Please clarify: do you need a density of 2.1g/L or so you want a concentration of 2.1g/L. I suspect you need the latter which is trivial; take 2.1g of ZnCl2 and make it up to 1.00 L by adding distilled water.
Do you mean a density of 2.1 g/mL and not 2.1 g/L? In that case, knowledge of partial molar volumes would be helpful.
According to this: http://www.zaclon.com/pdf/zinc_chloride_soln_tech_grade_625_msds.pdf
A 62.5% zinc chloride solution has a density of 1.79 g/mL. A saturated solution would be closer to 80% zinc chloride, and that might be closer to the density you want.
Tabulated values for the density of ZnCl2 aqueous solutions, at temperatures ranging from 0 ºC to 100 ºC, can be retrieved from (e.g.): R.H. Perry, D.W. Green, J.O. Maloney (Eds.), "Perry's Chemical Engineers’ Handbook", 7th ed., McGraw-Hill, 1997, cf. Table 2-103; E.W. Washburn (Ed.-in-chief), International Critical Tables (ICT), Vol. III, McGraw-Hill, 1928, p. 64.
how do I prepare a solution of Zinc Chloride at 50% weight/volume concentration
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