Some Basic Concepts of Chemistry
362 Questions
Start JEE Mains Test
2021
Q201
JEE Mains
Numerical
14 Mar 2026
The mole fraction of a solute in a 100 molal aqueous solution is ___________ $\times$ 10$-$2. (Round off to the Nearest Integer).
[Given : Atomic masses : H : 1.0 u, O : 16.0 u ]
[Given : Atomic masses : H : 1.0 u, O : 16.0 u ]
Correct Answer: 64
Explanation:
Let weight of H2O = 1000 g
Moles of solute = 100
(mole)H2O = ${{1000} \over {18}}$
Mole fraction of solute = ${{mole\,of\,solute} \over {Total\,moles}}$
$ = {{100} \over {100 + {{1000} \over {18}}}} = {{1800} \over {2800}}$
${X_{solute}} = 64 \times {10^{ - 2}}$
Moles of solute = 100
(mole)H2O = ${{1000} \over {18}}$
Mole fraction of solute = ${{mole\,of\,solute} \over {Total\,moles}}$
$ = {{100} \over {100 + {{1000} \over {18}}}} = {{1800} \over {2800}}$
${X_{solute}} = 64 \times {10^{ - 2}}$
2021
Q202
JEE Mains
Numerical
14 Mar 2026
When 35 mL of 0.15 M lead nitrate solution is mixed with 20 mL of 0.12 M chromic sulphate solution, _________ $\times$ 10$-$5 moles of lead sulphate precipitate out. (Round off to the Nearest Integer).
Correct Answer: 525
Explanation:
For 3 moles of Pb(NO3)2 , we require 1 mole of Cr2(SO4)3
For 5.25 moles of Pb(NO3)2, we require $\frac{1}{3} \times 5.25 $ mole of Cr2(SO4)3 = 1.75 moles
But we have 2.4 moles. So, Cr2(SO4)3 is excess reagent and Pb(NO3)2 is limiting reagent, (LR)
Moles of PbSO4 formed = moles of Pb(NO3)2 consumed
= 5.25 m mol = 525 $ \times $ 10-5 moles
2021
Q203
JEE Mains
Numerical
14 Mar 2026
Complete combustion of 750 g of an organic compound provides 420 g of CO2 and 210 g of H2O. The percentage composition of carbon and hydrogen in organic compound is 15.3 and ___________ respectively. (Round off to the Nearest Integer).
Correct Answer: 3
Explanation:
18 gm H2O $ \Rightarrow $ 2 gm H2
210 gm $ \Rightarrow $ ${2 \over {18}} \times 210$
= 23.33 gm H2
So, % H2 = ${{23.33} \over {750}} \times 100$ = 3.11% $ \approx $ 3%
210 gm $ \Rightarrow $ ${2 \over {18}} \times 210$
= 23.33 gm H2
So, % H2 = ${{23.33} \over {750}} \times 100$ = 3.11% $ \approx $ 3%
2021
Q204
JEE Mains
Numerical
14 Mar 2026
$2MnO_4^ - + b{C_2}O_4^{2 - } + c{H^ + } \to xM{n^{2 + }} + yC{O_2} + z{H_2}O$
If the above equation is balanced with integer coefficients, the value of c is ___________. (Round off to the Nearest Integer).
If the above equation is balanced with integer coefficients, the value of c is ___________. (Round off to the Nearest Integer).
Correct Answer: 16
Explanation:
$2MnO_4^ - + 5{C_2}O_4^{2 - } + 16{H^ + } \to 2M{n^{2 + }} + 10C{O_2} + 8{H_2}O$
2021
Q205
JEE Mains
Numerical
14 Mar 2026
A 6.50 molal solution of KOH (aq.) has a density of 1.89 g cm$-$3. The molarity of the solution is ____________ mol dm$-$3. (Round off to the Nearest Integer).
[Atomic masses : K : 39.0 u; O : 16.0 u; H : 1.0 u]
[Atomic masses : K : 39.0 u; O : 16.0 u; H : 1.0 u]
Correct Answer: 9
Explanation:
$m = {{1000 \times M} \over {1000 \times d - M \times {M_{solute}}}}$
$6.5 = {{1000 \times M} \over {1890 - M \times 56}}$
$ \Rightarrow $ $12285 - 364M = 1000M$
$ \Rightarrow $ $1364M = 12285$
$ \Rightarrow $ $M = 9$
$6.5 = {{1000 \times M} \over {1890 - M \times 56}}$
$ \Rightarrow $ $12285 - 364M = 1000M$
$ \Rightarrow $ $1364M = 12285$
$ \Rightarrow $ $M = 9$
2021
Q206
JEE Mains
Numerical
14 Mar 2026
The NaNO3 weighed out to make 50 mL of an aqueous solution containing 70.0 mg Na+ per mL is _________ g. (Rounded off to the nearest integer)
[Given : Atomic weight in g mol$-$1 - Na : 23; N : 14; O : 16]
[Given : Atomic weight in g mol$-$1 - Na : 23; N : 14; O : 16]
Correct Answer: 13
Explanation:
Na+ = 70 mg/mL
WNa+ in 50 mL solution
= 70 $\times$ 50 mg
= 3500 mg
= 3.5 gm
Moles of Na+ in 50 mL solution = ${{3.5} \over {23}}$
Moles of NaNO3 = moles of Na+
= ${{3.5} \over {23}}$ mol
Mass of NaNO3 = ${{3.5} \over {23}} \times 85 = 12.934$
$ \simeq $ 13 gm
WNa+ in 50 mL solution
= 70 $\times$ 50 mg
= 3500 mg
= 3.5 gm
Moles of Na+ in 50 mL solution = ${{3.5} \over {23}}$
Moles of NaNO3 = moles of Na+
= ${{3.5} \over {23}}$ mol
Mass of NaNO3 = ${{3.5} \over {23}} \times 85 = 12.934$
$ \simeq $ 13 gm
2021
Q207
JEE Mains
Numerical
14 Mar 2026
The number of significant figures in 50000.020 $\times$ 10$-$3 is _____________.
