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For the reaction $ 2 NO_{2(g)} \rightleftharpoons 2 NO_{(g)} + O_{2(g)} Kc = 1.8 \times 10 ^ {-6} at 184 ^\circ c R = 0.0831 KJ/mol.K $ When $ K_P and K_C are compared at 184 ^\circ C $ it is found that :
$ K_p = Kc ( RT) ^ { \triangle n (g) } \triangle n (g) = 1 $ $ = Kc \times 0.0831 \times 457 it means Kp \gt Kc $
Water is a
Water is an amphiprotic solvent as it can accept protons as well as give protons.
Ammonium ion is
Ammonium ion $ (NH _4 ^ +) is a conjugate acid of NH_3 $ $ NH_3 + H_2O \rightleftharpoons NH_4 ^ + + OH ^ - $ Bronsted base Conjugate acid
Species acting both as bronsted acid and a base is
$ HSO_4 ^ - $ can act as a bronsted acid as well as bronsted base. $ HSO_4 ^ - + H_2 O \rightleftharpoons SO_4 ^ {2-} + H_3 ^ + O $ Acid $ HSO_4 ^ - + H_2 O \rightleftharpoons H_2 SO_4 + OH^ - $ Base
A solution ofan acid has $ P^H = 4.70 find out the concentration of OH ^- pK_w =14 $
$ P ^ H = 4.7 \therefore [ H_3 ^ + O ] = 1.995 \times 10 ^ {-5} pK_w = 14 \therefore K_w = 1 \times 10 ^ {-14} $ $ = - log [ H_3 ^ + O ] Now K_w = [ H_3 ^ + O ] [ OH^- ] $ $ \therefore [OH^-] = { 1 \times 10 ^ { -14} \over 1.995 \times 10 ^ {-5} } = 5 \times 10 ^ {-10} M $
The conjugate base of $ H_2PO^- _4 $ is
Conjugate base of $ H_2 PO_4 ^ - is HPO_4 ^ {2-} $ $ H_2 PO_4 ^ - + H_2 O \rightleftharpoons HPO_4 ^ {2-} + H_3 O ^ + $ Acid
What is the conjugate base of $OH ^ - $ ?
Conjugate base of $ OH^- $ $ OH^- + H_2 O \rightleftharpoons O ^ {2-} + H_3 O ^ + $
An example for lewis acid is
Lewis acid always accepts a pair of $ e ^ - here AlCl_3 accepts a pair of e ^ - $ .
Which of the following molecule act as a lewis acid ?
$ (CH_3)_3 B accept a pair of e ^ - $ so lewis acid
In a given system, water and ice are in equilibrium. If pressure is applied to the above system, then,
Pressure on equilibrium system increases ,so volume decreases. volume
of ice is more than liquid $ H_2O$ so more ice is malted
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The bank mixes NEET previous year questions (PYQs) with practice questions, each tagged with its exam appearances where applicable.