Calculate the mass of the precipitate that will form and the concentration of Ag

Question

Calculate the mass of the precipitate that will form and the concentration of Ag+ remaining in
solution after 0.250 L of 0.200 M AgNO3 solution is mixed with 0.250 L of 0.350 M Na2CO3
solution (KSP for Ag2CO3 is 8.46 x 10^

Explanation / Answer

Ag2CO3 ------------> 2Ag+ + CO3 2- [Ag+] = 0.05 / (0.25 + 0.25) = 0.1 M [CO3 2-] = 0.175 M Ag2CO3 ------------> 2Ag+ + CO3 2- ---X----------------0.1-2X; 0.175-X --0.05-X--------------2X---;0.125+X 8.46 x 10^–12 = (0.1-2X)^2 * (0.175-X) => 8.46 x 10^–12 = (2X)^2 * (0.125+X) neglect X wrt 0.125 => 8.46 x 10^–12 = 0.5 * X^2 => X = 4.113 * 10^-6 Concentration of Ag+ remaining in = 2X = 8.23 * 10^-6 M Mass of Ag2CO3 = 0.05 * 0.5 * 275.75 = 6.9 g

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