Practice Concentration Of Solutions (molarity, Ppm) (1.3) - Chapter 1: Stoichiometric Relationships

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6 sample questions

Question 1.
What is the molarity of a solution with 2 moles of solute in 1 dm³ of solution?
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Use the formula M = n/V.
Question 2.
How many grams of NaCl are needed to prepare 1 liter of a 1 M solution?
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Remember the relationship of moles and grams.
3Question 3.
What is molarity defined as?
- A measure of pressure in a liquid.
- A measure of concentration in moles per liter.
- A measurement of temperature.
- A measure of mass.
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Recall the definition given earlier.
4Question 4.
Dilution affects the concentration of a solution.
- True
- False
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Consider how adding more solvent changes concentration.
Question 5.
You have a 0.25 M NaOH solution. How many grams of NaOH do you need to prepare 3 L?
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Find moles first: 0.25 moles x 3 L = 0.75 moles. Convert using molar mass: 0.75 moles x 40 g/mol.
Question 6.
Calculate the concentration in ppm if 2 mg of a pollutant is found in 100 L of water.
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Apply the conversion: 2 mg / 100L = (2 mg / 0.1 kg) x 1,000,000.

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