5A(oic)nehrddfbfbffbdgdgdv
Answer :
The Nernst equation :
![E_{cell}=E^o_{cell}-\frac{2.303RT}{nF}\log \frac{[Anode]}{[Cathode]}](https://tex.z-dn.net/?f=E_%7Bcell%7D%3DE%5Eo_%7Bcell%7D-%5Cfrac%7B2.303RT%7D%7BnF%7D%5Clog%20%5Cfrac%7B%5BAnode%5D%7D%7B%5BCathode%5D%7D)
where,
= standard cell potential
n = number of electrons in oxidation-reduction reaction
F = Faraday constant = 96500 C
R= gas constant = 8.314 J/Kmol
T = temperature
[Anode] = anodic ion concentration
[Cathode] = cathodic ion concentration
Balanced chemical reaction:
2Na₃PO₄(aq) + 3CaCl₂(aq) → 6NaCl(aq) + Ca₃(PO₄)₂(s).
Ionic reaction:
6Na⁺(aq) + 2PO₄³⁻(aq) + 3Ca²⁺(aq) + 6Cl⁻(aq) → 6Na⁺(aq) + 6Cl⁻(aq) + Ca₃(PO₄)₂(s).
Net ionic reaction: 2PO₄³⁻(aq) + 3Ca²⁺(aq) → Ca₃(PO₄)₂(s).
<span>(aq) means that
substances are dissociated on cations and anions in water.
</span>(s) means solid.
I'm not sure if what this question is asking but ill be assuming that the average molecular mass is required. An assuming that the abundance of each isotope is 50% the average molecular mass is 69.82 amu.
The concentration of a and b will decrease while c will increase provided all other physical quantities are kept constant in the reaction
