When 2.00 L of 1.00 M of AgNO_3AgNO3 and 1.25 L of 1.00 M of CaI_2CaI2 fully react, what is the molarity of Ca^2+Ca2+?

1 Answer
Jun 24, 2017

For 2AgNO_3(aq) + CaI_2(aq) rarr 2AgI(s)darr + Ca(NO_3)_2(aq)2AgNO3(aq)+CaI2(aq)2AgI(s)+Ca(NO3)2(aq)

Explanation:

The calcium ion, Ca^(2+)Ca2+, which is present in solution as (probably) [Ca(OH_2)_6]^(2+)[Ca(OH2)6]2+, remains in solution, and expresses its concentration fully because it does not precipitate....

"Moles of"Moles of Ca^(2+)=1.25*Lxx1.00*mol*L^-1=1.25*molCa2+=1.25L×1.00molL1=1.25mol.

The volume of solution is (2.00+1.25)*L=3.25*L(2.00+1.25)L=3.25L

And thus concentration of calcium ion is............

(1.25*mol)/((2.00+1.25)*L)=0.385*mol*L^-1......

Of course, the silver ion precipitates as a fine yellow powder of AgI.........