You prepare a solution by dissolving $0\mathrm{.}050g$ of $)=(111\mathrm{.}1\frac{g}{m}ol$ and $0\mathrm{.}115g$ of $\frac{g}{m}ol)$ with deionized water into a $500mL$ volumetric flask. Assume these salts dissociate completely and no reactions occur $($conservative substances$),$ calculate

a$)$ the ppm concentration of each ionic species

b$)$ the $m\frac{g}{L}$ concentrations of each ion species

c$)$ the mol$/$L concentration of each ionic species

d$)$ the ionic strength of the solution

e$)$ the activity coefficient for each species $($with the Davies equation and the EDHE$).$ Also report the RPD between the two $RPD=\frac{|\text{D}\text{a}\text{v}\text{i}\text{s}|-|EDHE|}{|\text{A}\text{v}\text{e}\text{r}\text{a}\text{g}\text{e}(\text{D}\text{a}\text{v}\text{i}\text{s},\text{E}\text{D}\text{H}\text{E})|}100$

f$)$ the activity of each species based on the EDHE

g$)$ what would be the change in the activity coefficients of each ionic species if the concentration of $CaC{l}_2$ is doubled? Do they increase or decrease? By how much?

$RPD=(EDH{E}_g)-EDH{E}_e$