You need 1.00L of a 0.10 M aqueous solution of HCl to do an experiment. How many moles of HCl do you need to prepare this solution? Since your lab can't measure out moles, convert the amount of HCl needed into grams. Once you’ve measured out that many grams of HCl, how do you finish making the solution?

The answer to your question is  3.65 g of HCl

Explanation:

Data

volume = 1 l

[HCl] = 0.1 M

moles of HCl = ?

Process

1.- Calculate the number of moles

Molarity = moles / volume

-Solve for moles

 moles = Molarity x volume

-Substitution

 moles = 0.1 x 1

-Result

 moles = 0.1 moles

2.- Convert moles to grams

-Calculate the molar mass of HCl

HCl = 1 + 35.5 = 36.5 g

-Convert

                     36.5 g of HCl 1 mol

                        x                   0.1 moles

                                x = (0.1 x 36.5) / 1

-Result

                               x = 3.65 g

-How to prepare the solution

Once I have weighed the mass of HCl, I place it in a volumetric flask and pour enough water till 1 l.

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explanation:

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