A chemist mixes 50.0 mL of 1.0 × 10^{−3} M AgNO_3 with 25.0 mL of 4.0 × 10^{−3} M NaCl at 25 °C. The solubility product constant for AgCl at this temperature is K_{sp} = 1.8 × 10^{−10}. Which statement correctly describes the resulting mixture?
(a) A precipitate of AgCl will form because Q is less than Ksp.
(b) No precipitate will form because dilution keeps both ion concentrations below the solubility product.
(c) A precipitate of AgCl will form because Q exceeds Ksp.
(d) No precipitate will form because the limiting Ag+ is completely used up, making Q effectively zero.