The following aqueous solutions are mixed: 90.0 mL of 0.100 M HCL and 80.0 mL of 0.100 AgNO3.
a) Before any reaction occurs, identify each ion and determine the moles of that ion.
- I think the ions would be Ag+, NO3-, H+, and Cl- . Not sure how I determine the moles of each ion. Do I use the equation n(moles) = M(molarity) * V(volume) ?
b) Write the net ionic equation for the reaction that occurs.
- Think I've got this one. Ag
+ + Cl
- AgCl
c) After the reaction has occurred and assuming that it goes to completion, determine the moles of each ion still present in solution.
- Running into the same problem here as part "a"
d) obtain 80 mL of 0.100 K2CO3 and identify new ions and the number of moles of any new ion.
- the ions would be K
+ and CO3
2- , right?
e) Add the solution from "d" to the mixture in step "c" . Write the net ionic equation for the next reaction that occurs
- I don't understand how to know what the products will be if I add K2CO3 to the original solution.
f) After the reaction has occurred and assuming it goes to completion, determine the moles of each ion whose amount in solution has changed.
I apologize for the all the questions. My professor is not having office hours today due to an unusual circumstance. I appreciate any help.