Calcium carbonate is insoluble in water.if you have 40g of it; how many Ca^2+ and CO3^2- ions are present in it ?

To determine the number of Ca^2+ and CO3^2- ions present in 40g of calcium carbonate (CaCO3), we first need to calculate the molar mass of CaCO3.

The molar mass of CaCO3 is:
Ca: 40.08 g/mol
C: 12.01 g/mol
O: 16.00 g/mol

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

Now, we can calculate the number of moles of CaCO3 in 40g:
Number of moles = Mass / Molar mass
Number of moles = 40g / 100.09 g/mol = 0.3996 mol

Since the formula of calcium carbonate is CaCO3, there is 1 Ca^2+ ion and 1 CO3^2- ion in each molecule of CaCO3. Therefore, the number of Ca^2+ ions and CO3^2- ions present in 40g of calcium carbonate is equal to the number of moles of CaCO3.

Therefore, in 40g of calcium carbonate, there are:
- 0.3996 moles of Ca^2+ ions
- 0.3996 moles of CO3^2- ions

To find the number of ions, we can use Avogadro's number:
1 mole of any substance contains 6.022 x 10^23 particles (Avogadro's number)

Therefore, in 40g of calcium carbonate, there are:
- 0.3996 x 6.022 x 10^23 Ca^2+ ions
- 0.3996 x 6.022 x 10^23 CO3^2- ions

Calculating these values will give you the exact number of Ca^2+ and CO3^2- ions present in 40g of calcium carbonate.

Step 1: Determine the molar mass of calcium carbonate (CaCO3)

- CaCO3 = 40.08 (Ca) + 12.01 (C) + 48.00 (O) = 100.09 g/mol

Step 2: Calculate the number of moles of CaCO3

- 40 g / 100.09 g/mol = 0.4 moles of CaCO3

Step 3: Determine the stoichiometry of CaCO3

- CaCO3 contains one Ca2+ ion and one CO32- ion.

Step 4: Calculate the number of Ca2+ and CO32- ions

- 0.4 moles of CaCO3 x (1 mole of Ca2+ / 1 mole of CaCO3) = 0.4 moles of Ca2+ ions
- 0.4 moles of CaCO3 x (1 mole of CO32- / 1 mole of CaCO3) = 0.4 moles of CO32- ions

Therefore, there are 0.4 moles of Ca2+ ions and 0.4 moles of CO32- ions present in 40 g of calcium carbonate.