Correct Answer: 8
Explanation:
10$-$3 has no role in significant digits. Here in 50000.020, Number of significant figure = 8 as all zeroes between non zero digits are counted as significant digits and also the last zero is also significant digit as zeroes at the end or right of the number is significant only if they are present at the right side of the decimal.
2021
Q208
JEE Mains
Numerical
14 Mar 2026
In basic medium $Cr{O_4}^{2 - }$ oxidises ${S_2}{O_3}^{2 - }$ to form $S{O_4}^{2 - }$ and itself changes into $Cr{(OH)_4}^ - $. The volume of 0.154 M $Cr{O_4}^{2 - }$ required to react with 40 mL of 0.25 M ${S_2}{O_3}^{2 - }$ is __________ mL. (Rounded off to the nearest integer)
Correct Answer: 173
Explanation:
$17{H_2}O + 8Cr{O_4} + 3{S_2}{O_3}\buildrel {} \over
\longrightarrow 6S{O_4} + 8Cr{(OH)_4}^ - + 2O{H^ - }$
Applying mole-mole analysis
${{0.154 \times v} \over 8} = {{40 \times 0.25} \over 3}$
v = 173 mL
Applying mole-mole analysis
${{0.154 \times v} \over 8} = {{40 \times 0.25} \over 3}$
v = 173 mL
2021
Q209
JEE Mains
Numerical
14 Mar 2026
The formula of a gaseous hydrocarbon which requires 6 times of its own volume of O2 for complete oxidation and produces 4 times its own volume of CO2 is CxHy. The value of y is _____________.
Correct Answer: 8
Explanation:
Combustion reaction :
${C_x}{H_y}(g) + \left( {x + {y \over 4}} \right){O_2}(g) \to xC{O_2}(g) + {y \over 2}{H_2}O(l)$
Suppose, volume of CxHy is V and volume of O2 is 6 times greater than CxHy = 6V
then volume of xCO2 $\Rightarrow$ Vx = 4 V
x = 4
Since, ${V_{{O_2}}} = 6 \times {V_{{C_x}{H_y}}}$
$V\left( {x + {y \over 4}} \right)$ = 6V
$\left( {x + {y \over 4}} \right) = 6$ ..... (i)
Put value of x = 4 in Eq. (i) we get,
$4 + {y \over 4} = 6 \Rightarrow y = 8$
${C_x}{H_y}(g) + \left( {x + {y \over 4}} \right){O_2}(g) \to xC{O_2}(g) + {y \over 2}{H_2}O(l)$
Suppose, volume of CxHy is V and volume of O2 is 6 times greater than CxHy = 6V
then volume of xCO2 $\Rightarrow$ Vx = 4 V
x = 4
Since, ${V_{{O_2}}} = 6 \times {V_{{C_x}{H_y}}}$
$V\left( {x + {y \over 4}} \right)$ = 6V
$\left( {x + {y \over 4}} \right) = 6$ ..... (i)
Put value of x = 4 in Eq. (i) we get,
$4 + {y \over 4} = 6 \Rightarrow y = 8$
2021
Q210
JEE Mains
Numerical
14 Mar 2026
1.86 g of aniline completely reacts to form acetanilide. 10% of the product is lost during purification. Amount of acetanilide obtained after purification (in g) is __________ $\times$ 10$-$2.
Correct Answer: 243
Explanation:
Given, weight = 18.6 g
Here, 1 mole of aniline gives 1 mole of acetanilide
$\therefore$ mole of aniline = mole of acetanilide
$\Rightarrow$ ${{1.86} \over {93}} = {{{W_\text{Acetanilide}}} \over {135}}$
${W_\text{Acetanilide}} = {{1.86 \times 135} \over {93}}g = 2.70g$
But efficiency of reaction is 90% only.
Hence, mass of acetanilide produced $ = 2.70 \times {{90} \over {100}}g = 2.43g = 243 \times {10^2}g$
x = 243
2021
Q211
JEE Mains
Numerical
14 Mar 2026
4.5 g of compound A (MW = 90) was used to make 250 mL of its aqueous solution. The
molarity of the solution in M is x $ \times $ 10-1.
