Sulfuric Acid with a molarity of .001 has a pH of 2.75. You want to dilute 1mL of this acid to a pH of 5.2. If you want to dilute 1mL of the original solution, what would the final volume of solution be?

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Answer 1 · 2018-05-19T15:28:59

282.1 ml

For the original solution:

#sf(pH=-log[H^+]=2.75)#

#sf([H^+]=0.00178color(white)(x)"mol/l")#

For the target solution:

#sf(pH=-log[H^+]=5.2)#

#sf([H^+]=6.31xx10^(-6)color(white)(x)"mol/l")#

This means the dilution factor to go from pH 2.75 to pH 5.2 will be:

#sf(0.00178/(6.31xx10^(-6))=282.1)#

This means you take 1 ml of the original solution and make it up to a final volume of 282.1 ml