# A 15.00 mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 x 10^3 mL. The concentration of the final solution is 0.00383 M. What is the molarity of the original solution?

Apr 25, 2017

$\text{Molarity of original solution} = 1.277 M$

#### Explanation:

Solution 1: 15.00mL
Solution 2: 125.0mL
Solution 3: 25.00mL
Solution 4: 1000.mL

$\text{mols Solution 4} = 1000. m L \cdot 0.00383 M = \textcolor{t e a l}{0.00383 m o l s}$

$\text{Molarity Solution 3} = \frac{\textcolor{t e a l}{0.00383 m o l s}}{25.00 m L} = \textcolor{p u r p \le}{0.1532 M}$

$\text{mols Solution 2} = \textcolor{p u r p \le}{0.1532 M} \cdot 125.0 m L = \textcolor{\mathmr{and} \chi d}{0.01915 m o l s}$

$\text{Molarity Solution 1} = \frac{\textcolor{\mathmr{and} \chi d}{0.01915 m o l s}}{15.00 m L} = \textcolor{s a l m o n}{1.276666667 M}$

$\text{Molarity of original solution} = \textcolor{s a l m o n}{1.277 M}$