From doing some research on the site I have found that many people have posted about solutions of HCl where [\ce{HCl}] = \pu{1e-8 mol dm-3}
Here they are able to deduce
[\ce{H+}] = \frac{[\ce{HCl}]_0}{2} + \sqrt{\frac{[\ce{HCl}]_0^2}{4} + K_\mathrm{w}}
where [\ce{HCl}]_0 is the initial concentration of \ce{HCl} dissolved.
Can we make a generalisation of this and say if \ce{H_xA} is a strong acid that will dissociate fully when dissolved in water? Then if [\ce{H_xA}]_0 < \sqrt{K_\mathrm{w}} then the \mathrm{pH} of solution can be expressed by
\mathrm{pH} = -\log_{10} \left(\frac{x[\ce{H_xA}]_0}{2} + \sqrt{\frac{(x[\ce{H_xA}]_0)^2}{4} + K_\mathrm{w}}\right)
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