What will be the molarity of $30 m L$ of $0.5 M$ $H_{2} {S O}_{4}$ solution diluted to $500 m L$ ?

0.3 M

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0.03 M

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3 M

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0.103 M

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Solution

The correct option is D $0.03 M$
Dilution Formula,
$M_{1} V_{1} = M_{2} V_{2}$

$M_{2} = \frac{M_{1} V_{1}}{V_{2}}$

In the problem $M_{1} = 0.5 M, V_{1} = 30 m L, V_{2} = 500 m L$

= $\frac{0.5 \times 30}{500} = \frac{15}{500} = 0.03 M$

Hence, option $B$ is correct.

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What will be the molarity of 30mL of 0.5M H2SO4 solution diluted to 500mL?

The correct option is D 0.03MDilution Formula,M1V1=M2V2M2=M1V1V2In the problem M1=0.5M,V1=30mL,V2=500mL=0.5×30500=15500=0.03MHence, option B is correct.

What will be the molarity of $30 m L$ of $0.5 M$ $H_{2} {S O}_{4}$ solution diluted to $500 m L$ ?

The correct option is D $0.03 M$
Dilution Formula,
$M_{1} V_{1} = M_{2} V_{2}$

$M_{2} = \frac{M_{1} V_{1}}{V_{2}}$

In the problem $M_{1} = 0.5 M, V_{1} = 30 m L, V_{2} = 500 m L$

= $\frac{0.5 \times 30}{500} = \frac{15}{500} = 0.03 M$

Hence, option $B$ is correct.