CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 10 - MCQExams.com

A $$5.25%$$ solution of a substance is isotonic with a $$1.5\%$$ solution of urea (molar mass = $$60g mol^{-1})$$ in the same solvent. If the densities of both the solutions are assumed to be equal to $$1.0 g cm^{-3}$$, molar mass of the substance will be:
  • $$105.0 g mol^{-1}$$
  • $$210.0 g mol^{-1}$$
  • $$90.0 g mol^{-1}$$
  • $$15.0 g mol^{-1}$$
Which of the following is the best example of law of conservation of mass?
[n and m are the masses of reactants and p and q are the masses of products formed.]
  • $$n-m=p-q$$
  • $$n+m=p+q$$
  • $$n=m$$
  • $$p=q$$
$$27\ gm\ Al$$ is heated with $$49\ ml$$ of $$H_{2}SO_{4}$$ (specific gravity $$=2$$) produces $$H_{2}$$ gas. Percentage of $$Al$$ reacted with $$H_{2}SO_{4}$$ is:
  • $$50\%$$
  • $$66.66\%$$
  • $$75\%$$
  • $$80\%$$
The amount of water obtained from combustion of $$16 grams$$ of methane is_______
  • 16g
  • 36g
  • 32g
  • 62g
Our body contains ___________ of water by weight.
  • $$70\%$$
  • $$60\%$$
  • $$50\%$$
  • $$80\%$$
$$H_2SO_4$$ is $$98\%$$ by weight of solution .Hence it is ?
  • 1 molal
  • 10 molal
  • 50 molal
  • 500 molal
If mass percentage of $$Mg^{2+}$$ in a biomolecule is 0.2%, then the number of $$Mg^{2+}$$ ions present in 10 g of biomolecule is (Atomic weight of Mg = 24)
  • $$\frac{1}{2} \times 10^{-2}N_{A}$$
  • $$\frac{1}{12} \times 10^{-2}N_{A}$$
  • $$\frac{1}{4}N_{A}$$
  • $$\frac{1}{12}N_{A}$$
What is the proportion by weight the constitution elements of $$Cu$$ and $$O$$ in the compound $$CuO$$?
  • $$3.971: 1$$
  • $$4 : 2.968$$
  • $$4 : 3.971$$
  • $$2.968 : 2$$
Suppose 30% molecules have M = 20000; 40% molecules have M= 30000, rest of them have M=then the PDI is :
  • 1.45
  • 1.20
  • 0.83
  • 0.98
How many grams of concentrated sulphuric acid $$ (80\%W/W) $$ sould be used to prepare 100 mL of one molar $$H_{2}SO_{4}$$ solution?
  • 10 g
  • 12. 25g
  • 15 g
  • 20 g
200 gram of a solution of water and sugar contains 20 g solute. What is the concentration of the solution in mass percentage?
  • 20%
  • 10%
  • 40%
  • 5%
If mass percentage of iron in a biomolecule is 0.4% then the minimum molecular weight of biomolecule will be (Atomic weight of Fe = 56)
  • 18000
  • 16000
  • 10000
  • 14000
$$40$$% of  a mixture of $$0.2mol$$ of $${N}_{2}$$ and $$0.6mol$$ of $${H}_{2}$$ reacts to give $${NH}_{3}$$ according to the equation:
$${N}_{2}(g)+3{H}_{2}(g)\rightleftharpoons  2{NH}_{3}(g)$$
at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases are
  • $$4:5$$
  • $$5:4$$
  • $$7:10$$
  • $$8:5$$

The actual molecular mass of chlorine is :
  • $$58.93 \times {10^{ - 24}}g$$
  • $$117.86 \times {10^{ - 24}}g$$
  • $$58.93 \times {10^{ - 24}}kg$$
  • $$117.86 \times {10^{ - 24}}kg$$
The weight of $$C{H_4}$$ in 9-L cylinder at $${27^0}C$$ temperature  and $$16$$ atm pressure is ($$R=0.08$$ L atm $${K^{ - 1}}\,mo{l^{ - 1}}$$).
  • $$9.6$$ g
  • $$96.0$$ g
  • $$4.8$$ g
  • $$48.0$$ g
A $$0.60g$$ sample consisting of only $$Ca{C}_{2}{O}_{4}$$ and $$Mg{C}_{2}{O}_{4}$$ is heated at $${500}^{o}C$$, converting the two salts of $$Ca{CO}_{3}$$ and $$Mg{CO}_{3}$$. The sample then weighs $$0.465g$$. If the sample had been heated to $${900}^{o}C$$, where the products are $$CaO$$ and $$MgO$$, what would the mixtures of oxides have weighed?
  • $$0.12g$$
  • $$0.21g$$
  • $$0.252g$$
  • $$0.3g$$
Zinc sulphate contains 22.65% Zn and 43.9% $$ \mathrm { H } _ { 2 } \mathrm { O } $$ . if the law of constant proportions is true, then the mass of Zinc required to give 40g crystal will be
  • 90.6 g
  • 9.06 g
  • 0.906 g
  • 906 g
60 g of solution containing 40% by mass of $$NaCl$$ are mixed with 100 g of a solution containing 15% by mass $$NaCl$$. Determine the mass percent of sodium chloride in the final solution.
  • 24.4 %
  • 78 %
  • 48.8 %
  • 19.68 %
The number of $$H_{3}O^{+}$$ ions present in 10ml of water at $$25^{\circ}C$$ is:
  • $$6.023 \times 10^{-14}$$
  • $$6.023 \times 10^{14}$$
  • $$6.023 \times 10^{-19}$$
  • $$6.023 \times 10^{19}$$
Which of the following represents the Avogadro number?
  • Number of molecule present in 1 L of gas at N.T.P
  • Number of molecule present in 22.4 L of gas at N.T.P
  • Number of molecule present in 22.4 of gas at 298K and 1 atm pressure
  • Number of molecule present in one mole of gas at any temp and pressure
What is the value of $$n$$ in the following equation?

$$Cr\left( OH \right) _{ 4 }^{ - }+OH^{ - }\longrightarrow  Cr{ O }_{ 4 }^{ 2- }+H_{ 2 }O\ +\ ne^-$$
  • $$3$$
  • $$6$$
  • $$5$$
  • $$2$$
A sample of potato starch was ground in ball mill to give a starch lime molecule of lower molecular weight. The product analysed $$0.86\%$$ phosphorus.  If each molecule is assumed to contain one atom of phosphorus.The molecular weight of the material is:-
  • $$3.6\times 10^{6}$$
  • $$4.9\times 10^{4}$$
  • $$7.2\times 10^{6}$$
  • $$3.6\times 10^{4}$$
The percentage loss in weight after heating a pure sample of potassium chlorate (mol. $$wt.=122.5$$) will be:
  • 12.25
  • 24.50
  • 39.18
  • 19.6
A solution containing  $$500 g$$  of a protein per litre is isotonic with a solution containing  $$3.42 g$$  of sucrose per litre. The molecular mass of protein is:
  • $$5$$
  • $$146$$
  • $$34200$$
  • $$50000$$
The carbonate of a metal is isomorphous with $$MgCO_{3}$$ and contains $$6.091\%$$ of carbon. Atomic weight of the metal is nearly:
  • $$48$$
  • $$68.5$$
  • $$137$$
  • $$120$$
A compound contains $$28\%$$ Nitrogen, by mass. The possible molecular mass of the compounds is/are?
  • $$100$$
  • $$125$$
  • $$150$$
  • $$140$$
Which  of the following weights the  most?
  • $$10^{23}$$ molecules of $$H_{2}$$
  • $$1$$ mole of $$H_{2}O$$
  • $$1$$ mole of $$N_{2}$$
  • $$10^{22}$$ atoms of oxygen
Hemoglobin contains 0.334 % of iron by weight. The molecular weight of hemoglobin is approximately 67200.The number of iron atoms (Atomic weight of Fe is 56) present in one molecule of hemoglobin is 
  • 4
  • 6
  • 3
  • 2
Effective atomic number of the central metal atom in the compound/complex $$\mathrm { Cr } ( \mathrm { CO } ) _ { 6 }$$ is:
  • 34
  • 35
  • 36
  • 37
If an iodized salt contains $$1\%$$ of $$KI$$ and a person takes $$2\ g$$ of the salt every day, the iodine ions going into his body every day would be approximately $$(K=39, I=127)$$ 
  • $$9.5 \times 10^{21}$$
  • $$7.2 \times 10^{19}$$
  • $$7.2 \times 10^{21}$$
  • $$9.5 \times 10^{19}$$
1 atomic mass unit is equal to:
  • $$\tfrac{1}{12}^{th}$$ mass of a carbon-12 atom
  • $$1.66\times 10^{-24}\ g$$
  • $$6.023\times 10^{-23}\ g$$
  • $$6.023\times 10^{23}\ g$$
The critical density of the gas $$CO_2$$ is 0.44 $$g\ cm^{–3}$$ at a certain temperature. If $$r$$ is the radius of the molecule, $$r^3$$ in $$cm^3$$ is approximate: 

[N is Avogadro number]
  • $$\cfrac {25} {\pi N}$$
  • $$\cfrac {100} {\pi N}$$
  • $$\cfrac {6} {\pi N}$$
  • $$\cfrac {25} {4N\pi}$$
The Statue of Liberty is made of $$2.0\times 10^5$$ lbs of copper sheets bolted to a framework $$(1 lb =454 g)$$. How many atoms of copper are there on the statue?

