SATHEE: Some Basic Concepts Of Chemistry Question 59

Some Basic Concepts Of Chemistry Question 59

Question: What is the molarity of $S O_{4}^{2 -}$ ion in aqueous solution that contain 34.2 ppm of $A l_{2} {(S O_{4})}_{3}$ ? (Assume complete dissociation and density of solution 1 g/mL)

Options:

A) $3 \times 10^{- 4} M$

B) $2 \times 10^{- 4} M$

C) $10^{- 4} M$

D) None of these

Show Answer

Answer:

Correct Answer: A

Solution:

[a] $\frac{m a s s o f A l_{2} {(S O_{4})}_{3}}{m a s s o f w a t e r} \times 10^{6} = 34.2$ 1 litre solution contains 1000 g of water

$\Rightarrow$ In 1 litre solution, mass of $A l_{2} {(S O_{4})}_{3} = \frac{34.2 \times 1000}{10^{6}} = 34.2 m g$ Molarity of $A l_{2} {(S O_{4})}_{3} = \frac{34.2 \times 10^{- 3}}{342} M = 10^{- 4} M$

$\underset{10^{, -, 4} M}{A l_{2} {(S O_{4})}_{3}}, (a q) \overset{}{\to} \underset{2 \times 10^{- 4} M, 3 \times 10^{- 4} M}{2 A l^{3 +} (a q) + 3 S O_{4}^{2 -} (a q)},] [[S O_{4}^{2 -}] = 3 \times 10^{- 4} M]$

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Some Basic Concepts Of Chemistry Question 59

Question: What is the molarity of SO42− ion in aqueous solution that contain 34.2 ppm of Al2(SO4)3 ? (Assume complete dissociation and density of solution 1 g/mL)

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Question: What is the molarity of $S O_{4}^{2 -}$ ion in aqueous solution that contain 34.2 ppm of $A l_{2} {(S O_{4})}_{3}$ ? (Assume complete dissociation and density of solution 1 g/mL)