Question

Find the volume of 0.120 M hydrochloric acid necessary to react completely with 1.55 g Al(OH)3.

Answer 1

Answer: The volume of HCl is 55.83 mL

Step-by-step explanation:

To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

Given mass of aluminium hydroxide = 1.55 g

Molar mass of aluminium hydroxide = 78 g/mol

Putting values in above equation, we get:

`\text{Moles of aluminium hydroxide}=(1.55g)/(78g/mol)=0.020mol`

The chemical reaction for the formation of chromium oxide follows the equation:

`Al(OH)_3+3HCl\rightarrow AlCl_3+6H_2O`

By Stoichiometry of the reaction:

1 mole of aluminium hydroxide reacts with 3 moles of HCl

So, 0.020 moles of aluminium hydroxide will react with =
`(1)/(3)* 0.020=0.0067mol` of HCl

To calculate the volume of HCl, we use the equation:

`\text{Molarity of the solution}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (in mL)}}`

We are given:

Moles of HCl = 0.0067 moles

Molarity of solution = 0.120 M

Putting values in above equation, we get:

`0.120=\frac{0.0024* 1000}{\text{Volume of HCl}}\\\\\text{Volume of HCl}=(0.0024* 1000)/(0.120)=55.83mL`

Hence, the volume of HCl is 55.83 mL

Answer 2

The balanced chemical reaction is expressed as:

3HCl + Al(OH)3 = AlCl3 + 3H2O

We are given the amount of aluminum hydroxide to be used up in the reaction. This value will be the starting point for the calculations. We calculate as follows:

1.55 g Al(OH)3 ( 1 mol Al(OH)3 / 78 g Al(OH)3 )( 3 mol HCl / 1 mol Al(OH)3 ) = 0.06 mol HCl

Volume = 0.06 mol HCl / 0.120 mol HCl/ L solution = 0.50 L solution