□ Resources Hint 597/1400 Check Ans nt Score 10 of14 > Determine the molar solubility (S) of Ag CO, in a buffered solution with a pH of 3.036 using the systematic treatment of equilibrium. Ksp...
Determine the molar solubility ( ? S ) of Ag 2 CO 3 Ag2CO3 in a buffered solution with a pH of 5.740 5.740 using the systematic treatment of equilibrium. ? sp ( Ag 2 CO 3 )=8.46× 10 −12 Ksp(Ag2CO3)=8.46×10−12 ; ? a1 ( H 2 CO 3 )=4.45× 10 −7 Ka1(H2CO3)=4.45×10−7 ; ? a2 ( H 2 CO 3 )=4.69× 10 −11 Ka2(H2CO3)=4.69×10−11 .
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.462 using the systematic treatment of equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7; Ka2(H2CO3) = 4.69 × 10–11.
Determine the molar solubility ( ? ) of Ag2CO3 in a buffered solution with a pH of 3.930 using the systematic treatment of equilibrium. ?sp(Ag2CO3)=8.46×10−12 ; ?a1(H2CO3)=4.45×10−7 ; ?a2(H2CO3)=4.69×10−11 .
Determine the molar solubility ( ? ) of Ag2CO3 in a buffered solution with a pH of 5.941 using the systematic treatment of equilibrium. ?sp(Ag2CO3)=8.46×10−12 ; ?a1(H2CO3)=4.45×10−7 ; ?a2(H2CO3)=4.69×10−11 .
determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.519 using the systematic treatment of equilibrium. Ksp (Ag2CO3) = 8.46x10^-12 ; Ka1 (H2CO3) = 4.45x10^-7 ; Ka2 (H2CO3) = 4.69 x 10^-11