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What do the following solutions have in common: a) 100 cm³ of 1 M solution b) 10 cm³ of 10 M solution c) 50 cm³ of 2 M solution?

Chemistry

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Answer

c

0.1 mol of solute\text{0.1 mol of solute}

Step-by-step solution

6 steps

To find what these solutions have in common, we will calculate the number of moles of solute in each solution. The formula for the number of moles is:

Moles=Molarity×Volume (in dm3)\text{Moles} = \text{Molarity} \times \text{Volume (in dm}^3\text{)}

We need to convert the given volumes from cm3\text{cm}^3 to dm3\text{dm}^3 by dividing by 1000.

Part a· 2 steps

For 100 cm3100 \text{ cm}^3 of a 1 M1\text{ M} solution

  1. Convert volume to dm3\text{dm}^3.

    100 cm3=1001000 dm3=0.1 dm3100 \text{ cm}^3 = \frac{100}{1000} \text{ dm}^3 = 0.1 \text{ dm}^3

  2. Calculate the number of moles.

    Moles=1 M×0.1 dm3=0.1 mol\text{Moles} = 1\text{ M} \times 0.1 \text{ dm}^3 = 0.1 \text{ mol}

Part b· 2 steps

For 10 cm310 \text{ cm}^3 of a 10 M10\text{ M} solution

  1. Convert volume to dm3\text{dm}^3.

    10 cm3=101000 dm3=0.01 dm310 \text{ cm}^3 = \frac{10}{1000} \text{ dm}^3 = 0.01 \text{ dm}^3

  2. Calculate the number of moles.

    Moles=10 M×0.01 dm3=0.1 mol\text{Moles} = 10\text{ M} \times 0.01 \text{ dm}^3 = 0.1 \text{ mol}

Part c

0.1 mol of solute\text{0.1 mol of solute}

For 50 cm350 \text{ cm}^3 of a 2 M2\text{ M} solution

  1. Convert volume to dm3\text{dm}^3.

    50 cm3=501000 dm3=0.05 dm350 \text{ cm}^3 = \frac{50}{1000} \text{ dm}^3 = 0.05 \text{ dm}^3

  2. Calculate the number of moles.

    Moles=2 M×0.05 dm3=0.1 mol\text{Moles} = 2\text{ M} \times 0.05 \text{ dm}^3 = 0.1 \text{ mol}

    All three solutions contain the same number of moles of solute.

    The commonality is that they all contain 0.1 mol of solute\boxed{\text{0.1 mol of solute}}.

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