The value of x is _______. (Rounded off to the nearest integer)
The value of x is _______. (Rounded off to the nearest integer)
Correct Answer: 2
Explanation:
Given, weight of compound A = 4.5 g
Molecular weight of compound A = 90 g/mol
Volume of solution (in mL) = 250 mL
Now, molarity is defined as number of moles of solute or compound A divided by volume of solution (in L).
$M = {{Number\,of\,moles\,of\,solute\,(n)} \over {Volume\,of\,solution}}$
$ = {{{{4.5} \over {90}}} \over {{{250} \over {1000}}}} = 0.2$ = 2 $\times$ 10$-$1 M
$\therefore$ $n = {{Weight\,of\,solute\,(compound\,A)} \over {Molecular\,weight\,of\,solute\,(compound\,A)}}$
Hence, x $\times$ 10$-$1 $\mu$
x = 2
Molecular weight of compound A = 90 g/mol
Volume of solution (in mL) = 250 mL
Now, molarity is defined as number of moles of solute or compound A divided by volume of solution (in L).
$M = {{Number\,of\,moles\,of\,solute\,(n)} \over {Volume\,of\,solution}}$
$ = {{{{4.5} \over {90}}} \over {{{250} \over {1000}}}} = 0.2$ = 2 $\times$ 10$-$1 M
$\therefore$ $n = {{Weight\,of\,solute\,(compound\,A)} \over {Molecular\,weight\,of\,solute\,(compound\,A)}}$
Hence, x $\times$ 10$-$1 $\mu$
x = 2
2021
Q212
AP-EAPCET
MCQ
20 May 2026
If the volume of $15.9 \mathrm{~g}$ of carbon tetrachloride is $10 \mathrm{~mL}$, calculate its density.
A.
$31.8 \mathrm{~g} \mathrm{~mL}^{-1}$
B.
$1.59 \mathrm{~g} \mathrm{~mL}^{-1}$
C.
$0.159 \mathrm{~g} \mathrm{~mL}^{-1}$
D.
$15.9 \mathrm{~g} \mathrm{~mL}^{-1}$
2021
Q213
AP-EAPCET
MCQ
20 May 2026
$0.63 \mathrm{~g}$ of oxalic acid is dissolved in order to obtain $250 \mathrm{~cm}^3$ of its solution. Find the normality of this solution. [oxalic acid $\left.(\mathrm{COOH})_2 \cdot 2 \mathrm{H}_2 \mathrm{O}\right]$
A.
0.05 N
B.
0.01 N
C.
0.04 N
D.
0.02 N
2021
Q214
AP-EAPCET
MCQ
20 May 2026
$7.8 \mathrm{~g}$ of a compound having molecular formula $\mathrm{C}_6 \mathrm{H}_6$, on reacting with $\mathrm{CH}_3 \mathrm{COCl} / \mathrm{AlCl}_3$ gives $8.4 \mathrm{~g}$ of a product which has molecular formula $\mathrm{C}_8 \mathrm{H}_8 \mathrm{O}$. Calculate the percentage yield of the product $\mathrm{C}_8 \mathrm{H}_8 \mathrm{O}$. (Given, atomic weights of $\mathrm{H}, \mathrm{C}$ and $\mathrm{O}$ respectively are 1, 12 and 16)
A.
70%
B.
60%
C.
80%
D.
75%
2021
Q215
AP-EAPCET
MCQ
20 May 2026
The complete combustion of one mole of benzene produces .......... grams of carbon dioxide.
A.
164
B.
220
C.
264
D.
308
2021
Q216
AP-EAPCET
MCQ
20 May 2026
An alloy of metals X and Y weighs 12 g and contains atoms X and Y in the ratio of 2 : 5. The percentage of metal X in the alloy is 20 by mass. If the atomic mass of X is 40 amu what is the atomic mass of metal Y ?
A.
64 amu
B.
32 amu
C.
60 amu
D.
50 amu
2021
Q217
AP-EAPCET
MCQ
20 May 2026
If 0.2 moles of sulphuric acid is poured into 250 mL of water, calculate the concentration of the solution.
A.
0.8 N
B.
0.8 M
C.
8 M
D.
0.2 N
2021
Q218
AP-EAPCET
MCQ
20 May 2026
When 20 g of CaCO$_3$ is treated with 20 g of HCl, the mass of CO$_2$ formed would be
A.
10 g
B.
8.8 g
C.
22.2 g
D.
20 g
2021
Q219
BITSAT
MCQ
11 Jun 2026
In Victor Meyer's method 0.2 g of an organic substance displaced 56 mL of air at STP the molecular weight of the compound
A.
56
B.
112
C.
80
D.
28
2021
Q220
BITSAT
MCQ
11 Jun 2026
The density (in g mL$-$1] of a 3.60 M sulphuric acid solution that is 29% H2SO4 (molar mass = 98 g mol$-$1) by mass will be
A.
1.64
B.
1.88
C.
1.22
D.
