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Praxis Chemistry (5245) Practice Tests & Test Prep by Exam Edge - Free Test


Our free Praxis Chemistry Content Knowledge (5245) Practice Test was created by experienced educators who designed them to align with the official Educational Testing Service content guidelines. They were built to accurately mirror the real exam's structure, coverage of topics, difficulty, and types of questions.

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Praxis Chemistry Content Knowledge - Free Test Sample Questions

What is the resulting molarity after diluting 250 ml of 2 M KOH solution to 2.0 L?

Correct Answer:
0.25 moles

to find the resulting molarity of a solution after dilution, we can use the dilution formula: m1 * v1 = m2 * v2, where m1 is the initial molarity, v1 is the initial volume, m2 is the final molarity, and v2 is the final volume.

in this specific problem, we are given that 250 ml (or 0.250 liters) of a 2 m koh solution is diluted to a final volume of 2.0 liters. we need to find the resulting molarity, m2, of the diluted solution.

plugging the given values into the dilution formula: - m1 (initial molarity) = 2 m - v1 (initial volume) = 0.250 liters - v2 (final volume) = 2.0 liters - m2 (final molarity) is what we want to find.

applying the values: \[ m1 \times v1 = m2 \times v2 \] \[ 2 \text{ m} \times 0.250 \text{ l} = m2 \times 2.0 \text{ l} \] \[ 0.5 \text{ m} \cdot \text{l} = m2 \times 2.0 \text{ l} \]

to isolate m2, divide both sides of the equation by the final volume (2.0 l): \[ m2 = \frac{0.5 \text{ m} \cdot \text{ l}}{2.0 \text{ l}} \] \[ m2 = 0.25 \text{ m} \]

therefore, the molarity of the koh solution after dilution to 2.0 liters is 0.25 m. this means the solution becomes less concentrated as we expected due to dilution with more solvent (water, in most cases). the final molarity provides the concentration of koh ions per liter of solution in the new diluted state.