11.7 g of NaCl is mixed in solution with 10.2 g of AgNO3: NaCl + AgNO3 -> AgCl + NaNO3 (Na = 23, Cl = 35.5, Ag = 108, N = 14, O = 16). Find the mass of AgCl precipitated in grams, to two decimal places.

JEE Main levelNumerical answerDifficulty 2 of 3mc046

$11.7 g$ of $NaCl$ is mixed in solution with $10.2 g$ of $AgNO X_{3}$ : $NaCl + AgNO X_{3} AgCl + NaNO X_{3}$ (Na = 23, Cl = 35.5, Ag = 108, N = 14, O = 16). Find the mass of $AgCl$ precipitated in grams, to two decimal places.

Numerical answer type, answer in g, tolerance 0.005.

n (NaCl) = 11.7/58.5 = 0.200

;

n (AgNO X_{3}) = 10.2/170 = 0.0600

AgNO X_{3}

is limiting, giving

0.0600

mol

AgCl

(

M = 143.5

). Mass

= 0.0600 \times 143.5 = 8.61 g