100 mL of 2.0 x 10^-5 M AgNO3 is mixed with 100 mL of 2.0 x 10^-5 M NaCl. Given K_sp(AgCl) = 1.8 x 10^-10, what happens?

No precipitate, because Q = 1.0 x 10^-10 < K_sp

No precipitate, because Q = 4.0 x 10^-10 < K_sp

Precipitate forms, because Q = 1.0 x 10^-10 > K_sp

Precipitate forms, because Q = 4.0 x 10^-10 > K_sp

NEET levelSingle correct optionDifficulty 1 of 3ia057

$100 mL$ of $2.0 \times 1 0^{- 5} M$ $AgNO X_{3}$ is mixed with $100 mL$ of $2.0 \times 1 0^{- 5} M$ $NaCl$ . Given $K_{s p} (AgCl) = 1.8 \times 1 0^{- 10}$ , what happens?

After mixing equal volumes each concentration is halved to

1.0 \times 1 0^{- 5} M

. The ionic product is

Q = (1.0 \times 1 0^{- 5})^{2} = 1.0 \times 1 0^{- 10}

, which is less than

1.8 \times 1 0^{- 10}

, so no precipitate forms. Forgetting the dilution gives the wrong value

4.0 \times 1 0^{- 10}