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AgCI is soluble in:...

`AgCI` is soluble in:

A

aqua regia

B

`H_(2)SO_(4)`

C

dil `HCI`

D

aq. `NH_(3)`

Text Solution

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The correct Answer is:
D
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The solubility product of a soluble salt A_(x)B_(y) is given by : K_(sp)=[A^(y+)]^(z)[B^(x-)]^(y) . As soon as prodcut of concentration of A^(y+) and B_(x-) . Becomes more than its K_(sp) , the salt starts precipitation. It may practically be noticed that AgCI is more soluble in water and its solubility decreases dramatically in 0.1m NaCI or 0.1 m AgNO_(3) solution. It can be concluded that in presence of a common ion the solubility of salt decreases. Which of the following statements wrong?

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The solubility product of a soluble salt A_(x)B_(y) is given by : K_(sp)=[A^(y+)]^(z)[B^(x-)]^(y) . As soon as prodcut of concentration of A^(y+) and B_(x-) . Becomes more than its K_(sp) , the salt starts precipitation. It may practically be noticed that AgCI is more soluble in water and its solubility decreases dramatically in 0.1m NaCI or 0.1 m AgNO_(3) solution. It can be concluded that in presence of a common ion the solubility of salt decreases. Equal volumes of two solutions are mixed. The one in which CaSO_(4)(K_(sp)=2.4xx10^(-5)) is precipitated is :

The solubility product of a soluble salt A_(x)B_(y) is given by : K_(sp)=[A^(y+)]^(z)[B^(x-)]^(y) . As soon as prodcut of concentration of A^(y+) and B_(x-) . Becomes more than its K_(sp) , the salt starts precipitation. It may practically be noticed that AgCI is more soluble in water and its solubility decreases dramatically in 0.1m NaCI or 0.1 m AgNO_(3) solution. It can be concluded that in presence of a common ion the solubility of salt decreases. The pH of a saturated solution of Mg (OH)_(2) is : (K_(sp)Mg(OH)_(2)=1xx10^(-11)

The solubility product of a soluble salt A_(x)B_(y) is given by : K_(sp)=[A^(y+)]^(z)[B^(x-)]^(y) . As soon as prodcut of concentration of A^(y+) and B_(x-) . Becomes more than its K_(sp) , the salt starts precipitation. It may practically be noticed that AgCI is more soluble in water and its solubility decreases dramatically in 0.1m NaCI or 0.1 m AgNO_(3) solution. It can be concluded that in presence of a common ion the solubility of salt decreases. The salting out action of RCOONa (soap) in presence of NaCI is based on :

The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y) . As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP) , the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases. Equal volumes of two solutions are mixed. The one in which CaSO_(4) (K_(SP)= 2.4xx10^(-5)) is precipitated, is :

The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y) . As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP) , the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases. The salting out action of RCOONa in presence of NaCI is based on:

The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y) . As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP) , the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases. The volume of water neede to dissolve 1g BaSO_(4)(K_(SP)= 1xx10^(-10)) is:

The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y) . As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP) , the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases. The pH of a saturated solution of Mg(OH)_(2) is: (K_(SP) of Mg(OH)_(2)= 1xx10^(-11))

GRB PUBLICATION-SALT ANALYSIS-D.Class-A Subgroup-II Acidic Radicals
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  12. Nitrates of all the metals except mercury and bismuth are:

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  14. Which of the following thermal decomposition yields a basic as well as...

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