated.

4.The percent by mass of a solution is defined as the mass of thesolute divided by the mass of the solution x 100.
If1.900 grams of a hydrogen peroxide solution requires 14.65 mL of a0.02500 M solution of potassium permanganate solution to reach theequivalence point. What is the percent by mass of the hydrogenperoxide solution?

I am working on this lab but can't seem to figure out how tofinish it.

1. For the NEW bottle of hydrogenperoxide, record and calculate the following:

a	Volumeof potassium permanganate used in each titration (mL)	50mL
b	Thevolume of potassium permanganate required to titrate 10 mL of thenew hydrogen peroxide (mL)	18.04mL
c	How many moles of potassiumpermanganate were required to titrate 10mL of the new hydrogenperoxide (moles)	0.013mol
d	Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles)
e	How many grams ofH₂O₂ were in the hydrogen peroxide solution(MW of H₂O₂ is 34.01) (grams)
f	1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the NEW solution. (% mass = (mass H2O2 /mass water) * 100%)

2. Repeat the calculations for the OLD bottle ofH₂O₂:

a	Volumeof potassium permanganate used in each titration (mL):	50mL
b	Thevolume of potassium permanganate required to titrate 10 mL of theold hydrogen peroxide (mL)	12.60mL
c	How many moles of potassiumpermanganate were required to titrate 10mL of the old hydrogenperoxide (moles)	0.013mol
d	Given the stoichiometry of thereaction, how many moles of hydrogen peroxide were in the 10mL ofthe solution (moles)
e	How many grams ofH₂O₂ were in the hydrogen peroxide solution(MW of H₂O₂ is 34.01) (grams)
f	1 mL ofwater weighs 1 g. Using this information and the numberof grams of H2O2 produced in the reaction, calculate the percentmass of H2O2 in the OLD solution. (% mass = (mass H2O2 /mass water) * 100%)

azureantelope319

Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings:
1) Write down the balanced chemical equation for this reaction.

2) Define the type/types of the reaction; assign the oxidation number of Manganese in potassium permanganate and manganese (II) sulfate. Also, offer an explanation for the color change.

3) Write down the ions present in the solution before & after the reaction. If 100 mL 0.5 M potassium permanganate was mixed with 50 mL 2 M sulfuric acid, what will be the final pH (>7 or <7) of the solution?

4) After the completion of reaction, when evolution of gas-bubbles ceased, what will happen if an aqueous solution of sodium carbonate was added to the reaction mixture? Please write down the net ionic equation.

5) If initially 5.65 g of potassium permanganate was taken for the reaction, calculate the total mass of manganese (II) sulfate present in the solution after the completion of the reaction. What is the Manganese ion concentration of the solution (assume that the total volume of the final reaction mixture is 500 mL)?

Useful hints: hydrogen peroxide is a strong oxidizing agent and considered to be a molecular compound

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