Aqueous solution of ${\mathrm{BaBr}}_2$ gives yellow precipitate with:

${\mathrm{BaBr}}_2$ in aqueous solution gives yellow ppt with  ${\mathrm{K}}_2{\mathrm{CrO}}_4$ as well as with  ${\mathrm{AgNO}}_3$ with ${\mathrm{K}}_2{\mathrm{CrO}}_4$, barium bromide gives yellow ppt of barium chromate whereas with ${\mathrm{AgNO}}_3$ it gives light yellow ppt of silver bromide.

$\begin{array}{l}{\mathrm{K}}_2{\mathrm{CrO}}_4+{\mathrm{BaBr}}_2\to {\mathrm{CrO}}_4\downarrow \text{ (yellow) }+2\mathrm{KBr}\\ {\mathrm{AgNO}}_3+{\mathrm{BaBr}}_2\to {\mathrm{BaNO}}_3+2\mathrm{AgBr}\downarrow \text{ (lightyellow) }\end{array}$