When 100 ml of 1.0 m na3po4 is mixed with 100 ml of 1.0 m agno3, a yellow precipitate forms and [ag ] becomes negligibly small. which of the following is a correct listing of the ions remaining in solution in order of increasing concentration?
a. po43- < no3- < na+
b. po43- < na+ < no3-
c. no3- < po43- < na+
d. na+ < no3- < po43-
e. na+ < po43- < no3-

In which [Ag+] in negligibly small and the concentration of each reactant is 1.0 M

The answer is A)  PO43- < NO3- < Na+

Explanation:

Ag+ is removed from the solution just like PO43-, so there are just 2 possible answers at this point: a or b. Then we can notice that Na3PO4 releases 3 moles of Na+ and just 1 mole of NO3-

We have 100mL of each reactant with the same concentration for both (1.0 M) so:

(0.1)(1)(3)= 0.3 mol Na+

(0.1)(1)= 0.1 mol NO3-

so PO43- < NO3- < Na+

a is the answer to this question

explanation: