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Question

20 mL of H2O2 reacts completely with acidified K2Cr2O7 solution. 40 mL of K2Cr2O7 solution was required to oxidise the H2O2 completely. Also, 2.0 mL of the same K2Cr2O7 solution required 5.0 mL of 1.0 M H2C2O4 solution to reach the equivalence point. Which of the following statements is/are correct?

A
The H2O2 solution is 5 M.
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B
The volume strength of H2O2 is 56 V.
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C
The volume strength of H2O2 is 112 V.
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D
If 40 mL of M8 H2O2 is further added to the 10 mL of the above H2O2 solution, the volume strength of the resulting solution is changed to 16.8 V.
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Solution

The correct options are
A The H2O2 solution is 5 M.
C If 40 mL of M8 H2O2 is further added to the 10 mL of the above H2O2 solution, the volume strength of the resulting solution is changed to 16.8 V.
D The volume strength of H2O2 is 56 V.
I. mEq of H2O2(n=2) mEq of Cr2O27(n=6)
20mL×N1=40 mL×N2 .....(i)
a. mEq of Cr2O27 mEq of C2O24(n=2)
2.0×N25.0×1.0×2
N2(Cr2O27)=5 ....(ii)
Therefore, substituting the N2 in equation (i)
20 mL×N2=40 mL×5
N1(H2O2)=10
M1(H2O2)=102=5 M
b. 1N H2O2=5.6 V
10 N H2O2=56 V
d. N1V1+N2V2=N3V3(V3=10+40=50 mL)
10×10+40×58×2=N3×50
N3(final) H2O2=3 N
The volume strength of H2O2=5.6×3=16.8 V

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