Seema Saini Solutions for Chapter: Qualitative Inorganic Salt Analysis, Exercise 3: DPP

Three separate samples of a solution of a single salt gave these results. One formed a white precipitate with an excess of ammonia solution, while the other formed a white precipitate with dilute $\mathrm{NaCl}$ solution. The third formed a black precipitate with ${\mathrm{H}}_2\mathrm{S}.$ The salt could be

${\mathrm{SO}}_3^{2-}$ and ${\mathrm{S}}^{2-}$ can be separated by

A mixture of two salts is not soluble in water, but soluble in dilute $\mathrm{HCl}$ solution. What can the mixture be?

Salt $\mathrm{A}$ is water-soluble and gives a pink colour with phenolphthalein. Salt $\mathrm{B}$ will not give a pink colour with phenolphthalein. However, both salts give a colourless and odourless gas $\left(\mathrm{X}\right)$ on heating. Gas $\left(\mathrm{X}\right)$ gives white turbidity with baryta water which disappears on passing excess of gas $\left(\mathrm{X}\right)$. What are salts $\mathrm{A}$ and $\mathrm{B}$?

${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3+{\mathrm{NH}}_4\mathrm{OH}⟶\mathrm{X}$. Select the correct statement(s) about compound $\mathrm{X}$.

What will be the hybridization in compound $\left(\mathrm{A}\right)$ (this question is from the book does not give details and is incorrect. Hence, it has been reframed along with options). An unknown compound (A) when treated with concentrated sulphuric acid, gives light brown fumes which intensify on the addition of copper turnings. When an aqueous solution of the compound is treated with freshly prepared ${\mathrm{FeSO}}_4$, followed by concentrated ${\mathrm{H}}_2{\mathrm{SO}}_4$, it yields a brown complex at the junction of the two liquids. When the compound is heated with sodium hydroxide solution, it evolves a colourless pungent gas. In another test tube, the solution of the compound is mixed with Nessler's reagent to form a brown precipitate. What is the hybridization of the compound (A)?

${\mathrm{CaCO}}_3\stackrel{\mathrm{\Delta }}{⟶}\mathrm{A}+\mathrm{B} \left(\mathrm{g}\right)$

$\mathrm{A}+{\mathrm{H}}_2\mathrm{O}⟶\mathrm{C}$

$\mathrm{C}+\mathrm{B}⟶\underset{\left(\mathrm{white} \mathrm{precipitate}\right)}{\mathrm{D}}+{\mathrm{H}}_2\mathrm{O}$

$\mathrm{D}+\mathrm{B} \left(\mathrm{g}\right)\to \underset{\left(\mathrm{water} \mathrm{soluble}\right)}{\mathrm{E}}\underset{{\mathrm{BaCl}}_2}{\stackrel{\mathrm{Boil}}{\to }}\underset{(\mathrm{white} \mathrm{precipitate})}{\mathrm{F}}$

Note: Question details are changed from that of the book.

Select the correct option(s) for the white precipitate shown in the above reactions.

Which of the following reaction(s) is/are not redox reactions?