229482
$\mathrm{H}_2 \mathrm{~S}$ gas when passed through a solutions if cations containing $\mathrm{HCl}$ precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
1 Presence of $\mathrm{HCl}$ decreases the sulphate ion concentration
2 Solubility product of group II sulphate is more than that of group IV sulphate
3 Presence of $\mathrm{HCl}$ increase the suphate ion concentration
4 Sulphate of group IV cations are unstable in $\mathrm{HCl}$
Explanation:
$\mathrm{H}_2 \mathrm{~S}$ gas is passed in presence of $\mathrm{HCl}$, in qualitative analysis of cation of second group, Therefor, due to common ion effect, lower concentration of sulphide ion is obtained which is sufficient for the precipitation of second group cation in form of their sulphides due to lower value of their solubility product $\left(\mathrm{K}_{\mathrm{sp}}\right)$. in presence of $\mathrm{HCl}$ decreases the sulphate ion concentration.
NEET-2005
Ionic Equilibrium
229487
The solubility of a saturated solution of calcium fluoride is $2 \times 10^{-4}$ moles per litre. Its solubility product is
229496
The ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$. Its product at $90^{\circ} \mathrm{C}$ will be
1 $1 \times 10^{-14}$
2 $1 \times 10^{-16}$
3 $1 \times 10^{-20}$
4 $1 \times 10^{-12}$
Explanation:
The ionic product of water increases with increases in temperature. This is because of the fact that with increase of temperature the degree of ionization of water increases. the only one option has a value greater than $10^{-14}$ ie $10^{-2}$ Hence ionic product of water at $90^{\circ} \mathrm{C}=1 \times 10^{-12}$.
229482
$\mathrm{H}_2 \mathrm{~S}$ gas when passed through a solutions if cations containing $\mathrm{HCl}$ precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
1 Presence of $\mathrm{HCl}$ decreases the sulphate ion concentration
2 Solubility product of group II sulphate is more than that of group IV sulphate
3 Presence of $\mathrm{HCl}$ increase the suphate ion concentration
4 Sulphate of group IV cations are unstable in $\mathrm{HCl}$
Explanation:
$\mathrm{H}_2 \mathrm{~S}$ gas is passed in presence of $\mathrm{HCl}$, in qualitative analysis of cation of second group, Therefor, due to common ion effect, lower concentration of sulphide ion is obtained which is sufficient for the precipitation of second group cation in form of their sulphides due to lower value of their solubility product $\left(\mathrm{K}_{\mathrm{sp}}\right)$. in presence of $\mathrm{HCl}$ decreases the sulphate ion concentration.
NEET-2005
Ionic Equilibrium
229487
The solubility of a saturated solution of calcium fluoride is $2 \times 10^{-4}$ moles per litre. Its solubility product is
229496
The ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$. Its product at $90^{\circ} \mathrm{C}$ will be
1 $1 \times 10^{-14}$
2 $1 \times 10^{-16}$
3 $1 \times 10^{-20}$
4 $1 \times 10^{-12}$
Explanation:
The ionic product of water increases with increases in temperature. This is because of the fact that with increase of temperature the degree of ionization of water increases. the only one option has a value greater than $10^{-14}$ ie $10^{-2}$ Hence ionic product of water at $90^{\circ} \mathrm{C}=1 \times 10^{-12}$.
229482
$\mathrm{H}_2 \mathrm{~S}$ gas when passed through a solutions if cations containing $\mathrm{HCl}$ precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
1 Presence of $\mathrm{HCl}$ decreases the sulphate ion concentration
2 Solubility product of group II sulphate is more than that of group IV sulphate
3 Presence of $\mathrm{HCl}$ increase the suphate ion concentration
4 Sulphate of group IV cations are unstable in $\mathrm{HCl}$
Explanation:
$\mathrm{H}_2 \mathrm{~S}$ gas is passed in presence of $\mathrm{HCl}$, in qualitative analysis of cation of second group, Therefor, due to common ion effect, lower concentration of sulphide ion is obtained which is sufficient for the precipitation of second group cation in form of their sulphides due to lower value of their solubility product $\left(\mathrm{K}_{\mathrm{sp}}\right)$. in presence of $\mathrm{HCl}$ decreases the sulphate ion concentration.
NEET-2005
Ionic Equilibrium
229487
The solubility of a saturated solution of calcium fluoride is $2 \times 10^{-4}$ moles per litre. Its solubility product is
229496
The ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$. Its product at $90^{\circ} \mathrm{C}$ will be
1 $1 \times 10^{-14}$
2 $1 \times 10^{-16}$
3 $1 \times 10^{-20}$
4 $1 \times 10^{-12}$
Explanation:
The ionic product of water increases with increases in temperature. This is because of the fact that with increase of temperature the degree of ionization of water increases. the only one option has a value greater than $10^{-14}$ ie $10^{-2}$ Hence ionic product of water at $90^{\circ} \mathrm{C}=1 \times 10^{-12}$.
229482
$\mathrm{H}_2 \mathrm{~S}$ gas when passed through a solutions if cations containing $\mathrm{HCl}$ precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
1 Presence of $\mathrm{HCl}$ decreases the sulphate ion concentration
2 Solubility product of group II sulphate is more than that of group IV sulphate
3 Presence of $\mathrm{HCl}$ increase the suphate ion concentration
4 Sulphate of group IV cations are unstable in $\mathrm{HCl}$
Explanation:
$\mathrm{H}_2 \mathrm{~S}$ gas is passed in presence of $\mathrm{HCl}$, in qualitative analysis of cation of second group, Therefor, due to common ion effect, lower concentration of sulphide ion is obtained which is sufficient for the precipitation of second group cation in form of their sulphides due to lower value of their solubility product $\left(\mathrm{K}_{\mathrm{sp}}\right)$. in presence of $\mathrm{HCl}$ decreases the sulphate ion concentration.
NEET-2005
Ionic Equilibrium
229487
The solubility of a saturated solution of calcium fluoride is $2 \times 10^{-4}$ moles per litre. Its solubility product is
229496
The ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$. Its product at $90^{\circ} \mathrm{C}$ will be
1 $1 \times 10^{-14}$
2 $1 \times 10^{-16}$
3 $1 \times 10^{-20}$
4 $1 \times 10^{-12}$
Explanation:
The ionic product of water increases with increases in temperature. This is because of the fact that with increase of temperature the degree of ionization of water increases. the only one option has a value greater than $10^{-14}$ ie $10^{-2}$ Hence ionic product of water at $90^{\circ} \mathrm{C}=1 \times 10^{-12}$.
