Notice that Barium sulfate is insoluble hence it doesn't dissociate and it precipitate.
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What is the equilibrium Ba2+ concentration when 2.38 L ofa 0.153 M barium acetate solution are...
What is the equilibrium Ba2+ concentration when 1.22 L of a 0.168 M barium chloride solution are mixed with 1.34 L of a 0.283 M potassium sulfate solution? [Ba2+] =
What is the equilibrium Ba2+ concentration when 1.66 L of a 0.138 M barium sulfide solution are mixed with 1.63 L of a 0.253 M potassium carbonate solution? [Ba2+] = M
What is the equilibrium Agt concentration when 1.25 L of a 0.197 M silver acetate solution are mixed with 1.16 L of a 0.203 M ammonium sulfide solution? [Agt] = M
What is the equilibrium Zn2+ concentration when 1.36 L of a 0.166 M zinc sulfate solution are mixed with 1.43 L of a 0.286 M ammonium sulfide solution? [Zn2+] = M
Solid barium acetate is slowly added to 75.0 mL of a 0.0376 M ammonium chromate solution. The concentration of barium ion required to just initiate precipitation is ____ M. Solid barium sulfate and solid barium carbonate are in equilibrium with a solution containing 1.43×10-2 M potassium carbonate. Calculate the concentration of sulfate ion present in this solution. [sulfate] = _____ M.
What is the equilibrium Pb2+ concentration when 2.61 L of a 0.103 M lead acetate solution are mixed with 2.82 L of a 0.370 M ammonium bromidesolution? [Pb2+] = M The solubility of AgCl in water is 1.34×10-5 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgCl when the solid is added to a solution that is 0.520 M in thiosulfate ion. For AgCl, Ksp = 1.80×10-10 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
What is the equilibrium Ag+ concentration when 2.13 L of a 0.111 M silver fluoride solution are mixed with 2.05 L of a 0.112 M ammonium sulfide solution? [Ag+] = M
What is the equilibrium Zn2+ concentration when 1.78 L of a 0.160 M zinc fluoride solution are mixed with 1.94 L of a 0.183 M ammonium phosphate solution? [Zn2+] = _______M
What is the equilibrium Mg^2+ concentration when 3.34 L of a 0.109 M magnesium bromide solution are mixed with 3.51 L of a 0.205 M ammonium solution?
Calculate the concentration in M) of barium ions (Ba2+) in a solution when BaCrO4 is dissolved in a solution that already contains 0.085 M of Cro 2-. The Ksy of BaCrO4 is 2.1 x 10-10 (4 points)