Equilibrium of a Sparingly Soluble Ionic Compound

In summary, equilibrium in the context of a sparingly soluble ionic compound refers to a state in which the rate of dissolution is equal to the rate of precipitation. The solubility of such compounds can be determined experimentally or calculated using the solubility product constant. Factors such as temperature, pressure, and other ions in the solution can affect the solubility, and changing these conditions can disturb the equilibrium. Additionally, the solubility can also be affected by the pH of the solution. Basic compounds will be more soluble in acidic solutions and less soluble in basic solutions.
  • #1
daphnelee-mh
66
4
Homework Statement
I can't get the correct answer, isn't it if Ksp>[Mn2+][OH-]^2, there is no precipitation. How to get the specific concentration of [OH-]?
Relevant Equations
Kb = [NH4+][OH-]/[NH3]
Ksp=[Mn2+][OH-]^2
1572962999036.png

Answer given is 6.61g.
 
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  • #2
You are looking for the highest concentration of OH- that doesn't produce precipitation, don't you?
 
  • #3
chemistry.jpeg


May I know which step is wrong? thanks
 
  • #4
You have worked out the concentration in g/L. What is the mass in the actual solution?
 
  • #5
chemistry.jpeg


Is this correct ? thanks.
 
  • #6
It is not quite equal to the given answer; I think that's because you rounded off [OH-] to 1.4e-6 M instead of 1.435e-6 M. Keep the extra digits through the calculation, and round off to the appropriate sig figs at the end.
 

Related to Equilibrium of a Sparingly Soluble Ionic Compound

1. What is meant by equilibrium of a sparingly soluble ionic compound?

The equilibrium of a sparingly soluble ionic compound refers to the state where the amount of dissolved ions in a solution is equal to the amount of ions that are precipitated out of the solution. This is a dynamic equilibrium where the rate of dissolution is equal to the rate of precipitation.

2. How is the equilibrium of a sparingly soluble ionic compound affected by temperature?

The solubility of a sparingly soluble ionic compound generally increases with an increase in temperature. This means that at higher temperatures, more of the compound will dissolve in the solution. However, there are some exceptions to this rule, and the solubility may decrease with an increase in temperature for certain compounds.

3. What factors influence the equilibrium of a sparingly soluble ionic compound?

The solubility of a sparingly soluble ionic compound is affected by several factors, including temperature, pressure, and the presence of other substances in the solution. The nature of the compound itself, such as its ionic charge and size, also plays a role in its solubility.

4. How is the equilibrium of a sparingly soluble ionic compound calculated?

The equilibrium of a sparingly soluble ionic compound can be calculated using the solubility product constant (Ksp), which is a measure of the compound's solubility at a given temperature. The Ksp is calculated by multiplying the concentrations of the dissolved ions raised to the power of their respective coefficients in the solubility equation.

5. What is the significance of the equilibrium of a sparingly soluble ionic compound?

The equilibrium of a sparingly soluble ionic compound is important because it determines the concentration of ions in a solution, which can have implications for the chemical reactions and processes that occur in that solution. It also helps to predict how much of the compound will dissolve in a particular solvent under specific conditions.

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