Pre-IB Chemistry Mole Review Problems

Explanation
The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters. In this case, we need to first calculate the number of moles of barium chloride. The molar mass of barium chloride (BaCl2) is 137.33 g/mol. Therefore, 23.1 g of barium chloride is equal to 0.168 moles (23.1 g / 137.33 g/mol). The volume of the solution is given as 1000 mL, which is equal to 1 liter. Dividing the number of moles by the volume of the solution, we get a molarity of 0.168 M, which is approximately equal to 0.111 M.

Explanation
The given answer is correct because it represents the conversion of the given number of molecules of carbon dioxide to moles. The prefix "mol" is used to denote moles, so all three options (.143 mol, 0.143 mol, 0.143 moles) are equivalent and represent the same amount.

Explanation
In order to determine the number of chloride ions dissolved in the solution, we need to use the concept of molarity. Molarity is defined as the number of moles of solute per liter of solution. First, we need to calculate the number of moles of aluminum chloride in the solution by multiplying the volume (45.0 mL) by the molarity (0.800 M), and then dividing by 1000 to convert mL to L. Next, since aluminum chloride has a 1:3 ratio of aluminum ions to chloride ions, we multiply the number of moles of aluminum chloride by 3 to get the number of moles of chloride ions. Finally, we can convert the moles of chloride ions to ions by multiplying by Avogadro's number (6.022 x 10^23). The result is 6.50 x 10^22 ions.

Explanation
To find the number of molecules, we can use Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 particles (atoms, molecules, ions, etc.). In this case, we have 0.0174 moles of Cl2. So, to find the number of molecules, we can multiply 0.0174 moles by Avogadro's number (6.022 x 10^23 molecules/mole). The result is approximately 1.05 x 10^22 molecules.