Question

The aqueous solution containing one mole of $CoC{l}_3.5N{H}_3$ consumed 2 mol of silver nitrate solution for precipitation of free chloride ions. The formula of the compound should be

• A. $\left[Co{\left(N{H}_3\right)}_{5}Cl\right]C{l}_2$
• B. $\left[Co{\left(N{H}_3\right)}_{6}C{l}_2\right]Cl$
• C. $\left[Co{\left(N{H}_3\right)}_{4}C{l}_3\right]N{H}_3$
• D. $\left[Co{\left(N{H}_3\right)}_{5}C{l}_3\right]$

Answer 1

Answer: (A)

Consumption of 2 mol of $AgN{O}_3$ indicates presence of 2 ionisable chloride ions per molecule. Hence the formula is $\left[Co{\left(N{H}_3\right)}_{5}Cl\right]C{l}_2$