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You need to make $10.0\,\text{L}$ of $1.2\,\text{M}$ $\text{KNO}_3$ . What molarity would the potassium nitrate solution need to be if you were to use only $2.5\,\text{L}$ of it?

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Convert between customary and metric systems

Full solution

Q. You need to make

10.0\,\text{L}

of

1.2\,\text{M}

\text{KNO}_3

. What molarity would the potassium nitrate solution need to be if you were to use only

2.5\,\text{L}

of it?

Identify Concentration: question_prompt: How concentrated does the $\text{KNO}_3$ solution need to be if using $2.5 \, \text{L}$ to make $10.0 \, \text{L}$ of $1.2 \, \text{M}$ solution?
Apply Dilition Formula: We need to find the concentration of the KNO $3$ solution that will be diluted to $10.0\,\text{L}$ . Use the dilution formula $M_1V_1 = M_2V_2$ , where $M_1$ is the concentration we need to find, $V_1$ is the volume of the concentrated solution, $M_2$ is the final concentration, and $V_2$ is the final volume.
Plug in Values: Plug in the known values: $M_1 \times 2.5 \, \text{L} = 1.2 \, M \times 10.0 \, \text{L}.$
Solve for M $1$ : Solve for $M1$ : $M1 = \frac{1.2 M \times 10.0 L}{2.5 L}.$
Calculate M $1$ : Calculate M $1$ : $M1 = \frac{12.0 \, \text{M} \cdot \text{L}}{2.5 \, \text{L}}$ .
Final Concentration: $M_1 = 4.8\,\text{M}$ . This is the concentration needed for the $2.5\,\text{L}$ of solution to make $10.0\,\text{L}$ of $1.2\,\text{M}\,\text{KNO}_3$ solution.

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