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The solubility product of different sparingly soluble salts are:
(i) XY = 4x10-20
(ii) X2Y = 3.2x10-11
(iii) XY3 = 2.7 x 10-31
The increasing order of solubility is:
(i) XY = 4x10-20
(ii) X2Y = 3.2x10-11
(iii) XY3 = 2.7 x 10-31
The increasing order of solubility is:
- a)(i),(iii),(ii)
- b)(ii),(i),(iii)
- c)(i),(ii),(iii)
- d)(iii),(i),(ii)
Correct answer is option 'A'. Can you explain this answer?
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The solubility product of different sparingly soluble salts are:(i)XY ...
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The solubility product of different sparingly soluble salts are:(i)XY ...
Increasing order of solubility can be determined by comparing the solubility product constants (Ksp) of the given sparingly soluble salts.
The solubility product constant (Ksp) is a measure of the extent to which a sparingly soluble salt dissolves in water. It is a mathematical expression of the equilibrium between the dissolved ions and the undissolved salt in a saturated solution.
The solubility product constant (Ksp) is given by the equation:
Ksp = [X+]a[Y-]b
where [X+] and [Y-] are the concentrations of the cation X+ and anion Y- in the saturated solution, and a and b are the stoichiometric coefficients of the cation and anion in the balanced equation of the dissolution reaction.
Comparing the given solubility product constants (Ksp):
(i) XY = 4x10-20
(ii) X2Y = 3.2x10-11
(iii) XY3 = 2.7x10-31
The solubility product constants can be compared by considering the magnitude of the values.
- The higher the value of Ksp, the more soluble the salt is, as it indicates a higher concentration of the ions in the saturated solution.
- The lower the value of Ksp, the less soluble the salt is, as it indicates a lower concentration of the ions in the saturated solution.
In this case, we can see that the solubility product constant of XY3 (2.7x10-31) is the lowest among the given salts. This indicates that XY3 is the least soluble salt among the three.
Comparing the remaining two salts, XY (4x10-20) and X2Y (3.2x10-11), we can see that XY has a lower solubility product constant than X2Y. This indicates that XY is less soluble than X2Y.
Therefore, the increasing order of solubility is (i) XY, (ii) X2Y, and (iii) XY3.
Hence, the correct answer is option 'A' - (i), (iii), (ii).
The solubility product constant (Ksp) is a measure of the extent to which a sparingly soluble salt dissolves in water. It is a mathematical expression of the equilibrium between the dissolved ions and the undissolved salt in a saturated solution.
The solubility product constant (Ksp) is given by the equation:
Ksp = [X+]a[Y-]b
where [X+] and [Y-] are the concentrations of the cation X+ and anion Y- in the saturated solution, and a and b are the stoichiometric coefficients of the cation and anion in the balanced equation of the dissolution reaction.
Comparing the given solubility product constants (Ksp):
(i) XY = 4x10-20
(ii) X2Y = 3.2x10-11
(iii) XY3 = 2.7x10-31
The solubility product constants can be compared by considering the magnitude of the values.
- The higher the value of Ksp, the more soluble the salt is, as it indicates a higher concentration of the ions in the saturated solution.
- The lower the value of Ksp, the less soluble the salt is, as it indicates a lower concentration of the ions in the saturated solution.
In this case, we can see that the solubility product constant of XY3 (2.7x10-31) is the lowest among the given salts. This indicates that XY3 is the least soluble salt among the three.
Comparing the remaining two salts, XY (4x10-20) and X2Y (3.2x10-11), we can see that XY has a lower solubility product constant than X2Y. This indicates that XY is less soluble than X2Y.
Therefore, the increasing order of solubility is (i) XY, (ii) X2Y, and (iii) XY3.
Hence, the correct answer is option 'A' - (i), (iii), (ii).
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The solubility product of different sparingly soluble salts are:(i)XY = 4x10-20 (ii) X2Y = 3.2x10-11 (iii) XY3= 2.7 x 10-31The increasing order of solubility is:a)(i),(iii),(ii)b)(ii),(i),(iii)c)(i),(ii),(iii)d)(iii),(i),(ii)Correct answer is option 'A'. Can you explain this answer?
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