Embibe Experts Solutions for Chapter: Some Basic Concepts of Chemistry, Exercise 1: Exercise-1

A sample of gaseous hydrocarbon occupying $1.12$ litre at $\mathrm{NTP}$, completely burnt in air and produced $2.2 \mathrm{g}$ of ${\mathrm{CO}}_2$ and $1.8 \mathrm{g} {\mathrm{H}}_2\mathrm{O}$. Calculate the mass of compound taken and volume of ${\mathrm{O}}_2$ at $\mathrm{NTP}$ required for its burning. Also calculate molecular formula of hydrocarbon.

The reaction $\mathrm{A} \left(\mathrm{g}\right)+\mathrm{B} \left(\mathrm{g}\right)\rightleftharpoons \mathrm{C} \left(\mathrm{g}\right)+\mathrm{D} \left(\mathrm{g}\right)$ is studied in a one litre vessel at $250 °\mathrm{C}$. The initial concentration of $\mathrm{A}$ was $3\mathrm{n}$ and that of $\mathrm{B}$ was $\mathrm{n}$. When equilibrium was attained, equilibrium concentration of $\mathrm{C}$ was found to the equal to the equilibrium concentration of $\mathrm{B}$. What is the concentration of $\mathrm{D}$ at equilibrium?

$20 \mathrm{ml}$ of ${\mathrm{H}}_2{\mathrm{O}}_2$, after acidification with dilute ${\mathrm{H}}_2{\mathrm{SO}}_4$, required $30 \mathrm{ml}$ of $\frac{\mathrm{N}}{12} {\mathrm{KMnO}}_4$ for complete oxidation. Determine the strength of ${\mathrm{H}}_2{\mathrm{O}}_2$ solution.

$\mathrm{x} \mathrm{g}$ of the metal gave $\mathrm{y}$ $\mathrm{g}$ of its oxide. Hence equivalent weight of the metal

Equivalent wt. of ${\mathrm{H}}_3{\mathrm{PO}}_4$ in each of the reaction will be respectively -

${\mathrm{H}}_3{\mathrm{PO}}_4+{\mathrm{OH}}^{-}\to {\mathrm{H}}_2{\mathrm{PO}}_{4^{-}}^{}+{\mathrm{H}}_2\mathrm{O}$
${\mathrm{H}}_3{\mathrm{PO}}_4+2{\mathrm{OH}}^{-}\to {\mathrm{HPO}}_4^{2-}+2{\mathrm{H}}_2\mathrm{O}$
${\mathrm{H}}_3{\mathrm{PO}}_4+3{\mathrm{OH}}^{-}\to {\mathrm{PO}}_4^{3-}+3{\mathrm{H}}_2\mathrm{O}$

One litre of a solution contains $18.9 \mathrm{g}$ of ${\mathrm{HNO}}_3$ and one litre of another solution contains $3.2 \mathrm{g}$ of $\mathrm{NaOH}.$ In what volume ratio must these solution be mixed to obtain a neutral solution?

A fresh ${\mathrm{H}}_2{\mathrm{O}}_2$ solution is labeled as $11.2 \mathrm{V}.$  Calculate its concentration in $\mathrm{wt}/\mathrm{vol}$ percent.

What will the concentration of $\left[{\mathrm{Ca}}^{+2}\right]$ in a sample of $1$ litre hard water if after treatment with washing soda $10 \mathrm{g}$ insoluble ${\mathrm{CaCO}}_3$ is precipitated.