Christina G.

# what is the total concentration of all ions in a solution formed by dissolving 1.50 g Al2(SO4)3 in 100.0 ml of solution?

what is the total concentration of all ions in a solution formed by dissolving 1.50 g Al2(SO4)3 in 100.0 ml of solution?

Haroon I.

To determine the total concentration of all ions in a solution formed by dissolving 1.50 g of Al2(SO4)3 in 100.0 ml of solution, we need to calculate the moles of Al2(SO4)3 and then determine the concentration of each ion. 1. Calculate the moles of Al2(SO4)3: The molar mass of Al2(SO4)3 is: 2(Al) + 3(S) + 12(O) = 2(26.98 g/mol) + 3(32.06 g/mol) + 12(16.00 g/mol) = 342.15 g/mol Moles of Al2(SO4)3 = Mass / Molar mass = 1.50 g / 342.15 g/mol 2. Calculate the concentration of each ion: Al2(SO4)3 dissociates into 2 Al3+ ions and 3 SO4^2- ions. Since 1 mole of Al2(SO4)3 gives 2 moles of Al3+ ions and 3 moles of SO4^2- ions, the moles of each ion are: Moles of Al3+ ions = 2 * (moles of Al2(SO4)3) Moles of SO4^2- ions = 3 * (moles of Al2(SO4)3) 3. Calculate the concentration (molarity) of each ion: The concentration of each ion is determined by dividing the moles of that ion by the volume of the solution in liters. Volume of solution = 100.0 ml = 100.0 ml * (1 L / 1000 ml) = 0.1000 L Concentration of Al3+ ions = Moles of Al3+ ions / Volume of solution Concentration of SO4^2- ions = Moles of SO4^2- ions / Volume of solution Now you can substitute the values you calculated in steps 1 and 3 to find the concentrations of the Al3+ and SO4^2- ions in the solution.
Report

8d

By:

Tutor
New to Wyzant

Expert chemistry tutoring with a wealth of experience

## Still looking for help? Get the right answer, fast.

Get a free answer to a quick problem.
Most questions answered within 4 hours.

#### OR

Choose an expert and meet online. No packages or subscriptions, pay only for the time you need.