What is the volume of the solution that would result by diluting 60.00 mL of 9.19×10−2 M NaOH to a concentrati?
What is the volume of the solution that would result by diluting 60.00 mL of 9.19×10−2 M NaOH to a concentration of 1.40×10−2 M?
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We know that M = m/V where M is the molarity, m is the amount of moles, and V is the volume of the solution.
With M = m/V, we can arrange to give m = MV. Since this is constant for both solutions (no NaOH is added), we have:
M₁V₁ = M₂V₂ (you have probably seen this equation)
==> (9.19 x 10^-2 mol/L)(0.060 L) = (1.40 x 10^-2 mol/L)V₂
==> V₂ = (9.19 x 10^-2 mol/L)(0.060 L)/(1.40 x 10^-2 mol/L) = 394 mL.
I hope this helps!