Concept explainers
Interpretation:
The compoundsthatprecipitate out firstand last areto be identified with given concentration of ions.
Concept introduction:
The amount of solute dissolved in a given volume of the solvent to form a saturated solution at a given temperature is termed as the solubility of the solute in the solvent at that temperature.
The solubility product of a sparingly soluble salt is given as the product of the concentration of the ions raised to the power equal to the respective stoichiometric coefficients after the dissociation of the electrolyte.
Number of moles of solute dissolved per litre of solution is called molar solubility.
The unit of molar solubility is
Molar solubility can be evaluated from the solubility product constant
When equilibrium is reached between a solid and its constituent ions in a solution, it is known as the solubility product constant
At a given temperature, the product of molar concentrations of the ions of salt present in the solution is known as the solubility product of the salt. It is represented by
Higher is the value of solubility product of a salt, more is its solubility.
The presence of common ions in the solution decreases the solubility of a given compound.
For a general reaction:
The solubility product can be calculated by the expression as:
Here,
The solubility product
The more the molar concentration of the ions, the more time it’ll take to precipitate. The less the molar concentration of the ions, the lesser time it’ll take to precipitate.
Answer to Problem 118AP
Solution: No, comparison of two salts with similar formulas that have the same number of cations and anions is possible.
Explanation of Solution
Given information: The concentration of
The compound
The equation for the dissociation of
Consider
The concentration of
The ICE table for theionization of
The equilibrium expression for a reaction is written as follows:
Here,
Substitute the values of
The value of
On solving further,
The concentration of
Hence, the concentration of
The equation for the dissociation of
The concentration of
The ICE tablefor the ionisation of
Consider
The equilibrium expression for a reaction is written as follows:
Here,
Substitute the values of
The value of
The concentration of
Hence, the concentration of
The equation for the dissociation of
The concentration of
The ICE table for the ionisation of
Consider
The equilibrium expression for a reaction is written as follows:
Here,
Substitute the values of
The value of
The concentration of
Hence, the concentration of
The order of precipitation depends upon the molar concentration of
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Chapter 17 Solutions
Chemistry
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