How much Ca NO 3 2 in mg must be present in a 50 mL solution with 2 . 35 ppm of Ca ? ρ = 1 g cc - 1

Given, Concentration of Ca = 2 . 35 ppm Volume of solution = 50 mL Parts per million ppm = Mass of solute ( g ) Volume of solution ( mL ) × 10 6 2 . 35 = Mass of Ca in g 50 × 10 6 Mass of Ca = 117 . 5 × 10 - 6 g Moles of Ca = Weight Atomic weight = 117 . 5 × 10 - 6 40 = 2 . 93 × 10 - 6 mol Ca Moles of Ca = moles of Ca NO 3 2 = 2 . 93 × 10 - 6 mol Mass of Ca NO 3 2 = n mole × Molar mass = 2 . 93 × 10 - 6 × 164 = 480 . 5 × 10 - 6 g = 0 . 48 mg .

What is the molarity of NaCl solution having 1 . 52 ppm of Na and the solution density is 1 . 0 g / cm 3 ?

Given, Na = 1 . 52 ppm Density of solution = 1 g cm - 3 Parts per million ppm = mass of solute g mass of solution g × 10 6 So the ⇒ mass of Na = 1 . 52 g Mass of solution = 10 6 g Density = mass g volume mL 1 g ml - 1 = 10 6 Volume of solution mL Volume of solution = 10 3 litre Molarity means moles of solute per litre solution. M = n solute V solution = w M × V solution L = 1 . 52 23 × 10 3 = 6 . 6 × 10 - 5 M .

Calculate the volume of H 2 O to be added to 50 mL of HNO 3 having density 1 . 5 g mL - 1 and 63 . 0 % by weight to have one molar solution.

Given HNO 3 is 63 .0 % by weight. W HNO 3 = 63 . 0 g W Solution = 100 g Moles of HNO 3 = Weight Molecular weight = 63 63 = 1 mole Density of solution = 1 . 5 g ml - 1 Density = mass volume = 1 .5 = 100 V solution mL V solution = 100 1 .5 = 66 .7 ml Molarity means number of moles of solute. Present per litre of the solution M = n solute v solution L = 1 × 1000 66 .7 = 15 M According to dilution law, moles of solute does not change. M 1 V 1 = M 2 V 2 15 × 50 = 1 × V 2 V 2 = 750 ml So added volume of water = V 2 − V 1 = 750 − 50 = 700 ml

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$2.4 g$ of pure $Mg$ (atomic mass $24$ ) is dropped in $100 mL$ of $1 N HCl$ . What is true?

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Important Questions on Some Basic Concepts, Mole Concept and Stoichiometry

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.4>Q 13

$A + B \to A_{3} B_{2}$ (unbalanced)

$A_{3} B_{2} + C \to A_{3} B_{2} C_{2}$ (unbalanced)

Above two reactions are carried out by taking $3$ moles each of $A$ and $B$ and one mole of $C$ . Then which option is/are correct?

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IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.4>Q 14

27 g

of carbon is mixed with

88 g

of oxygen and is allowed to burn to produce

{CO}_{2}

, then:

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.4>Q 15

A mixture containing $64.0 g H_{2}$ and $64.0 g O_{2}$ is ignited so that water is formed as follows: $2 H_{2} + O_{2} ⟶ 2 H_{2} O$ . Which of the following statements is/are correct?

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.4>Q 16

Which of the following is/are correct? The following reaction occurs:

${Na}_{2} {CO}_{3} + 2 HCl ⟶ 2 NaCl + {CO}_{2} + H_{2} O$

$106.0 g$ of ${Na}_{2} {CO}_{3}$ reacts with $109.5 g$ of $HCl$ .

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Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.5>Q 1

How much

Ca {({NO}_{3})}_{2}

mg

must be present in a

50 mL

solution with

2.35 ppm

Ca ? (ρ = 1 g {cc}^{- 1})

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IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.5>Q 1

What is the molarity of

NaCl

solution having

1.52 ppm

Na

and the solution density is

1.0 g / {cm}^{3} ?

HARD

JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.5>Q 2

Calculate the ionic strength (in

g L^{- 1}

) of a solution containing

0.2 M NaCl

and

0.1 M {Na}_{2} {SO}_{4}

HARD

JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 1 - Some Basic Concepts, Mole Concept and Stoichiometry>DPP 1.5>Q 3

Calculate the volume of

H_{2} O

to be added to

50 mL

{HNO}_{3}

having density

1.5 g {mL}^{- 1}

and

63.0 %

by weight to have one molar solution.

2.4 g of pure Mg (atomic mass 24) is dropped in 100 mL of 1 N HCl. What is true?

Important Questions on Some Basic Concepts, Mole Concept and Stoichiometry

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$2.4 g$ of pure $Mg$ (atomic mass $24$ ) is dropped in $100 mL$ of $1 N HCl$ . What is true?