The Notes: What is the molarity of a 250. mL H2SO4 solution that was made from a 20.0 mL of a 10.0 M stock solution?

Wednesday, September 1, 2010

What is the molarity of a 250. mL H2SO4 solution that was made from a 20.0 mL of a 10.0 M stock solution?

You can solve this equation by using the following dilution formula:

$\displaystyle~{M}_{{1}}$ x $\displaystyle~{V}_{{1}}$ = $\displaystyle~{M}_{{2}}$ x $\displaystyle~{V}_{{2}}$

$\displaystyle~{M}_{{1}}$ = molarity of the stock solution = 10.0 M

$\displaystyle~{V}_{{1}}$ = volume of the stock solution = 20.0 mL

$\displaystyle~{M}_{{2}}$ = molarity of the diluted solution = ? M

$\displaystyle~{V}_{{2}}$ = volume of the diluted solution = 250. mL

Step 1: Rearrange the dilution formula to solve for $\displaystyle~{M}_{{2}}$ .

To rearrange the formula, divide both sides of the formula by $\displaystyle~{V}_{{2}}$ . The $\displaystyle~{V}_{{2}}$ variables on the right side of the equation cancel out leaving you with:

( $\displaystyle~{M}_{{1}}$ x $\displaystyle~{V}_{{1}}$ )/ $\displaystyle~{V}_{{2}}$ = $\displaystyle~{M}_{{2}}$

Step 2: Rewrite the formula so that the unknown variable is on the left.

$\displaystyle~{M}_{{2}}$ = ( $\displaystyle~{M}_{{1}}$ x $\displaystyle~{V}_{{1}}$ )/ $\displaystyle~{V}_{{2}}$

Step 2: Plug in the known values and solve for $\displaystyle~{M}_{{2}}$ .

$\displaystyle~{M}_{{2}}$ = [10.0 M x 20.0 mL]/250. mL

= 0.800 M

The Notes

Wednesday, September 1, 2010

What is the molarity of a 250. mL H2SO4 solution that was made from a 20.0 mL of a 10.0 M stock solution?

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