Home
Class 11
CHEMISTRY
In a reaction, Cr(2)O(7)^(2-) is reduced...

In a reaction, `Cr_(2)O_(7)^(2-)` is reduced to `Cr^(3+)`. What is concentration of `0.1M K_(2)Cr_(2)O_(7)` in equivalent per litre?
`Cr_(2)O_(7)^(2-)+14H^(+)+6erarr2Cr^(3+)+7H_(2)O`

Promotional Banner

Similar Questions

Explore conceptually related problems

In a redox reaction, dichromate ion (Cr_(2)O_(7)^(2-)) is reduced to Cr^(3+) ion, the equivalent mass of K_(2)Cr_(2)O_(7) in this reaction is :

A 100 mL sample of water was treated to convert any iron present to Fe^(2+) . Addition of 25 mL of 0.002 M K_(2)Cr_(2)O_(7) resulted in the reaction : 6Fe^(2+)+Cr_(2)O_(7)^(2-)+14H^(+)rarr6Fe^(3+)+2Cr^(3+) + 7H_(2)O The excess K_(2)Cr_(2)O_(7) was back-titrated with 7.5 mL of 0.01 M Fe^(2+) solution. Calcution the parts per million (ppm) of iron in the water sample.

How many moles of electrons are involved in the conversion of 1 mol Cr_(2)O_(7)^(2-) into Cr^(3+) ion? Cr_(2)O_(7)^(2-)+14H^(+)+6e^(-) to 2Cr^(3+)+7H_(2)O

In laboratory K_(2)Cr_(2)O_(7) is used mainly not Na_(2)Cr_(2)O_(7). Why?

A 100 mL sample of water was treated to convert any iron present to Fe^(2+) . Addition of 25mL of 0.002M K_(2)Cr_(2)O_(7) resulted in the reaction. 6Fe^(2+)+Cr_(2)O_(7)^(2-)+14H^(+) to 6Fe^(3+)+2Cr^(3+)+7H_(2)O The excess K_(2)Cr_(2)O_(7) was back- titrated with 7.5mL of .01M Fe^(2+) solution. Calculate the parts per million (ppm) of iron in the water sample.