Multiple Choice
What is the molarity of a solution that contains 17 g of NH3 (ammonia) in 0.50 L of solution? (Molar mass of NH3 = 17 g/mol)
6. Chemical Quantities & Aqueous Reactions
Molarity
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What volume of a 2.00 M solution of sulfuric acid is needed to provide 0.0500 mol of sulfuric acid?
A
0.2000 L
B
0.0500 L
C
0.0250 L
D
0.1000 L
Verified step by step guidance1
Identify the given information: You have a 2.00 M solution of sulfuric acid (H₂SO₄) and you need to find the volume that contains 0.0500 mol of H₂SO₄.
Recall the formula for molarity: \( M = \frac{n}{V} \), where \( M \) is the molarity, \( n \) is the number of moles, and \( V \) is the volume in liters.
Rearrange the formula to solve for volume: \( V = \frac{n}{M} \).
Substitute the known values into the equation: \( V = \frac{0.0500 \text{ mol}}{2.00 \text{ M}} \).
Calculate the volume to find out how many liters of the solution are needed to provide 0.0500 mol of sulfuric acid.
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