$AB\overset {{K_1}} \longleftrightarrow {A^ + } + {B^{ - 1}}$
${K_1} = \frac{{[{A^ + }][{B^ - }]}}{{[AB]}}$
$AB + {B^ - }\overset {{K_2}} \longleftrightarrow AB_2^ - $
${K_2} = \frac{{[AB_2^ - ]}}{{[AB][{B^ - }]}}$
Dividing $K_1$ and $K_2$ we get
$K = \frac{{{K_1}}}{{{K_2}}} = \frac{{[{A^ + }]{{[{B^ - }]}^2}}}{{[AB_2^ - ]}}$
$\therefore \,\frac{{[{A^ + }]}}{{[AB_2^ - ]}} = \frac{K}{{{{[{B^ - }]}^2}}}$
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$(I)\,[Kr]\,5s^1$ $(II)\, [Rn]\,5f^{14}\,6d^1\,7s^2$
$(III)\,[Ar]\,3d^{10}\,4s^2\,4p^5$ $(IV)\,[Ar]\,3d^6\,4s^2$
Consider the following Statements
$(i)\, I$ shows variable oxidation State
$(ii)\, II$ is a $d-block$ element
$(iii)$ The compound formed between $I$ and $III$ is covalent
$(iv)\,IV$ shows single oxidation state
Which Statement is True $(T)$ or False $(F)$?
$(A)$ The compound is optically active
$(B)$ The compound possesses centre of symmetry
$(C)$ The compound possesses plane of symmetry
$(D)$ The compound possesses axis of symmetry