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Question

If $$E_{CIO_3/CIO_4}^0=0.36 V$$ and $$E_{CIO_3/CIO_2}^0=0.33 V$$ at $$300K$$.The equilibrium concentration of perchlorate ion $$(CIO_4^-)$$ which was initially $$1.0$$M in $$CIO_3^-$$ when the reaction starts to attains the equilibrium ,
$$2ClO_^- \rightleftharpoons CIO_3^-+ClO_4^-$$
Given :$$AL(0.509)=3.329$$

A
$$0.0236M$$
B
$$0.0190M$$
C
$$0.123M$$
D
$$0.191M$$
Solution
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Correct option is A. $$0.0236M$$

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Similar Questions
Q1
In the following process of disproportionation:
$$\underset {Chlorate\ ion}{2ClO_{3}^{-}} \rightleftharpoons ClO_{2}^{-} + \underset {Per\ chlorate\ ion}\ E^{\circ}_{ClO_{4}^{-}}/ ClO_{3}^{-}} = + 0.36\ V$$
$$E^{\circ}_{ClO_{3}^{-}}/ ClO_[2}^{-}} = + 0.33\ V$$
Initial concentration of chlorate ion was $$0.1\ M$$. The equilibrium concentration of perchlorate ion will be ?
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Q2
EoClO4/ClO3 and EoClO3/ClO2 are+0.36V and +0.33Vrespectively. The equilibrium concentration of per chlorate ion for the given reaction would be:

2ClO3ClO2+ClO4
t=0 0.1 M 0 0

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Q3
The chlorate ion can disproportionate in basic solution according to reaction,
2ClO3ClO2+ClO4
The concentration of chlorate ion present initially is 0.1 M.
The equilibrium concentration of perchlorate ions at 298 K is x. What is the value of 1x?
Given : EClO4|ClO3=0.36V and EClO3|ClO2=0.33.V At 298 KRTF=0.06 V10=3.16

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Q4
The chlorate ion can disproportionate in basic solution according to reaction,
2ClO3ClO2+ClO4
what is the equilibrium concentration of perchlorate ions from a solution initially at 0.1 M in chlorate ions at 298 K?
Given that :EClO4|ClO3=0.36 V and EClO3|ClO2=0.33 V at 298 K.

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Q5
The type of hybrid orbitals used by chlorine atom in $$CIO^-$$, $${ CIO }_{ 2 }^{ - }$$ $${ CIO }_{ 3 }^{ - }$$ and $${ CIO }_{ 4 }^{ - }$$ is/are :
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