# Convert 355mL of a solution containing 6.31 ppm CaCO3 to mmol?

So, we can convert the volume of the solution to a mass:

So, we currently have:

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Here's what I got.

Next, convert this to milligrams of solute per milligrams of solvent

To convert this to mmol per liter, calculate the number of mmoles of calcium carbonate you have in one liter of solution

The answers are rounded to three sig figs.

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To convert ppm to mmol, multiply the concentration in ppm by the molecular weight of the substance and then divide by 1000.

[ \text{mmol} = \left(\frac{\text{ppm} \times \text{volume in mL}}{1000}\right) \times \text{molecular weight} ]

For CaCO3 (calcium carbonate), the molecular weight is 100.09 g/mol.

[ \text{mmol} = \left(\frac{6.31 \times 355}{1000}\right) \times 100.09 ]

[ \text{mmol} \approx 2.24 , \text{mmol} ]

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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