What volume of a solution that is 6.0*mol*L^-16.0⋅mol⋅L−1 HClHCl is required to make 1.00*L1.00⋅L of a 0.10*mol*L^-10.10⋅mol⋅L−1 solution?

1 Answer
anor277
Jun 1, 2017

We need under 20*mL20⋅mL of stock solution.

Explanation:

We use the old relationship, C_1V_1=C_2V_2C1V1=C2V2. The product in each side gives units of "moles"moles.

And so 6.0*mol*L^-1xxV_1=1.000*Lxx0.1*mol*L^-16.0⋅mol⋅L−1×V1=1.000⋅L×0.1⋅mol⋅L−1

and thus..............................

V_1=(1.000*Lxx0.1*mol*L^-1)/(6.0*mol*L^-1)=0.0167*L=16.7*mL.V1=1.000⋅L×0.1⋅mol⋅L−16.0⋅mol⋅L−1=0.0167⋅L=16.7⋅mL.

Do you add the water to the acid, or the acid to water? (I am not taking the p, the order of addition is important!)

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