A student dissolved 3.65 g of hydrogen chloride gas,HCL in water to make 1.0dm^3 of solution.Calculate the volume of a 0.1 mol dm^-3 barium hydroxide,Ba(OH)2 solution required to completely neutralise 25.0 cm^3 of the acid solution.(RAM:H,1;CL,35.5)

This is done by the same procedure as the NaOH/H3PO4 problem above.

To start this problem, we need to calculate the number of moles of hydrogen chloride (HCl) in the given mass. We can use the formula:

moles = mass / molar mass

The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl):

molar mass of HCl = atomic mass of H + atomic mass of Cl

= 1 + 35.5

= 36.5 g/mol

Now, we can calculate the number of moles of HCl using the given mass:

moles of HCl = 3.65 g / 36.5 g/mol

= 0.1 mol

We are also given the concentration of the barium hydroxide (Ba(OH)2) solution as 0.1 mol dm^-3, which means that there are 0.1 moles of Ba(OH)2 in one liter (1000 cm^3) of the solution.

Now, we can calculate the volume of Ba(OH)2 solution required to neutralize 0.1 moles of HCl.

First, we need to find the number of moles of HCl neutralized by 25.0 cm^3 of the acid solution (HCl).

moles of HCl neutralized = (moles of HCl / volume of HCl solution) x volume of HCl neutralized

volume of HCl neutralized = 0.1 moles / (25.0 cm^3 / 1000 cm^3/dm3)

= 4.0 cm^3

The volume of a 0.1 mol dm^-3 Ba(OH)2 solution required to completely neutralize 25.0 cm^3 of the acid solution is 4.0 cm^3.