Determine the number of sodium ions contained in 25cm^3 of 0.5M sodium carbonate solution.
Just like the one I just did
25 cm^3 ( 1 liter / 1000 cm^3) = 0.025 liters
0. 5 mols/liter * 0.025liters = 0.0125 moles
2 Na ions / Na2CO3 molecule
2 (Avagadro's number) * 0.0125
To determine the number of sodium ions in the given solution, we need to know the concentration of sodium carbonate in moles and then consider the stoichiometry of sodium carbonate.
Here's how you can calculate it:
1. Begin by calculating the number of moles of sodium carbonate in the solution. The formula for calculating moles is:
Moles = Concentration (M) x Volume (L)
Given that the concentration is 0.5M and the volume is 25cm^3, we need to convert the volume to liters:
Volume (L) = 25 cm^3 / 1000 cm^3/L = 0.025 L
Now, we can calculate the moles of sodium carbonate:
Moles = 0.5M x 0.025 L
2. Next, consider the stoichiometry of sodium carbonate (Na2CO3). From the formula, we know that one mole of sodium carbonate contains two moles of sodium ions (Na+).
Therefore, the number of moles of sodium ions is:
Moles of Sodium Ions = 2 x Moles of Sodium Carbonate
3. Finally, we need to convert the moles of sodium ions to the number of sodium ions. Since one mole of any substance contains Avogadro's number (6.022 x 10^23) entities, we can use this conversion factor:
Number of Sodium Ions = Moles of Sodium Ions x Avogadro's Number
Now, let's calculate the number of sodium ions:
1. Moles of Sodium Carbonate = 0.5M x 0.025 L = 0.0125 moles
2. Moles of Sodium Ions = 2 x 0.0125 moles = 0.025 moles
3. Number of Sodium Ions = 0.025 moles x 6.022 x 10^23 ions/mole
By plugging in the values, we can calculate the number of sodium ions contained in 25cm^3 of 0.5M sodium carbonate solution.