First, let's define a base according to the Arrhenius theory: A base is a substance that, when dissolved in water, increases the hydroxide ion (OH-) concentration in the solution.
Now, let's calculate the number of moles of hydroxide ions (OH-) in beaker B:
Moles of OH- in beaker B = (Volume in beaker B) x (Concentration of KOH in beaker B)
Moles of OH- in beaker B = (400 cm³) x (0.1 mol/dm³)
Moles of OH- in beaker B = 40 mmol
7.3.1
To calculate the concentration, X, of the Ba(OH)2 in beaker A, we need more information. Specifically, we need to know the volume of the solution in beaker A. Once we have that, we can use the following formula:
Concentration of Ba(OH)2 in beaker A = (Moles of OH- in beaker A) / (Volume in beaker A)
7.3.2 and 7.3.3
The balanced equation for the reaction is:
CH3COOH(aq) + OH(aq) -> CH3COO(aq) + H2O(l)
7.3.4
Ethanoic acid, CH3COOH(aq), is a weak acid. This is because it only partially dissociates in water, meaning it does not completely donate a proton (H+) to the water molecule. Instead, it forms an equilibrium with the dissociated and non-dissociated forms. The reason for this behavior is the acid's structure and the strength of the bond between the hydrogen atom and the oxygen atom in the molecule.
7.3.5
To calculate the concentration of the ethanoic acid, we need to know the moles of ethanoic acid used in the titration and the total volume of the solution after adding the 15 cm³ of the solution from beaker C. Once we have that information, we can use the formula:
Concentration of CH3COOH = (Moles of CH3COOH) / (Total volume of the solution)
