Question #12ca1
1 Answer
Here's what I got.
Explanation:
The underlying principle of a dilution is that you can decrease the concentration of the solution by
- keeping the number of moles of solute constant
- increasing the total volume of the solution
So, in order to dilute a solution you must increase its volume without changing the amount of solute it contains.
Let's assume that solution
#["A"]_0 = n_A/V_(A0)#
#["A"]_0 = n_A/(0.3 * 10^(-3)"L") = (10/3 * 10^3 * n_A)color(white)(a)"mol L"^(-1)#
After you mix this solution with solution
#V_"total" = "0.3 mL" + "6.7 mL" = "7.0 mL"#
Keeping in mind the fact tha the resulting solution must contain
#["A"]_"dil" = n_A/(7.0 * 10^(-3)"L") = (1/7 * 10^3 * n_A)color(white)(a)"mol L"^(-1)#
So, by what factor,
#"D.F." = ( 10/3 * color(blue)(cancel(color(black)(10^3 * n_a))) color(red)(cancel(color(black)("mol L"^(-1)))))/(1/7 * color(blue)(cancel(color(black)(10^3 * n_a))) color(red)(cancel(color(black)("mol L"^(-1)))))#
#"D.F." = 10/3 * 7 = color(green)(bar(ul(|color(white)(a/a)23.3color(white)(a/a)|)))#
This tells you that the resulting solution is
An interesting thing to notice here is that you can get the dilution factor by dividing the final volume by the initial volume of the solution
#"D.F." = (7.0 color(red)(cancel(color(black)("mL"))))/(0.3color(red)(cancel(color(black)("mL")))) = color(green)(bar(ul(|color(white)(a/a)23.3color(white)(a/a)|))) -># for solution#"A"#
The exact same approach can be used to find the dilution of
#"D.F." = (7.0color(red)(cancel(color(black)("mL"))))/(6.7color(red)(cancel(color(black)("mL")))) = color(green)(bar(ul(|color(white)(a/a)1.04color(white)(a/a)|))) -># for solution#"B"#
So, to sum this, the dilution factor for a given dilution is equal to
#color(blue)(|bar(ul(color(white)(a/a)"D.F." = "initial concentration"/"final concentration" = "final volume"/"initial volume"color(white)(a/a)|)))#