Precipitation of a lead(II) sulfate
The stability constant of $\ce{Pb−EDTA}$ complex is $\ce{10^{18}}$, which is huge. The solubility product of $\ce{PbSO_4}$ is $10^{−8}$
, which cannot be compared to the effect of $\ce{EDTA}$. So the precipitate $\ce{PbSO4}$ must be soluble in $\ce{EDTA}$ solutions. These numerical data have been taken from J. G. Stark, Chemistry Data Book, John Murray, London, $1994$