1.45
2020
Q221
JEE Mains
MCQ
14 Mar 2026
The average molar mass of chlorine is
35.5 g mol–1. The ratio of 35Cl to 37Cl in naturally
occuring chlorine is close to :
A.
1 : 1
B.
2 : 1
C.
3 : 1
D.
4 : 1
2020
Q222
JEE Mains
MCQ
14 Mar 2026
A solution of two components containing
n1 moles of the 1st component and n2 moles of
the 2nd component is prepared. M1 and M2 are
the molecular weights of component 1 and 2
respectively. If d is the density of the solution
in g mL–1, C2 is the molarity and x2 is the mole
fraction of the 2nd component, then C2 can be
expressed as :
A.
${C_2} = {{1000{x_2}} \over {{M_1} + {x_2}\left( {{M_2} - {M_1}} \right)}}$
B.
${C_2} = {{1000d{x_2}} \over {{M_1} + {x_2}\left( {{M_2} - {M_1}} \right)}}$
C.
${C_2} = {{d{x_2}} \over {{M_1} + {x_2}\left( {{M_2} - {M_1}} \right)}}$
D.
${C_2} = {{d{x_1}} \over {{M_1} + {x_2}\left( {{M_2} - {M_1}} \right)}}$
2020
Q223
JEE Mains
MCQ
14 Mar 2026
The strengths of 5.6 volume hydrogen peroxide
(of density 1 g/mL) in terms of mass percentage
and molarity (M), respectively, are:
(Take molar mass of hydrogen peroxide as
34 g/mol)
A.
0.85 and 0.5
B.
0.85 and 0.25
C.
1.7 and 0.25
D.
1.7 and 0.5
2020
Q224
JEE Mains
MCQ
14 Mar 2026
The ammonia (NH3) released on quantitative reaction of 0.6 g urea (NH2CONH2) with sodium hydroxide (NaOH) can be neutralized by :
A.
200 ml of 0.02 N HCl
B.
100 ml of 0.2 N HCl
C.
100 ml of 0.1 HCl
D.
200 ml of 0.4 N HCl
2020
Q225
JEE Mains
MCQ
14 Mar 2026
Amongst the following statements, that which was not proposed by Dalton was :
A.
Matter consists of indivisible atoms all the atoms of a given element have.
B.
Chemical reactions involve reorganization of atoms. These are neither created not destroyed in
a chemical reaction.
C.
When gases combine or reproduced in a chemical reactionn they do so in a simple ratio by
volume provided all gases are the same T & P.
D.
Identical properties including identical mass. Atoms of differemt element differ in mass.
2020
Q226
JEE Mains
Numerical
14 Mar 2026
Consider the following equations :
2Fe2+ + H2O2 $ \to $ xA + yB
(in basic medium)
2MnO4- + 6H+ + 5H2O2 $ \to $ x'C + y'D + z'E
(in acidic medium)
The sum of the stoichiometric coefficients x, y, x', y', and z' for products A, B, C, D and E, respectively, is ______.
2Fe2+ + H2O2 $ \to $ xA + yB
(in basic medium)
2MnO4- + 6H+ + 5H2O2 $ \to $ x'C + y'D + z'E
(in acidic medium)
The sum of the stoichiometric coefficients x, y, x', y', and z' for products A, B, C, D and E, respectively, is ______.
Correct Answer: 19
Explanation:
2Fe2+ + H2O2 $ \to $ 2Fe3+ + 2OH–
2MnO4- + 6H+ + 5H2O2 $ \to $ 2Mn2+ + 8H2O + 5O2
$ \therefore $ x + y + x' + y' + z' = 19
2MnO4- + 6H+ + 5H2O2 $ \to $ 2Mn2+ + 8H2O + 5O2
$ \therefore $ x + y + x' + y' + z' = 19
2020
Q227
JEE Mains
Numerical
14 Mar 2026
A 20.0 mL solution containing 0.2 g impure
H2O2 reacts completely with 0.316 g of KMnO4
in acid solution. The purity of H2O2 (in %) is
_____________
(mol. wt. of H2O2 = 34; mol. wt. of KMnO4 = 158)
(mol. wt. of H2O2 = 34; mol. wt. of KMnO4 = 158)
Correct Answer: 85
Explanation:
5H2O2 + 2MnO4- + 6H+ $ \to $ 2Mn2+ + 5O2 + 8H2O
Moles of KMnO4 = ${{0.316} \over {158}}$ = 2 $ \times $ 10-3
Equivalents of H2O2 = Equivalent of KMnO4
= 2 × 10–3 × 5 = 0.01
Moles of H2O2 = ${{0.01} \over 2}$ = 0.005
Mass of pure H2O2 = 0.005 × 34 = 0.170 gm
Percentage purity = ${{0.17} \over {0.2}}$ $ \times $ 100 = 85 %
Moles of KMnO4 = ${{0.316} \over {158}}$ = 2 $ \times $ 10-3
Equivalents of H2O2 = Equivalent of KMnO4
= 2 × 10–3 × 5 = 0.01
Moles of H2O2 = ${{0.01} \over 2}$ = 0.005
Mass of pure H2O2 = 0.005 × 34 = 0.170 gm
Percentage purity = ${{0.17} \over {0.2}}$ $ \times $ 100 = 85 %
2020
Q228
JEE Mains
Numerical
14 Mar 2026
The mass of ammonia in grams produced when
2.8 kg of dinitrogen quantitatively reacts with 1
kg of dihydrogen is _______.
