# How many equivalents of sulfuric acid are in 20 mL of 0.35 N H2SO4 solution? How many grams?

## Question:

How many equivalents of sulfuric acid are in 20 mL of 0.35 N {eq}H_2SO_4 {/eq} solution? How many grams?

## Molar Mass:

The molar mass is a fixed quantity for chemical compounds that gives the mass per mole of a compound. The molar mass is essential in preparing reagents in chemistry experiments such that we multiply the number of moles we need for our solution to the molar mass to determine how much of the substance we need.

## Answer and Explanation:

Determine the equivalent number of moles of {eq}\displaystyle H_2SO4 {/eq} there is in the given solution by multiplying the volume, {eq}\displaystyle V {/eq}, in liters, to the concentration, {eq}\displaystyle M {/eq}, of the solution.

{eq}\begin{align} \displaystyle n &= VM\\ &= 0.02\ L\times 0.35\ M\ H_2SO_4\\ &= 0.007\ mol\ H_2SO_4 \end{align} {/eq}

Now, we determine the mass of {eq}\displaystyle H_2SO_4 {/eq} by multiplying the acquired number of moles to the molar mass, {eq}\displaystyle 98.079 \rm{g/mol} {/eq}. We proceed with the solution.

{eq}\begin{align} \displaystyle m &=0.007\ mol\ H_2SO_4\times 98.079 \rm{g/mol}\\ &\approx 0.7\ g\ H_2SO_4 \end{align} {/eq}