What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)

Question

BlackTom AI · Accepted Answer

To tackle this problem, start by converting the mass of solute into moles using the molar mass: moles = mass / molar mass = 56 g / 26 g/mol ≈ 2.154 mol. Next, convert the volume to liters: 959 mL = 0.959 L. The molarity is moles of solute per liter of solution, so M = 2.154 mol / 0.959 L ≈ 2.246 M, which rounds to about 2.2 M.

Option by option:
- 1.5 M: This underestimates either the mole amount or overestimates the volume effect. If you plug in 1.5 M and solve for required moles, you’d need 1.5 M × 0.959 L ≈ 1.439 mol, which is far less than the 2.154 mol actually present. Hence incorrect.
- 2.2 M: This matches the calculation we performed (approximately 2.246 M, rounding to two significant figures gives 2.2 M). It aligns with both the mole and volume data.
- 2.1 M: This is close but would require either a slightly smaller mole amount or a slightly larger volume to achieve exactly 2.1 M. Since the actual computed value is about 2.246 M, 2.1 M is not the correct result.
- 0.0022 M: This is orders of magnitude too small. Achieving such a low concentration would require a far smaller amount of solute or a vastly larger volume, not consistent with the given numbers.

Overall, the calculation steps—convert mass to moles, convert volume to liters, then divide moles by liters—lead to a value near 2.2 M, making 2.2 M the correct choice among the options.

What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)Single choice

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