What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?

Question

BlackTom AI · Accepted Answer

To determine molarity, we use the formula M = moles of solute / liters of solution.
First, convert the volume from milliliters to liters: 569 mL × (1 L / 1000 mL) = 0.569 L.
Next, plug in the values: M = 7.0 moles / 0.569 L ≈ 12.31 M.
Now evaluate each option:
Option 1: 81 M. This is far too high; it would require only about 0.086 L (or 86 mL) of solution to reach 7 moles, which contradicts the given 569 mL. The calculation clearly shows a much larger figure than 81 M.
Option 2: 0.081 M. This is off by roughly a factor of 150; the denominator would need to be around 86 L to yield such a small value with 7.0 moles, which is not consistent with 0.569 L.
Option 3: 12 M. This aligns with the calculated value when rounded to two significant figures (7.0 moles and 569 mL imply about 12 M). The slight difference between 12.31 M and 12 M is due to rounding.
Option 4: 4.0 M. This is not supported by the computation; achieving 4.0 M with 7.0 moles would require a volume of about 1.75 L, which contradicts the given 0.569 L.
In summary, the correct interpretation from the calculation is that the solution’s molarity is approximately 12 M, matching the option that reflects this rounded value.

What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?

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