1
JEE Main 2022 (Online) 25th July Evening Shift
+4
-1

$${K_{{a_1}}}$$, $${K_{{a_2}}}$$ and $${K_{{a_3}}}$$ are the respective ionization constants for the following reactions (a), (b) and (c).

(a) $${H_2}{C_2}{O_4} \mathbin{\lower.3ex\hbox{\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}}} {H^ + } + H{C_2}O_4^ -$$

(b) $$H{C_2}O_4^ - \mathbin{\lower.3ex\hbox{\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}}} {H^ + } + H{C_2}O_4^{2 - }$$

(c) $${H_2}{C_2}O_4^{} \mathbin{\lower.3ex\hbox{\buildrel\textstyle\rightarrow\over {\smash{\leftarrow}\vphantom{_{\vbox to.5ex{\vss}}}}}} 2{H^ + } + {C_2}O_4^{2 - }$$

The relationship between $${K_{{a_1}}}$$, $${K_{{a_2}}}$$ and $${K_{{a_3}}}$$ is given as

A
$${K_{{a_3}}}$$ $$=$$ $${K_{{a_1}}}$$ $$+$$ $${K_{{a_2}}}$$
B
$${K_{{a_3}}}$$ $$=$$ $${K_{{a_1}}}$$ $$-$$ $${K_{{a_2}}}$$
C
$${K_{{a_3}}}$$ $$=$$ $${K_{{a_1}}}$$ $$/$$ $${K_{{a_2}}}$$
D
$${K_{{a_3}}}$$ $$=$$ $${K_{{a_1}}}$$ $$\times$$ $${K_{{a_2}}}$$
2
JEE Main 2022 (Online) 30th June Morning Shift
+4
-1

The equilibrium constant for the reversible reaction

2A(g) $$\rightleftharpoons$$ 2B(g) + C(g) is K1

$${3 \over 2}$$A(g) $$\rightleftharpoons$$ $${3 \over 2}$$B(g) + $${3 \over 4}$$C(g) is K2.

K1 and K2 are related as :

A
$${K_1} = \sqrt {{K_2}}$$
B
$${K_2} = \sqrt {{K_1}}$$
C
$${K_2} = K_1^{3/4}$$
D
$${K_1} = K_2^{3/4}$$
3
JEE Main 2022 (Online) 29th June Morning Shift
+4
-1

The solubility of AgCl will be maximum in which of the following?

A
0.01 M KCl
B
0.01 M HCl
C
0.01 M AgNO3
D
Deionised water
4
JEE Main 2022 (Online) 24th June Evening Shift
+4
-1

For a first order reaction, the time required for completion of 90% reaction is 'x' times the half life of the reaction. The value of 'x' is

(Given : ln 10 = 2.303 and log 2 = 0.3010)

A
1.12
B
2.43
C
3.32
D
33.31
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