Calculating pH of the 1,96 % H3PO4 solution

[brunetteangel]

Homework Statement

Calculate pH of the 1,96% solution of H3PO4 (ρ≈1 g/cm^3). Take in account only the first constant of dissociation (7,5 * 10^-3 mol/cubic dm). The reduction of the concentration of H3PO4 because of dissociation can be ignored.

% = 1,96%
ρ (H3PO4) ≈1 g/cm^3
K = 7,5 * 10^-3 mol/cubic dm

Homework Equations

No equations in this task.

The Attempt at a Solution

Couldn't even attempt to solve it, because I don't know how to put the information together.

 

[Borek]

Convert to the molar concentration first.

You don't know anything about calculating pH of a weak acid? Equilibrium? Dissociation constants?

 

[brunetteangel]

I know a few formulas, but I think I can't use any of them in this task yet, because I don't have enough information.

And which formula is used for molar concentration, this one:

c (substance) = n (substance) / V (whole solution volume)

or this one:

b (substance) = n (substance) / m (mass of solvent)

I know that pH can be calculated as

pH = -log [H+] / mol dm^-3

but that doesn't help at the moment. :/

nor this one:

[H+] = Kw / [OH-]

I also know this:

K = alpha^2 * c

But none of this helps. :/

 

[Borek]

There is enough information.

First things first - you have to find a way to convert a %w/w concentration (given) to the molar concentration.

Then it will be about dissociation. Can you write reaction equation for the first step of the phosphoric acid dissociation? Can you write formula for the equilibrium constant for this reaction? This will be identical to the definition of the dissociation constant K_a1 (given in the question, just marked K).