When ammonia is added to water,which of the f | vedclass

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Question

(A) Ammonia $(NH_3)$ is a weak base that reacts with water as follows:$NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq)$In this reaction,$N

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$OH^-$

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(A) Ammonia $(NH_3)$ is a weak base that reacts with water as follows:$NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq)$In this reaction,$NH_3$ accepts a proton from water to form the ammonium ion $(NH_4^+)$ and releases hydroxide ions $(OH^-)$.The increase in the concentration of $OH^-$ ions makes the solution basic,which leads to a decrease in the concentration of $H_3O^+$ ions due to the ionic product of water $(K_w = [H_3O^+][OH^-])$.Therefore,the $OH^-$ ion is responsible for the change.

$A$. $HI$	$(i)$ $3.2 \times 10^9$
$B$. $HF$	$(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$	$(iii)$ $1.3 \times 10^6$
$D$. $HBr$	$(iv)$ $1.0 \times 10^9$

When ammonia is added to water,which of the following ions is responsible for the increase in its basicity (or decrease in $H_3O^+$ concentration)?

Similar Questions

Calculate the dissociation constant of a $0.001 \ M$ weak monoacidic base undergoing $2 \%$ dissociation.

Arrange the following species in the decreasing order of their basic strength: $(a) OH^{-}, (b) NH_2^{-}, (c) F^{-}$.

Match the given ionisation constant values with the corresponding acids.
$A$. $HI$ $(i)$ $3.2 \times 10^9$
$B$. $HF$ $(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$ $(iii)$ $1.3 \times 10^6$
$D$. $HBr$ $(iv)$ $1.0 \times 10^9$

The correct match is:

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Give the conjugate acid of the following species: $HS^{-}, NH_{3}, C_{6}H_{5}COO^{-}, OH^{-}$

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