Correct Answer: 3400
Explanation:
N2(g) + 3H2(g) $ \to $ 2NH3(g)
Number of moles of N2 = ${{2.8 \times {{10}^3}} \over {28}}$ = 100
Number of moles of H2 = ${{1000} \over 2}$ = 500
Here N2 is limiting reagent.
$ \therefore $ Number of moles of NH3 produced = 2 $ \times $ 100 = 200
Mass of NH3 produced = 200 × 17 = 3400 gm
Number of moles of N2 = ${{2.8 \times {{10}^3}} \over {28}}$ = 100
Number of moles of H2 = ${{1000} \over 2}$ = 500
Here N2 is limiting reagent.
$ \therefore $ Number of moles of NH3 produced = 2 $ \times $ 100 = 200
Mass of NH3 produced = 200 × 17 = 3400 gm
2020
Q229
JEE Mains
Numerical
14 Mar 2026
6.023 $ \times $ 1022 molecules are present in 10 g of a substance 'x'. The molarity of a solution containing
5 g of substance 'x' in 2 L solution is _____ × 10-3
Correct Answer: 25
Explanation:
Mass of 6.023 × 1022 molecules of a substance
= 10 g
Mass of 6.023 × 1023 molecules of the substance = 100 g
$ \therefore $ Molar mass of the substance = 100 g mol–1
Molarity of the solution =
= ${{\left( {5/100} \right)} \over 2}$ = 0.025
Mass of 6.023 × 1023 molecules of the substance = 100 g
$ \therefore $ Molar mass of the substance = 100 g mol–1
Molarity of the solution =
moles of solute
volume of solution(in l)
= ${{\left( {5/100} \right)} \over 2}$ = 0.025
2020
Q230
JEE Mains
Numerical
14 Mar 2026
The volume (in mL) of 0.1 N NaOH required to neutralise 10 mL of 0.1 N phosphinic acid is ___________.
Correct Answer: 10
Explanation:
H3PO2 + NaOH $ \to $ NaH2PO2 + H2O
Using Stoichiometry
$ \Rightarrow $ ${{0.1 \times 10} \over 1}$ = 0.1 × VNaOH
$ \Rightarrow $ VNaOH = 10 ml
Using Stoichiometry
Moles of H3PO2 reacted
1
=
Moles of NaOH reacted
1
$ \Rightarrow $ ${{0.1 \times 10} \over 1}$ = 0.1 × VNaOH
$ \Rightarrow $ VNaOH = 10 ml
2020
Q231
JEE Mains
Numerical
14 Mar 2026
The mole fraction of glucose (C6H12O6
) in an aqueous binary solution is 0.1. The mass percentage of
water in it, to the nearest integer, is _______.
Correct Answer: 47
Explanation:
Mole fraction of glucose in aqueous solution
= 0.1
Let total mole is 1 mol then mole of glucose will be 0.1 and mole of water will be 0.9.
So mass % of water = ${{0.9 \times 18} \over {0.1 \times 180 + 0.9 \times 18}}$ $ \times $ 100
= 47.37 $ \simeq $ 47
Let total mole is 1 mol then mole of glucose will be 0.1 and mole of water will be 0.9.
So mass % of water = ${{0.9 \times 18} \over {0.1 \times 180 + 0.9 \times 18}}$ $ \times $ 100
= 47.37 $ \simeq $ 47
2020
Q232
JEE Mains
Numerical
14 Mar 2026
The volume strength of 8.9 M H2O2
solution calculated at 273 K and 1 atm is ______. (R = 0.0821 L
atm K-1 mol-1) (rounded off ot the nearest integer)
Correct Answer: 100
Explanation:
Volume strength of H2O2 at 1 atm
273 kelvin
= M × 11.2 = 8.9 × 11.2 = 99.68 $ \simeq $ 100
= M × 11.2 = 8.9 × 11.2 = 99.68 $ \simeq $ 100
2020
Q233
JEE Mains
Numerical
14 Mar 2026
The ratio of the mass percentages of ‘C & H’
and ‘C & O’ of a saturated acyclic organic
compound ‘X’ are 4 : 1 and 3 : 4 respectively.
Then, the moles of oxygen gas required for
complete combustion of two moles of organic
compound ‘X’ is ________.
