A solution contains 0.0200 mol of [Co(NH3)5Cl]Cl2 and 0.0300 mol of [Co(NH3)4Cl2]Cl. Excess AgNO3 is added and only the free (ionic) chloride is precipitated. Find the amount of AgCl formed in millimoles (nearest integer).

JEE Main levelNumerical answerDifficulty 2 of 3cc123

A solution contains $0.0200$ mol of $[Co (NH X_{3}) X_{5} Cl] Cl X_{2}$ and $0.0300$ mol of $[Co (NH X_{3}) X_{4} Cl X_{2}] Cl$ . Excess $AgNO X_{3}$ is added and only the free (ionic) chloride is precipitated. Find the amount of $AgCl$ formed in millimoles (nearest integer).

Numerical answer type, answer in mmol, tolerance 0.5.

Free chloride per formula unit: 2 for the first complex and 1 for the second. Moles

AgCl

= 0.0200 \times 2 + 0.0300 \times 1 = 0.0700

mol. This equals 70 mmol.