# A 24.5*g mass of sulfuric acid is dissolved in enough water to make a solution of 100*mL volume. What is the concentration with respect to H_2SO_4?

Oct 27, 2016

$\text{Molarity}$ $=$ $\text{Moles of Solute"/"Volume of solution}$

#### Explanation:

$\text{Moles of sulfuric acid}$ $=$ $\frac{24.5 \cdot g}{98.08 \cdot g \cdot m o {l}^{-} 1}$

$\text{Concentration of sulfuric acid}$

$=$ $\frac{24.5 \cdot g}{98.08 \cdot g \cdot m o {l}^{-} 1} \times \frac{1}{100 \cdot c {m}^{3} \times {10}^{-} 3 \cdot L \cdot c {m}^{-} 3}$

$=$ ??mol*L^-1.

Note that this answer is dimensionally consistent. We require an answer with units of concentration, and we got one! This is why scientists place so much emphasis on units; it helps to get the calculations right.

What is the concentration with respect to ${H}_{3} {O}^{+}$?
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