\(10 \mathrm{~g}\) of \(\mathrm{NaOH}\) is dissolved in \(500 \mathrm{~mL}\) of aqueous solution. Calculate…
\(10 \mathrm{~g}\) of \(\mathrm{NaOH}\) is dissolved in \(500 \mathrm{~mL}\) of aqueous solution. Calculate the molarity of this solution? (Given, formula weight of \(\mathrm{NaOH}=40\) )
\(0.5 \times 10^{-3} \mathrm{M}\)
\(0.4 \mathrm{M}\)
\(0.25 \times 10^{-3} \mathrm{M}\)
\(0.5 \mathrm{M}\)
Solution
\(\therefore\) Molarity \(=\frac{\text { Mass of solute }\left(\text { in } \mathrm{gL}^{-1}\right)}{\text { Molar of solute }\left(\text { in } \mathrm{g} \mathrm{mol}^{-1}\right)}\)
\(=\frac{\frac{10}{500} \times 1000}{40} \mathrm{M}=0.5 \mathrm{M}\)