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

$1 \mathrm{g} \mathrm{Ca}$ was burnt in excess of ${\mathrm{O}}_2$ and the oxide was dissolved in water to make up one litre of solution. The normality of solution is

An element $\mathrm{A}$ reacts with compound ${\mathrm{BO}}_3$ to produce ${\mathrm{A}}_3{\mathrm{O}}_4$ and ${\mathrm{B}}_2{\mathrm{O}}_3.$ The no. of moles of ${\mathrm{A}}_3{\mathrm{O}}_4$ produced if one mole each of $\mathrm{A}$ and ${\mathrm{BO}}_3$ is reacted?

$1$ litre of gaseous aliphatic compound ${\mathrm{C}}_{\mathrm{x}}{\mathrm{H}}_{\mathrm{y}}{\mathrm{O}}_{\mathrm{z}}$ is completely burnt in excess of ${\mathrm{O}}_2$ and cooled to room temperature. The contraction in volume is

One gram of the silver salt of an organic dibasic acid yields, on strong heating, $0.5934 \mathrm{g}$ of silver. If the weight percentage of carbon in it $8$ times the weight percentage of hydrogen and one-half the weight percentage of oxygen, determine the molecular formula of the acid. [Atomic weight of $\mathrm{Ag}=108$$]$

At $20°\mathrm{C},$ the osmotic pressure of a solution of $100 \mathrm{ml}$ of which contains $6.33 \mathrm{g}$ of the colouring substance of the blood haematin is $243.4{\mathrm{kP}}_{\mathrm{a}}.$ What is the molecular formula of the haematin; if the elementary composition of haematin is $\mathrm{C}=64.4\%, \mathrm{H}=5.2\%, \mathrm{N}=3.8\%, \mathrm{O}=12.6\%$ and $\mathrm{Fe} 8.8\%?$

A bottle of oleum is labelled as $109\%.$ Which of the following statement is/are correct for this oleum sample?

Identify the correct chemical equations with respect to substance, reagent and product

A salt mixture $\left(1.0\mathrm{g}\right)$ contains $25\mathrm{wt}\%$ of ${\mathrm{MgSO}}_4$ and $75\mathrm{wt}\%$ of ${\mathrm{M}}_2{\mathrm{SO}}_4$. Aqueous solution of this salt mixture on treating with excess ${\mathrm{BaCl}}_2$ solution results in the precipitation of $1.49 \mathrm{g}$ of ${\mathrm{BaSO}}_4$. The atomic mass of $\mathrm{M}$ in ${\mathrm{gmol}}^{-1}$ (rounded off to two decimal places) is _____.
(Given: the atomic masses of $\mathrm{Mg},\mathrm{S},\mathrm{O},\mathrm{Ba}$ and $\mathrm{Cl}$ are $24.31,32.06,16.00,137.33$ and $35.45 {\mathrm{gmol}}^{-1}$, respectively)