Calculate Ionic Strength of Ca2+ in 0.01M CaCO3 Solution

In summary, the conversation discusses calculating the ionic strength of Ca2+ in a 0.01M CaCO3 solution using the equation u=0.5 sum(Mi)(zi)^2, where M is the concentration and z is the charge of the species. The question is whether or not to include CO3^2- in the calculation, to which the expert responds that ionic strength is defined for the entire solution and not for individual species. However, it is suggested to calculate the contribution of Ca2+ alone (0.02M) to address the questioner's intent. The expert also recommends informing the questioner that ionic strength is not defined for individual species.
  • #1
higherme
129
0
Calculate the ionic strength of Ca2+ in a 0.01M CaCO3 solution.

equation to use is:

u=0.5 sum(Mi)(zi)^2
where M is the concentration and z is the charge of the species

my question is when I am calculating the ionic strength of Ca2+, do I have to include
CO3^2- that is in that solution?

so, it would be :

U=0.5 (0.01M Ca2+)(2+)^2 + (0.01M CO3^2-)(2-)^2
U=0.04M

if I don't include:
U=0.5 (0.01M Ca2+)(2+)^2
U=0.02M
 
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  • #2
higherme said:
Calculate the ionic strength of Ca2+ in a 0.01M CaCO3 solution.
The question is meaningless to me. The ionic strength is defined for the entire solution, not for individual species.

As meaningless as it may be, it appears that the questioner what's you to calculate the contribution of Ca2+ alone (your second calculation). But this is just my interpretation of intent.

If you get a chance, please inform the person that wrote this question that ionic strength is not defined for individual species. If this is from a book, please cite the title, author, edition and page number.
 
  • #3


I would include both Ca2+ and CO3^2- in the calculation of ionic strength since they are both present in the solution and contribute to the overall ionic strength. The equation for ionic strength takes into account the concentration and charge of all ionic species present in a solution, so it is important to include all relevant ions in the calculation. Therefore, the correct calculation would be:

U=0.5 (0.01M Ca2+)(2+)^2 + (0.01M CO3^2-)(2-)^2
U=0.04M

This means that the ionic strength of Ca2+ in a 0.01M CaCO3 solution is 0.04M.
 

1. How do you calculate the ionic strength of a solution?

The ionic strength of a solution is calculated by summing the concentration of all ions in the solution, multiplied by their respective charges squared.

2. What is the formula for calculating the ionic strength of a solution?

The formula for calculating the ionic strength of a solution is Σ(ci * zi^2), where ci is the concentration of each ion and zi is the charge of each ion.

3. How do you determine the concentration of Ca2+ in a 0.01M CaCO3 solution?

To determine the concentration of Ca2+ in a 0.01M CaCO3 solution, you can use the solubility product constant (Ksp) of CaCO3 to calculate the concentration of Ca2+ ions present in the solution.

4. Is the ionic strength of a solution affected by temperature?

Yes, the ionic strength of a solution can be affected by temperature. As temperature increases, the solubility of certain compounds may change, thus altering the concentration of ions in the solution and ultimately affecting the ionic strength.

5. How does the ionic strength of a solution impact chemical reactions?

The ionic strength of a solution can impact chemical reactions by influencing the activity and behavior of ions in the solution. High ionic strength can decrease the activity of ions, while low ionic strength can increase their activity. This, in turn, can affect reaction rates and equilibrium constants.

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