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How many mL's of 4.00 M HCl (aq) are required to prepare 500.0 mL of 0.200...

How many mL's of 4.00 M HCl (aq) are required to prepare 500.0 mL of 0.200 M HCl (aq)?

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Answer #1

As we know the molarity of the solution is defined as the moles of solute present in the 1L solution.

It can be written in the mathematical form as:

Here the prepared solution have

volume(v)= 500mL

molarity= 0.200M

m= molar mass = molar mass of HCl=36.5gm/mol

By applying the rule of molarity we can calculate the mass of HCl.

The required mass is 3.65g of HCl are required to prepare the 0.200 M HCl in 500mL

Again 3.65gm of 4.00 M HCl are required to prepare the 0.2M HCl in 500mL of water.For this preparation of the solution, the volume of solvent is to to be determined by using the law of molarity calculator.

That is

Here w= 3.65g

m=36.5

Molarity= 4.00 M

Hence we need 25mL of 4.00M of HCl to prepared the 0.2 M of HCl in 500mL of water.

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