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?
moles = g/molar mass.
There is 1 mole Ca^+2 in 1 mole CaCO3.
To calculate the moles of calcium carbonate that have dissolved in water, we need to use the molar mass of calcium carbonate (CaCO3), which is 100.09 g/mol.
First, we convert the given mass of calcium carbonate (0.02 g) to moles by using the formula:
moles = mass / molar mass
moles of CaCO3 = 0.02 g / 100.09 g/mol = 0.0002 mol
Therefore, 0.0002 moles of calcium carbonate have dissolved in the water.
Since there is only one calcium ion (Ca2+) in one formula unit of calcium carbonate, the number of moles of Ca2+ ions in solution will be the same as the moles of calcium carbonate, which is 0.0002 mol.
To calculate the number of Ca2+ ions in solution, we need to consider the stoichiometry of calcium carbonate. In one formula unit of calcium carbonate, there is one Ca2+ ion.
So, the number of Ca2+ ions in solution will be equal to the moles of Ca2+ ions, which is 0.0002 mol.
Keep in mind that this calculation assumes 100% dissociation of calcium carbonate in water. In reality, not all of the calcium carbonate may dissociate into Ca2+ ions.