Correct Answer: 5
Explanation:
Let the organic compound X is = CxHyOz
Here moles of C = x, moles of H = y, moles of O = z
Given, ${{{W_C}} \over {{W_H}}} = {4 \over 1}$
$ \therefore $ ${x \over y} = {{{{{W_C}} \over {12}}} \over {{{{W_H}} \over 1}}}$ = ${4 \over 1} \times {1 \over {12}}$ = ${1 \over 3}$
Also Given, ${{{W_C}} \over {{W_O}}} = {3 \over 4}$
$ \therefore $ ${x \over z} = {{{{{W_C}} \over {12}}} \over {{{{W_O}} \over {16}}}}$ = ${3 \over 4} \times {{16} \over {12}}$ = 1
$ \Rightarrow $ x = z
$ \therefore $ Empirical formula = CxH3xOx = CH3O
As compound is saturated acyclic organic
compound, so molecular formula = C2H6O2
C2H6O2 + ${5 \over 2}$O2 $ \to $ 2CO2 + 3H2O
For 1 mole of C2H6O2 number of moles of O2 required = ${5 \over 2}$
$ \therefore $ For 2 mole of C2H6O2 number of moles
of O2 required = ${5 \over 2}$ $ \times $ 2 = 5
Here moles of C = x, moles of H = y, moles of O = z
Given, ${{{W_C}} \over {{W_H}}} = {4 \over 1}$
$ \therefore $ ${x \over y} = {{{{{W_C}} \over {12}}} \over {{{{W_H}} \over 1}}}$ = ${4 \over 1} \times {1 \over {12}}$ = ${1 \over 3}$
Also Given, ${{{W_C}} \over {{W_O}}} = {3 \over 4}$
$ \therefore $ ${x \over z} = {{{{{W_C}} \over {12}}} \over {{{{W_O}} \over {16}}}}$ = ${3 \over 4} \times {{16} \over {12}}$ = 1
$ \Rightarrow $ x = z
$ \therefore $ Empirical formula = CxH3xOx = CH3O
As compound is saturated acyclic organic
compound, so molecular formula = C2H6O2
C2H6O2 + ${5 \over 2}$O2 $ \to $ 2CO2 + 3H2O
For 1 mole of C2H6O2 number of moles of O2 required = ${5 \over 2}$
$ \therefore $ For 2 mole of C2H6O2 number of moles
of O2 required = ${5 \over 2}$ $ \times $ 2 = 5
2020
Q234
JEE Mains
Numerical
14 Mar 2026
10.30 mg of O2 is dissolved into a liter of sea
water of density 1.03 g/mL. The concentration
of O2 in ppm is__________.
Correct Answer: 10
Explanation:
1030 gm of sea water contains = 10.3 × 10–3 gm
106 gm of sea water contains = ${{10.3 \times {{10}^{ - 3}}} \over {1030}} \times {10^6}$ = 10 ppm
106 gm of sea water contains = ${{10.3 \times {{10}^{ - 3}}} \over {1030}} \times {10^6}$ = 10 ppm
2020
Q235
JEE Mains
Numerical
14 Mar 2026
The molarity of HNO3 in a sample which has
density 1.4 g/mL and mass percentage of 63%
is _____.
(Molecular Weight of HNO3 = 63)
(Molecular Weight of HNO3 = 63)
Correct Answer: 14
Explanation:
%w/w = 63%
dsolution = 1.4 g/ml
Molarity =
= ${{63 \times 1.4 \times 10} \over {63}}$ = 14 M
dsolution = 1.4 g/ml
Molarity =
%w/w $ \times $ dsolution
Moleculer weight of Solute
.$ \times $ 10
= ${{63 \times 1.4 \times 10} \over {63}}$ = 14 M
2020
Q236
JEE Mains
Numerical
14 Mar 2026
The hardness of a water sample containing
10–3 M MgSO4 expressed as CaCO3 equivalents
(in ppm) is ______.
(molar mass of MgSO4 is 120.37 g/mol)
(molar mass of MgSO4 is 120.37 g/mol)
Correct Answer: 100
Explanation:
Equivalance of MgSO4 = Equivalance of CaCO3
$ \Rightarrow $ 10-3 $ \times $ 2 = [CaCO3] $ \times $ 2
$ \Rightarrow $ [CaCO3] = 10-3 M = 10-3 mol/lit
= 10-3 $ \times $ 100 g/lit
= 100 mg/lit
= 100 ppm
$ \Rightarrow $ 10-3 $ \times $ 2 = [CaCO3] $ \times $ 2
$ \Rightarrow $ [CaCO3] = 10-3 M = 10-3 mol/lit
= 10-3 $ \times $ 100 g/lit
= 100 mg/lit
= 100 ppm
2020
Q237
JEE Mains
Numerical
14 Mar 2026
The volume (in mL) of 0.125 M AgNO3 required to quantitatively precipitate chloride ions in 0.3 g of
[Co(NH3)6]Cl3 is ________.
M[Co(NH3)6Cl3] = 267.46 g/mol
MAgNO3 = 169.87 g/mol
M[Co(NH3)6Cl3] = 267.46 g/mol
MAgNO3 = 169.87 g/mol
Correct Answer: 26.80to27.00
Explanation:
[Co(NH3)6]Cl3 + 3AgNO3 $ \to $ 3AgCl
$ \Rightarrow $ ${{0.3} \over {267.46}} = {{0.125 \times v \times {{10}^{ - 3}}} \over 3}$
$ \Rightarrow $ v = 26.92 ml
Mole of [Co(NH3)6]Cl3
1
=
Mole of AgNO3
3
$ \Rightarrow $ ${{0.3} \over {267.46}} = {{0.125 \times v \times {{10}^{ - 3}}} \over 3}$
$ \Rightarrow $ v = 26.92 ml
2020
Q238
JEE Mains
Numerical
14 Mar 2026
Ferrous sulphate heptahydrate is used to fortify foods with iron. The amount (in grams) of the salt required to
achieve 10 ppm of iron in 100 kg of wheat is _______.
