An isotonic solution will produce an osmotic pressure of 10.00 atm measured against pure water at $37°C$. How many grams of $NaCl$ must be dissolved in one litre of water to produce at isotonic solution

Given data : It is given to identify How many grams of $NaCl$ must be dissolved in one litre of water to produce at isotonic solution

Explanation :

At $37°C$, an isotonic solution has an osmotic pressure of 10.00 atm when measured against pure water. To make an isotonic solution, W grams of $NaCl$ must be dissolved in one litre of water.

$NaCl$ has a molar mass of $58.5 g/mol.$

$$\begin{gathered} Molecular concentration. \\ \mathrm{C}=\frac{\mathrm{Wg}}{58.5 \mathrm{g}/\mathrm{mol}\times 1 \mathrm{L}} \\ \mathrm{C}=\frac{\mathrm{W}}{58.5}\mathrm{M} \\ \mathrm{Isotonic} \mathrm{solutions} \mathrm{have} \mathrm{the} \mathrm{same} \mathrm{osmotic} \mathrm{pressure}. \\ \mathrm{\pi }=\mathrm{iCRT} \\ 10 \mathrm{atm}=2\times \frac{\mathrm{W}}{58.5}\mathrm{M}\times 0.08206 \mathrm{L} \mathrm{atm}/\mathrm{mol}/\mathrm{K}\times (37+273)\mathrm{K} \\ \mathrm{W}=11.4 \mathrm{g} \\ \mathrm{To} \mathrm{make} \mathrm{an} \mathrm{isotonic} \mathrm{solution}, \mathrm{dissolve} 11.46\mathrm{g} \mathrm{grams} \mathrm{of} \mathrm{NaCl} \mathrm{in} \mathrm{one} \mathrm{litre} \mathrm{of} \mathrm{water}. \\ \mathrm{NaCl}\rightleftharpoons {\mathrm{Na}}^{+}+{\mathrm{Cl}}^{-} \end{gathered}$$

Hence, the correct option (A).11.46g