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3 years ago

How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 101.5 mL of 0.17 M H2SO4?

Chemistry

1 answer:

elena-14-01-66 [18.8K]3 years ago

6 0

Answer:

3.451 mL.

Explanation:

It is a dilution process.

We have the rule states that the no. of millimoles before dilution is equal to the no. of millimoles after dilution.

<em>(MV) before dilution = (MV) after dilution</em>

M before dilution = 5.0 M.

V before dilution = ??? mL.

M after dilution = 0.17 M.

V after dilution = 101.5 mL.

∴ The volume before dilution = (MV) after dilution / M before dilution = (0.17 M)(101.5 mL) / (5.0 M) = 3.451 mL.

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Tanya [424]

Answer:

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In this case for the solution you are given, we first use the mass to compute the moles of CuNO3:

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Next, knowing that the molarity has units of moles over liters, we can solve for volume as follows:

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By plugging in the moles and molarity, we obtain:

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47.0ml of a HBr solution were titrated with 37.5ml of a 0.215M LiOH solution to reach the equivalence point. what is the molarit

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Why?

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