Some Basic Concepts of Chemistry · Chemistry · TS EAMCET

A solid mixture weighing 5 g contains equal number of moles of $\mathrm{Na}_2 \mathrm{CO}_3$ and NaHCO . This solid mixture was dissolved in 1 L of water. What is the volume (in mL ) of 0.1 M HCl required to completely react with this 1 L mixture solution?

4.0 g of a mixture containing $\mathrm{Na}_2 \mathrm{CO}_3$ and $\mathrm{NaHCO}_3$ is heated to 673 K . Loss in mass of the mixture is found to be 0.62 g . The percentage of sodium carbonate in the mixture is

0.43 g of a metal of valence 2 was dissolved in 50 mL of $0.5 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution. The unreacted acid required 14.2 mL of 1 M NaOH solution for neutralisation. The atomic weight of the metal is

The incorrect rule regarding the determination of significant figures is

12 g of an element reacts with 32 g of oxygen. What is the equivalent weight of the element ?

Which one of the following has the same number of atoms as are in 6 g of $\mathrm{H}_2 \mathrm{O}$ ?

The sum of three values $12.0,19.034$ and 2.0143 is equal to $X$. The number of significant figures in $X$ is

The masses of carbondioxide and water (in g) respectively formed during complete combustion of 10 g of glucose at STP are

Round the number 234555359 to 3 significant figure.

Magnetite can be reduced with CO to yield iron metal and carbon dioxide. Calculate the mass of magnetite (in kg ) needed to obtain 4 kg of iron if the process is $80 \%$ efficient. [Atomic weight of Fe and O are 56 g and 16 g , respectively]

Combustion of 10 mL of a gaseous hydrocarbon gives 40 mL of $\mathrm{CO}_2$ and 50 mL of water vapour under the same conditions. The molecular formula of the hydrocarbon is

The average molecular weight of the air which has $21 \%$ of $\mathrm{O}_2$ and $79 \%$ of $\mathrm{N}_2$, is

The number of significant figures in 2.0400 is

Identify the values of $a, b, c, d$ and $e$ for the following unbalanced reaction,

$$ \begin{aligned} a \mathrm{KNO}_3+5 \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \longrightarrow b \mathrm{~N}_2 & +c \mathrm{CO}_2 +d \mathrm{H}_2 \mathrm{O}+e \mathrm{~K}_2 \mathrm{CO}_3 \end{aligned} $$

Calculate the number of moles of NaOH required to completely neutralise 100 g of $118 \%$ oleum.

The amount of $50 \%(w / w)$ solution of hydrochloric acid required to react with 200 g of $\mathrm{CaCO}_3$ would be

Given the ratio of amounts of nitrogen and oxygen in a particular gaseous mixture is $4: 1$. Calculate the ratio of number of their molecules?

Sulphuric acid reacts with sodium hydroxide as follows:

$$ \mathrm{H}_2 \mathrm{SO}_4+2 \mathrm{NaOH} \longrightarrow \mathrm{Na}_2 \mathrm{SO}_4+2 \mathrm{H}_2 \mathrm{O} $$

What will be the amount of sodium sulphate formed, when l L of 0.2 M sulphuric acid is allowed to react with l L of 0.2 M sodium hydroxide solution?

The molecular mass of sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)$ is

How much volume of 1 N aqueous solution of $\mathrm{H}_2 \mathrm{SO}_4$ should be taken, which will contain 0.2 moles of $\mathrm{H}_2 \mathrm{SO}_4$ ?

For a given unbalanced reaction, $\mathrm{MnO}_2+\mathrm{HCl} \longrightarrow \mathrm{MnCl}_2+\mathrm{H}_2 \mathrm{O}$, which is the limiting reagent, if the initial amount for each of the reactant is 100 grams?

[Molar masses : $\mathrm{MnO}_2=86.9 ; \mathrm{HCl}=36.5 ; \mathrm{MnCl}_2 \left.=125.8 ; \mathrm{Cl}_2=70.9 ; \mathrm{H}_2 \mathrm{O}=18\right]$

The emperical formula of a compound is $\mathrm{C}_2 \mathrm{H}_5 \mathrm{O}$ and its vapour density is 45 . What is the molecular formula of the compound?

Identify the law for which the following statement is true.

"Equal volume of all gases at same temperature and pressure should contain equal number of molecules".

25 mL of 0.1 N NaOH solution neutralises 12.5 mL of HCl solution. The amount of water needed to convert 500 mL of such HCl solution to 0.1 N is