Salt solution$\underset{\mathrm{Salt} \mathrm{solution}}{\left[\mathrm{X}\right]}\stackrel{\mathrm{dil}. \mathrm{HCl}}{\to }$$\underset{\mathrm{White} \mathrm{ppt}}{\left[\mathrm{Y}\right]}$

                                                              $\downarrow$

           If ppt.is washed by decantation and dilute is added 

                   $\underset{\mathrm{White} \mathrm{ppt}.\left(\mathrm{Z}\right)}{\downarrow }$

Here, white ppt. of ['Y'] is

By adding a solution containing chloride ions to a solution of lead(II) nitrate, white precipitate lead(II) chloride can be produced. You might use sodium chloride solution to give the chloride ions, but it is typically quicker to simply add some weak hydrochloric acid.

${\mathrm{Pb}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)\to {\mathrm{PbCl}}_2\left(\mathrm{s}\right)$