0.02 g of CaCO3 is dissolved in 1 L of water. Calculate the moles of calcium carbonate that have dissolved in the water, the moles of Ca2+ ions in solution, and the number of Ca2+ ions in solution?

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To calculate the moles of calcium carbonate (CaCO3) dissolved in water, we need to use its molar mass and the given mass.

Step 1: Calculate the molar mass of CaCO3:
Ca: 40.08 g/mol
C: 12.01 g/mol
O: 16.00 g/mol (3 atoms)

Molar mass of CaCO3 = (40.08 g/mol) + (12.01 g/mol) + (16.00 g/mol × 3) = 100.09 g/mol

Step 2: Convert the given mass to moles:
Given mass = 0.02 g
Moles of CaCO3 = (Given mass of CaCO3 / Molar mass of CaCO3)

Moles of CaCO3 = (0.02 g) / (100.09 g/mol) = 0.000199 moles

Therefore, the moles of calcium carbonate (CaCO3) dissolved in water are approximately 0.000199 moles.

Next, let's calculate the number of moles of Ca2+ ions in solution. Since every mole of CaCO3 produces one mole of Ca2+ ions, the moles of Ca2+ ions will be the same as the moles of CaCO3.

Therefore, the moles of Ca2+ ions in solution are also approximately 0.000199 moles.

Finally, let's calculate the number of Ca2+ ions in solution. Since each mole of Ca2+ ions contains one mole of Ca2+ ions, the number of Ca2+ ions will be equal to the number of moles of Ca2+ ions.

Number of Ca2+ ions in solution = 0.000199 moles

So, approximately 0.000199 moles of CaCO3 and Ca2+ ions have dissolved in the water, and the number of Ca2+ ions in solution is also approximately 0.000199 moles.