Calculate Ksp from molar solubility.
Understand the Problem
The question is asking how to calculate the solubility product constant (Ksp) from the molar solubility of a salt. To solve this, we will typically convert the molar solubility into the Ksp expression based on the dissociation of the salt in solution.
Answer
$0.01$
Answer for screen readers
The value of the solubility product constant (Ksp) is $0.01$.
Steps to Solve
- Identify the dissociation of the salt
Determine how the salt dissociates into its ions in solution. For example, if we have a salt $AB$ that dissociates into $A^+$ and $B^-$. The dissociation can be represented as: $$ AB_{(s)} \rightleftharpoons A^+{(aq)} + B^-{(aq)} $$
- Write the expression for Ksp
The solubility product constant (Ksp) is calculated using the concentrations of the ions at equilibrium. For the example salt $AB$, the Ksp expression would be: $$ Ksp = [A^+][B^-] $$ If the molar solubility of $AB$ is denoted as $s$, then: $$ Ksp = s \cdot s = s^2 $$
- Substitute the molar solubility into the Ksp expression
If you have a specific value for the molar solubility (let’s say $s = 0.1 , mol/L$), substitute this value into the Ksp expression you derived: $$ Ksp = (0.1)^2 $$
- Calculate the value of Ksp
Now perform the calculation. For the molar solubility of $s = 0.1 , mol/L$, we compute: $$ Ksp = 0.1^2 = 0.01 $$
The value of the solubility product constant (Ksp) is $0.01$.
More Information
The solubility product constant (Ksp) is essential in chemistry as it indicates the extent to which a salt can dissolve in water. It is particularly important in understanding precipitation reactions and the solubility of salts in various conditions.
Tips
- Misidentifying the dissociation products: Always double-check the dissociation of the salt to avoid incorrect Ksp expressions.
- Forgetting the powers in the Ksp expression: Remember to use the coefficients from the balanced dissociation equation when writing the Ksp expression.
