50 mL of 0.10 M $AgNO X_{3}$ is mixed with 50 mL of 0.060 M $BaCl X_{2}$ (volumes additive; $Ag = 108$ , $Cl = 35.5$ ). Treat AgCl as completely insoluble. Which statements are correct?

AThe final $[Cl X^{-}]$ is 0.010 M
BThe final $[Ba X^{2 +}]$ is 0.060 M
CThe mass of AgCl precipitated is 0.7175 g
DThe final $[NO X_{3} X^{-}]$ is 0.050 M

Answer: A, C, D

Ag X^{+}

= 5.0 mmol;

Cl X^{-}

= 2 x 3.0 = 6.0 mmol, so Ag+ is limiting and AgCl = 5.0 mmol = 0.7175 g (true). Cl- left = 1.0 mmol in 100 mL = 0.010 M (true). Ba2+ = 3.0 mmol in 100 mL = 0.030 M, so 0.060 is false (false). Nitrate = 5.0 mmol in 100 mL = 0.050 M (true).

Practice Mole Concept More on Concentration terms (molarity, molality, mole fraction, ppm) and dilution

Previous questionNext question

50 mL of 0.10 M AgNOX3​ is mixed with 50 mL of 0.060 M BaClX2​ (volumes additive; Ag=108, Cl=35.5). Treat AgCl as completely insoluble. Which statements are correct?

Answer: A, C, D

More questions on Concentration terms (molarity, molality, mole fraction, ppm) and dilution

50 mL of 0.10 M $AgNO X_{3}$ is mixed with 50 mL of 0.060 M $BaCl X_{2}$ (volumes additive; $Ag = 108$ , $Cl = 35.5$ ). Treat AgCl as completely insoluble. Which statements are correct?