Match the columns. List - I List - II (A) 5 m of NaOH solution ( d solution = 0.6 g / ml ) Molarity of solution is (P) 16 M (B) 250 ml of H 2 O 2 solution provides 64 g of O 2 . Molarity of H

Question

Match the columns. List - I List - II (A) 5 m of NaOH solution ( d solution ​ = 0.6 g / ml ) Molarity of solution is (P) 16 M (B) 250 ml of H 2 ​ O 2 ​ solution provides 64 g of O 2 ​ . Molarity of H 2 ​ O 2 ​ solution is (Q) 1 M (C) 100 ml of 1 M − H 2 ​ SO 4 ​ solution (dsolution = 1.5 g / ml ) is mixed with 400 ml of water, density of fi nal solution = 1.25 g / ml . Molarity of resulting solution is (R) 2.5 M (D) 100 ml of 6 M − NaCl solution is mixed with 100 ml of 17% ( w / w ) AgNO 3 ​ solution ( d solution ​ = 8 g / ml). Molarity of Ag + ions in the resulting solution is (S) 0.227 M

TestHub · Accepted Answer

(A) 5 m NaOH

5 moles NaOH in 1000 gm solvent

Mass of solution $= (5 \times 40) + 1000 = 1200 gm$

Volume of solution $= \frac{1200}{0.6} \Rightarrow 2000 ml$

Molarity $= \frac{5 moles}{2 L} \Rightarrow 2.5 M$

(B) $4 mole H_{2} O_{2} \to H_{2} O + \frac{1}{2} 64 gm 2 mole O_{2}$

$M = 4 \times \frac{1000}{250} = 16 M$ $(C) H_{2} SO_{4} 100 ml, 1 M d = 1.5 gm / ml Mass = 100 \times 1.5 = 150 gm + Wa t er 400 ml d = 1 gm / ml Mass = 400 gm \to H_{2} SO_{4} resulting solution Mass = 400 + 150 \Rightarrow 550 d = 1.25 gm / ml V = 550/1.25 ml M = \frac{100 m moles}{550 ml} \times 1.25 = 0.227 M$

(D) NaCl

+

AgNO_{3} ⟶

AgCl + NaNO_{3}

$100 ml, 6 M$ 100 ml (ppt)

600 m moles $d = 8 gm / ml$

0.6 moles Mass = 100 x 8 gm

= 800 gm

17% (w/W)

100 gm → 17 gm AgNO₃

800 gm 17 x 8 gm AgNO₃

=136 gm AgNO₃

Moles = 136/170 = 0.8 moles

(L.R.)

0.6 moles 0.8 moles

- 0.2 moles

Moles of Ag⁺ = 0.2 moles

Total volume = 100 ml + 100 ml = 0.2 L

Molarity = 0.2 moles/0.2 L = 1 M

List - I	List - II
(A) 5 m of NaOH solution ( $d_{solution} = 0.6 g / ml$ ) Molarity of solution is	(P) 16 M
(B) 250 ml of $H_{2} O_{2}$ solution provides 64 g of $O_{2}$ . Molarity of $H_{2} O_{2}$ solution is	(Q) 1 M
(C) 100 ml of $1 M - H_{2} SO_{4}$ solution (dsolution $= 1.5 g / ml$ ) is mixed with 400 ml of water, density of fi nal solution $= 1.25 g / ml$ . Molarity of resulting solution is	(R) 2.5 M
(D) 100 ml of $6 M - NaCl$ solution is mixed with 100 ml of $17% (w / w) AgNO_{3}$ solution ( $d_{solution} = 8 g /$ ml). Molarity of $Ag^{+}$ ions in the resulting solution is	(S) 0.227 M

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