Atomic weight : Fe = 55.85; S = 32.00; O = 16.00
Atomic weight : Fe = 55.85; S = 32.00; O = 16.00
Correct Answer: 4.95to4.97
Explanation:
FeSO4.7H2O (M = 277.85)
PPM =
$ \Rightarrow $ 10 =
$ \Rightarrow $ Mass of Iron = 1 gm
Molecular mass of FeSO4.7H2O is 277.85
55.85 gm iron is present in 277.85 gm of salt
1 gm iron is present in = ${{277.85} \over {55.85}}$ = 4.97 gm of salt.
PPM =
Mass of Iron
Mass of wheat
$ \times $ 106
$ \Rightarrow $ 10 =
Mass of Iron
100 $ \times $ 103
$ \times $ 106
$ \Rightarrow $ Mass of Iron = 1 gm
Molecular mass of FeSO4.7H2O is 277.85
55.85 gm iron is present in 277.85 gm of salt
1 gm iron is present in = ${{277.85} \over {55.85}}$ = 4.97 gm of salt.
2020
Q239
JEE Mains
Numerical
14 Mar 2026
The flocculation value of HCl for arsenic sulphide sol.
is 30 m mol L-1 If H2SO4 is used for the flocculatiopn of arsenic sulphide, the amount in grams, of H2SO4 in 250 ml required for the above purposed is ______.
(molecular mass of H2SO4 = 98 g/mol)
is 30 m mol L-1 If H2SO4 is used for the flocculatiopn of arsenic sulphide, the amount in grams, of H2SO4 in 250 ml required for the above purposed is ______.
(molecular mass of H2SO4 = 98 g/mol)
Correct Answer: 0.36to0.38
Explanation:
Arsenic sulphide sol is negatively charged, so for flocculation
positive ion required. Here positive ion H+ present.
for 1 L, 30 mm moles of H+ is required
for 250 ml, ${{30} \over 4}$ mm moles H+ is required
$ \therefore $ for 250 ml, ${{30} \over {4 \times 2}}$ mm moles H2SO4 is required.
$ \therefore $ Weight of H2SO4 required = ${{30} \over {4 \times 2}} \times {10^{ - 3}} \times 98$
= 0.3675 g
for 1 L, 30 mm moles of H+ is required
for 250 ml, ${{30} \over 4}$ mm moles H+ is required
$ \therefore $ for 250 ml, ${{30} \over {4 \times 2}}$ mm moles H2SO4 is required.
$ \therefore $ Weight of H2SO4 required = ${{30} \over {4 \times 2}} \times {10^{ - 3}} \times 98$
= 0.3675 g
2020
Q240
JEE Advanced
Numerical
14 Mar 2026
In the chemical reaction between stoichiometric quantities of KMnO4 and KI in weakly basic solution, what is the number of moles of I2 released for 4 moles of KMnO4 consumed?
Correct Answer: 6
Explanation:
In alkaline medium : Iodide is oxidised to iodate
$2MnO_4^ - + {H_2}O + {I^ - }\buildrel {} \over \longrightarrow 2Mn{O_2} + 2O{H^ - } + IO_3^ - $
But in weakly basic solution :
$\mathop {KMn{O_4}}\limits^{ + 7} + \mathop {KI}\limits^{ - 1} \buildrel {} \over \longrightarrow \mathop {Mn{O_2}}\limits^{ + 4} + \mathop {{I_2}}\limits^0 $
Eq. of KMnO4 = Eq. of I2
$4 \times 3 = n \times 2 \Rightarrow n = 6$
$2MnO_4^ - + {H_2}O + {I^ - }\buildrel {} \over \longrightarrow 2Mn{O_2} + 2O{H^ - } + IO_3^ - $
But in weakly basic solution :
$\mathop {KMn{O_4}}\limits^{ + 7} + \mathop {KI}\limits^{ - 1} \buildrel {} \over \longrightarrow \mathop {Mn{O_2}}\limits^{ + 4} + \mathop {{I_2}}\limits^0 $
Eq. of KMnO4 = Eq. of I2
$4 \times 3 = n \times 2 \Rightarrow n = 6$
2020
Q241
JEE Advanced
Numerical
14 Mar 2026
5.00 mL of 0.10 M oxalic acid solution taken in a conical flask is titrated against NaOH from a burette using phenolphthalein indicator. The volume of NaOH required for the appearance of permanent faint pink color is tabulated below for five experiments. What is the concentration, in molarity, of the NaOH solution?
| Exp. No. | Vol. of NaOH (mL) |
|---|---|
| 1 | 12.5 |
| 2 | 10.5 |
| 3 | 9.0 |
| 4 | 9.0 |
| 5 | 9.0 |
Correct Answer: 0.11
Explanation:
Oxalic acid solution titrated with NaOH solution using phenolphthalein as an indicator.
