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What volume o...

Question

What volume of water must be added to $50 mL$ of a $0.5 M H_{2} S O_{4}$ to give a solution having a concentration of $0.1 M H_{2} S O_{4} ?$

200 mL

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250 mL

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105 mL

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550 mL

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Solution

The correct option is A $200 mL$
Let’s assume the volume after dilution to be $V mL$ and the concentration becomes $0.1 M$ .
$M_{1} V_{1} = M_{2} V_{2}$
$\Rightarrow (0.1 \times V) = (0.5 \times 50)$
On solving, $V = 250 mL$
So, the volume of water to be added $= (250 - 50) mL = 200 mL$

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What volume of water must be added to 50 mL of a 0.5 M H2SO4 to give a solution having a concentration of 0.1 M H2SO4?

The correct option is A 200 mLLet’s assume the volume after dilution to be V mL and the concentration becomes 0.1 M. M1V1=M2V2 ⇒(0.1×V)=(0.5×50) On solving, V=250 mL So, the volume of water to be added =(250−50) mL=200 mL

What volume of water must be added to $50 mL$ of a $0.5 M H_{2} S O_{4}$ to give a solution having a concentration of $0.1 M H_{2} S O_{4} ?$

The correct option is A $200 mL$
Let’s assume the volume after dilution to be $V mL$ and the concentration becomes $0.1 M$ .
$M_{1} V_{1} = M_{2} V_{2}$
$\Rightarrow (0.1 \times V) = (0.5 \times 50)$
On solving, $V = 250 mL$
So, the volume of water to be added $= (250 - 50) mL = 200 mL$