# What is the molar concentration of sulfuric acid is we have an "80% w/w" concentration with rho_"solution"=1.73*g*mL^-1?

Mar 26, 2016

Approx. $14$ $m o l \cdot {L}^{-} 1$

#### Explanation:

We know that $1$ $m L$ of sulfuric acid has a mass of $1.73$ $g$, of which $1.384$ $g$ is ${H}_{2} S {O}_{4}$.

So $\text{concentration}$ $=$ $\text{Moles of solute"/"Volume of solution}$

$\frac{1.384 \cdot \cancel{g}}{98.079 \cdot \cancel{g} \cdot m o {l}^{-} 1}$ $\times$ 1/(1*cancel(mL)xx(10^-3L*cancel(mL^-1)) $=$ ?? mol*L^-1

$\text{98% sulfuric acid (w/w)}$ has a density of $1.83 \cdot g \cdot m {L}^{-} 1$. What is the molarity of this solution.