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?

Question

1132 views around the world

You can reuse this answer
Creative Commons License

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