Calibration data for a bromide ion$-$selective electrode $($ISE$)$ was collected and recorded in the table. The potential of the ISE was measured against a saturated calomel electrode $($SCE$).$ All solutions were buffered at a $pH$ of $7\mathrm{.}56.$ A linear calibration curve can be constructed from this data as a plot of potential $($in $mV)$ vs$.log[B{r}^{-}].$

Determine the slope and $y-$intercept of such a plot of the calibration data given.

$\backslash$table$[[[B{r}^{-}](M),$Potential $($mV$)],[0\mathrm{.}300,-21\mathrm{.}4],[0\mathrm{.}0300,36\mathrm{.}6],[0\mathrm{.}00300,96\mathrm{.}5],[0\mathrm{.}000300,155\mathrm{.}4],[0\mathrm{.}0000300,224\mathrm{.}8]]$

slope $=$

$y-$intercept $=$

Two unknown solutions were tested for $B{r}^{-}$using the same bromide ISE. The potential reading for unknown $1$ was $-19\mathrm{.}9mV,$ and the potential reading for unknown $2$ was $186\mathrm{.}1mV.$ Using the calibration curve you constructed, determine the concentration of $B{r}^{-}$in each unknown solution.

unknown $1[B{r}^{-}]=$

M

unknown $2[B{r}^{-}]=$

M