Question

Homework #8 Due Monday, November 18 1. Decide whether a precipitate will form when the following solutions are mixed (use Table 18.2): (a) 27.0 mL of 0.0010 M NaCl and 73.0 mL of 0.0040 M AGNO, Ksp = lor NaCl(s) + A. NO Na NO₃ + Ag ClRsp = [A7 AgCl → Ag" - CITO _274L) = M = (100) Qsp = [Agt]. [ci]. 2.710-4 (100292) (2.7.10-4) Qso = 17.88×10 -7 > Ksp _13mL) = M. (100mL) Reaction will shift left, pr -.00292 will form. (b) 1.0 mL of 1.0 M KF, 10.0 mL of 0.0030 M CaCl2, and 100 mL of water
part B please

Answer 1

Solubility equillibrium of CaF2 is

CaF2(s) <-------> Ca²⁺(aq) + 2F^-(aq)

K_sp = [ Ca²⁺] [ F^-]²= 3.9 × 10^-11

Q_sp = [Ca²⁺]_initial × [F^-]²_initial

Total volume = 1.0ml + 10.0ml + 100ml = 111ml

[Ca²⁺]_initial = 0.0030M/(111.0ml / 10ml)) = 0.0002703M

[F^-]_initial = 1.0M/ ( 111.0ml/ 1.0ml) = 0.009009M

Q_sp = 0.0002703M × ( 0.009009M)² = 2.19 × 10^-8

Q_sp > K_sp

Therefore

Precipitate will form