${H_2}{C_2}{O_4} + 2NaOH\buildrel {} \over \longrightarrow N{a_2}{C_2}{O_4} + 2{H_2}O$
Equivalent of H2C2O4 reacted = Equivalent of NaOH reacted
$ = {{5 \times 2 \times 0.1} \over {1000}} = {{9 \times {M_{(NaOH)}} \times 1} \over {1000}}$
${M_{(NaOH)}} = {1 \over 9} = 0.11$
${H_2}{C_2}{O_4} + 2NaOH\buildrel {} \over \longrightarrow N{a_2}{C_2}{O_4} + 2{H_2}O$
Equivalent of H2C2O4 reacted = Equivalent of NaOH reacted
$ = {{5 \times 2 \times 0.1} \over {1000}} = {{9 \times {M_{(NaOH)}} \times 1} \over {1000}}$
${M_{(NaOH)}} = {1 \over 9} = 0.11$
2019
Q242
JEE Mains
MCQ
14 Mar 2026
25 g of an unknown hydrocarbon upon burning produces 88 g of CO2 and 9 g of H2O. This unknown
hydrocarbon contains :
A.
18 g of carbon and 7 g of hydrogen
B.
20 g of carbon and 5 g of hydrogen
C.
22 g of carbon and 3 g of hydrogen
D.
24 g of carbon and 1 g of hydrogen
2019
Q243
JEE Mains
MCQ
14 Mar 2026
Thermal decomposition of a Mn compound (X) at 513 K results in compound Y, MnO2 and gaseous product.
MnO2 reacts with NaCl and concentrated H2O4 to give a pungent gas Z. X, Y and Z, respectively, are :
A.
KMnO4, K2MnO4 and Cl2
B.
K2MnO4, KMnO4 and SO2
C.
K3MnO4, K2MnO4 and Cl2
D.
K2MnO4, KMnO4 and Cl2
2019
Q244
JEE Mains
MCQ
14 Mar 2026
The mole fraction of a solvent in aqueous solution of a solute is 0.8. The molality (in mol kg–1
) of the
aqueous solution is :
A.
13.88 × 10–1
B.
13.88 × 10–3
C.
13.88
D.
13.88 × 10–2
2019
Q245
JEE Mains
MCQ
14 Mar 2026
5 moles of AB2 weigh 125 × 10–3
kg and 10 moles of A2B2 weigh 300 × 10–3
kg. The molar mass of A (MA)
and molar mass of B (MB) in kg mol are:
A.
MA = 10 × 10–3
and MB = 5 × 10–3
B.
MA = 25 × 10–3
and MB = 50 × 10–3
C.
MA = 5 × 10–3
and MB = 10 × 10–3
D.
MA = 50 × 10–3
and MB = 25 × 10–3
2019
Q246
JEE Mains
MCQ
14 Mar 2026
The minimum amount of O2(g) consumed per gram of reactant is for the reaction :
(Given atomic mass : Fe = 56, O = 16, Mg = 24, P = 31, C = 12, H = 1)
(Given atomic mass : Fe = 56, O = 16, Mg = 24, P = 31, C = 12, H = 1)
A.
4Fe(s) + 3O2(g) $ \to $ 2Fe2O3(s)
B.
P4(s) + 5O2(g) $ \to $ P4O10(s)
C.
C3H8(g) + 5O2(g) $ \to $ 3CO2(g) + 4H2O(l)
D.
2Mg(s) + O2(g) $ \to $ 2MgO(s)
2019
Q247
JEE Mains
MCQ
14 Mar 2026
At 300 K and 1 atmospheric pressure, 10 mL of a hydrocarbon required 55 mL of O2 for complete
combustion, and 40 mL of CO2 is formed. The formula of the hydrocarbon is :
A.
C4H7Cl
B.
C4H6
C.
C4H8
D.
C4H10
2019
Q248
JEE Mains
MCQ
14 Mar 2026
What would be the molality of 20% (mass/
mass) aqueous solution of KI?
(molar mass of KI = 166 g mol–1)
(molar mass of KI = 166 g mol–1)
A.
1.51
B.
1.35
C.
1.08
D.
1.48
2019
Q249
JEE Mains
MCQ
14 Mar 2026
For a reaction,
N2(g) + 3H2(g) $ \to $ 2NH3(g) ;
identify dihydrogen (H2) as a limiting reagent in the following reaction mixtures.
N2(g) + 3H2(g) $ \to $ 2NH3(g) ;
identify dihydrogen (H2) as a limiting reagent in the following reaction mixtures.
A.
56g of N2 + 10g of H2
B.
14g of N2 + 4g of H2
C.
28g of N2 + 6g of H2
D.
35g of N2 + 8g of H2
2019
Q250
JEE Mains
MCQ
14 Mar 2026
The percentage composition of carbon by mole
in methane is :
A.
80%
B.
20%
C.
75%
D.
25%