What mass and volume of "25% orthophosphoric acid" is required for a 1.0*mol*L^-1 solution of H_3PO_4(aq)?

1 Answer
anor277
Jul 4, 2017

You need to quote the "density", rho, "of 25% orthophosphoric acid".

Explanation:

And http://pubs.acs.org/doi/abs/10.1021/ie50546a062 quotes rho=1.17*g*mL^-1. This value should have been quoted with the question.

And so we can work out the concentration, by considering just a "litre volume".

We need ((97.99*g)/(97.99*g*mol^-1))/(1.0*L " of solution").

And so we need 97.99*g with respect to H_3PO_4.

=(97.99*g)/(25%xx1.17*g*mL^-1)=335.0*1/(1/(mL))=335.0*mL

And so we take a 335.0*mL volume of 25%(w/w) H_3PO_4, and dilute it up to a ONE LITRE volume. The order of addition is important, because "if you SPIT in acid it spits back........"

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