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What would be the final volume of a diluted solutions that was made by diluting 250 mL a 4.5M solutions of H2SO4 to make a 3.5M solution? How much water would have to be added to reach the final volume?

Answer 1

You know you should add acid to water.................I get approx., #71*mL#

Normally, we add ACID to WATER. However, the acid is not too concentrated, and so you would get away with reverse addition.

#"Molarity or concentration"="Moles of solute"/"Volume of solution"#

And thus, since #C_1V_1=C_2V_2#........(because the moles of solute was a constant and depends on the initial concentration).

#V_2=(C_1V_1)/C_2=(250*mLxx4.5*mol*L^-1)/(3.5*mol*L^-1)=321.4*mL#

But since #V_1=250*mL#, we need to ADD #71.4*mL# to the initial #250*mL# volume to give the required concentration.

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Answer 2

Naomi Aronson

The final volume of the diluted solution would be 321.43 mL. To reach the final volume, 71.43 mL of water would need to be added.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.