I am sort of confused on how to do solubility problem calculations.
When does the concentration of ions equal the molarity and when do you have to calculate it?
For example from this problem: "The Ksp of AgI in aq sol is 10^-16mol/L. If a 10^5 M soln of AgNo3 is saturated with AgI, what is the final concentration of iodine ion?" In the solution it says that the concentration Ag ion in AgNO3 is 10^5 mol/L.
My question is how do we know when the ion concentration is the same and when do we calculate it?
Also, I dont understand the reasoning behind the solution to this problem:
"The resulting soln made from the combination of 50mL of 1M LiOH with 50mL of 1M HBr will be identical in all respects to 100mL of": Answer: .5M LiBr
to solve this what i did was use MV+MV=MV and I added 50mL and 50mL to get 100mL find that they are equal. Why did they just use one of them?
thanks so much!!
When does the concentration of ions equal the molarity and when do you have to calculate it?
For example from this problem: "The Ksp of AgI in aq sol is 10^-16mol/L. If a 10^5 M soln of AgNo3 is saturated with AgI, what is the final concentration of iodine ion?" In the solution it says that the concentration Ag ion in AgNO3 is 10^5 mol/L.
My question is how do we know when the ion concentration is the same and when do we calculate it?
Also, I dont understand the reasoning behind the solution to this problem:
"The resulting soln made from the combination of 50mL of 1M LiOH with 50mL of 1M HBr will be identical in all respects to 100mL of": Answer: .5M LiBr
to solve this what i did was use MV+MV=MV and I added 50mL and 50mL to get 100mL find that they are equal. Why did they just use one of them?
thanks so much!!
