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

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BlackTom AI · Accepted Answer

We start by parsing the given quantities. The solute mass is 56 g, and the molar mass is 26 g/mol, so the number of moles of solute is moles = mass / molar mass = 56 g / 26 g/mol ≈ 2.1538 mol.

Next, the solution volume is 959 mL, which in liters is 0.959 L. Molarity is defined as moles per liter, so M = 2.1538 mol / 0.959 L ≈ 2.2456 M.

Now we compare this calculated value to the provided answer choices. 2.2456 M rounds to about 2.25 M when expressed with two decimal places, which is closest to 2.2 M in the options given. This demonstrates that the near value corresponds to the option around 2.2 M after rounding.

Evaluate the other choices to see why they are not correct:
- 1.5 M would require the ratio to be 1.5 M, which would imply a smaller amount of solute or a larger volume than given; the computed moles over the given volume do not yield 1.5 M.
- 2.1 M is close to the calculated 2.25 M but still underestimates the result by a noticeable margin given the precise calculation; the 2.2456 M value is better represented as 2.25 M, which aligns with rounding toward 2.2 M rather than 2.1 M.
- 0.0022 M is vastly too small by about three orders of magnitude, indicating a misplacement of decimal or a unit error rather than a rounded result from the correct calculation.

In summary, the computation gives a molarity around 2.25 M, and among the provided options, the one closest after proper rounding is the 2.2 M choice.

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

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