Strontium iodate, Sr(IO3)2(s), is used in some analytical procedures. A chemist adds 0.200 g of Sr(IO3)2 to 500.0 mL of water at 25 °C and allows the mixture to stir until equilibrium is reached. The temperature remains constant and no other sources of ions are present.
(a) For Sr(IO3)2(s) dissolving in water, write the balanced equilibrium equation and the corresponding Ksp expression.
(b) The solubility‐product constant at 25 °C is Ksp=3.2×10−9. Calculate the molar solubility of Sr(IO3)2 in mol L−1.
(c) Using your result from part (b), determine the maximum mass (in g) of Sr(IO3)2 that can dissolve in 500.0 mL of water at 25 °C.
(d) Based on the initial 0.200 g added and your calculation in part (c), state whether any solid Sr(IO3)2 remains undissolved at equilibrium. If so, calculate the mass that remains as solid.