(Atomic weight: $$Cu=63.5$$).
  • $$2.1\times 10^{27}$$
  • $$8.6\times 10^{29}$$
  • $$4.3\times 10^{26}$$
  • $$8.6\times 10^{26}$$
Number of $$HCl$$ molecules present in $$10$$ mL of $$0.1 N$$ $$HCl$$ solution is 
  • $$6.022 \times 10^{23}$$
  • $$6.022 \times 10^{22}$$
  • $$6.022 \times 10^{21}$$
  • $$6.022 \times 10^{20}$$
One gram molecule of any gas at $$NTP$$ occupies $$22.4\ L$$. This fact was derived from:
  • Dalton's theory
  • Avogardro's hypothesis
  • Berzelius hypothesis
  • Law of gaseous volume
The weight of $$H_{2}C_{2}O_{4},2H_{2}O$$ required to prepare 500 ml of 0.2 N solution is:
  • 1.26 g
  • 6.3 g
  • 1.575 g
  • 3.15 g
A gaseous mixture contains $$70\%N_{2}$$ and a $$30\%$$ unknown gas, by volume. If the average molecular weight of gaseous mixture is $$37.60$$, the molecular weight of unknown gas is:
  • $$42.2$$
  • $$60$$
  • $$40$$
  • $$50$$
$$12$$ gm of an alkaline earth metal gives $$14.8$$g of its nitride. The atomic mass of metal is:
  • $$12$$
  • $$24$$
  • $$20$$
  • $$40$$
A gas mixture contains $$50\%$$ helium and $$50\%$$ methane by volume. What is the percent by weight of methane in the mixture?
  • $$19.97\%$$
  • $$20.05\%$$
  • $$50\%$$
  • $$80.03\%$$
The solubility of potassium chloride in water at $$20^oC$$ is $$34.7g$$ in $$100g$$ of water. The density of solution is $$1.3g/ml$$. Calculate the % of mass/volume concentration of potassium chloride.
  • $$25.76\%$$
  • $$33.49\%$$
  • $$24.7\%$$
  • $$1.3\%$$
Number of $$g$$ of oxygen in $$32.2\ g\ Na_{2}SO_{4}\ 10H_{2}O$$ is:[$$Mol. w t=322$$ ]
  • $$16.0$$
  • $$2.24$$
  • $$18.0$$
  • $$22.4$$
In $$\overset { 14 }{ \underset { 7 }{ N }  } $$ if mass attributed to electron were doubled & the mass attributed to protons were halved, the atomic mass would become approximately:-
  • Halved
  • Doubled
  • Reduced by 25%
  • Remain same
The weight of 1 mole of a gas of density is $${\text{0}}{\text{.1784}}{\kern 1pt} {\kern 1pt} {\text{g}}{\kern 1pt} {{\text{L}}^{ - 1}}{\text{at}}{\kern 1pt} {\text{NTP}}{\kern 1pt} {\text{is}}{\kern 1pt}  - $$
  • 0.1784 g
  • 1 g
  • 4 g
  • 4 amu
Find the concentration of glucose in blood which have osmotic pressure $$\pi = 7.7 \ atm$$ at $$T = 25^oC$$
  • $$0.31M$$
  • $$0.45M$$
  • $$0.56M$$
  • $$0.89M$$
The crystalline salt $$Na_{2}SO_{4}.xH_{2}O$$ on heating loses 55.9% of its weight. The formula of the crystalline salt is :
  • $$Na_{2}SO_{4}. 5 H_{2}O$$
  • $$Na_{2}SO_{4}. 7H_{2}O$$
  • $$Na_{2}SO_{4}. 2H_{2}O$$
  • $$Na_{2}SO_{4}. 10H_{2}O$$
Calculate the concentration in $$m/v  \%$$ (in (mg/mL) of KCl solution which contains 0.0245 gm of KCl in 35 mL of solution.
  • 40
  • 60
  • 70
  • 30
The energy of an electron in $$n^{th}$$ orbit of hydrogen atom is:
  • $$\dfrac { 13.6 }{ { n }^{ 4 } } eV$$
  • $$\dfrac { 13.6 }{ { n }^{ 3 } } eV$$
  • $$\dfrac { 13.6 }{ { n }^{ 2 } } eV$$
  • $$\dfrac { 13.6 }{ { n } } eV$$
A $$5\%$$ solution of sucrose is isotonic with $$3\%$$ solution of a solute find molecular weight of that solute?
  • $$54 g$$
  • $$108 g$$
  • $$216 g$$
  • $$65 g$$
3 g of a solute was dissolved in 9 g of water. Find the percentage mass of solute
  • 25%
  • 33.33%
  • 18.7%
  • 20%
0.132 g of an organic compound gave 50 ml of $$N_2$$ at NTP. The weight percentage of nitrogen in the compound is close to 
  • 15
  • 20
  • 48.9
  • 47.34
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