Donna asks…solid AgCl is placed in 1L of 0.55 M NaCl, what mass of AgCl will dissolve? using Ksp=1.8x10-10?Nancy answers:Ksp =
Let x = molar solubility, so
1.8x10^-10 = (x) (x)
But initially = 0.55 M, so
1.8x10^-10 = (x) (0.55+x)
Since 0.55>>x, we can write
1.8x10^-10= (x) (0.55)
Solving, x = = 3.3x10^-10 M
MW of AgCl is 143.4 g/mole, so
(1 L) (3.3x10^-10 mole/L) (143.4 g/mole) = 4.7x10^-8 g of AgCl dissolves.David asks…For the reaction between aqueous silver nitrate and
