Commerical hydrochloric acid is 37% by mass HCl and has a solution density of 1.18g/mL. What minimum volume of hydrocloric acid is needed to dissolve 16g Al. The balanced equation is
2Al + 6Hcl --> 2AlCl3 + 3H2
Use stoichiometry to determine the mols of HCl needed.
Probably the easiest thing to do next is to determine the molarity of the commerical HCl.
M = mols/L.
density = 1.18 g/mL; therefore,
mass of 1000 mL = 1.18 g/mL x 1000 mL = 1180 grams.
How much of that is HCl.
1180 g x 0.37 = 436.6 grams HCl.
How many mols. 436.6/36.46 = 11.97 so HCl is 11.97 Molar.
mols needed to dissolve Al = M x L
You know mols needed. You know M. Solve for Liters
Post your work if you needed additional help.
To calculate the minimum volume of hydrochloric acid needed to dissolve 16g of Al, we need to use stoichiometry and the given information. Here's how you can approach it step by step:
Step 1: Calculate the moles of Al
Use the molar mass of Al (which is 26.98 g/mol) to convert the given mass of Al (16g) into moles. Divide the mass by the molar mass to find the moles of Al:
16g Al × (1 mol Al/26.98g Al) = 0.593 mol Al
Step 2: Determine the stoichiometry between Al and HCl
From the balanced equation, we can see that 2 moles of Al react with 6 moles of HCl. Therefore, the mole ratio between Al and HCl is 2:6, which reduces to 1:3.
Step 3: Calculate the moles of HCl needed
Since the mole ratio between Al and HCl is 1:3, the moles of HCl needed can be found by multiplying the moles of Al by the ratio:
0.593 mol Al × (3 mol HCl/1 mol Al) = 1.779 mol HCl
Step 4: Calculate the mass of HCl needed
Using the mass percent and density of the hydrochloric acid solution, you can find the mass of HCl needed. The density of the solution is given as 1.18g/mL, which means 1 mL of the solution weighs 1.18g. Multiplying the density by the volume gives the mass.
Density = Mass / Volume => Mass = Density × Volume
We need to find the volume, so rearrange the formula: Volume = Mass / Density
The mass of HCl needed can be calculated using the following formula:
Mass HCl = (Mass HCl Solution) × (% HCl/100)
Let's assume the volume of the hydrochloric acid solution required is V mL.
Now we have:
(Mass HCl Solution) = (Density of Solution) × (Volume of Solution)
(Mass HCl Solution) = 1.18g/mL × V mL
(Mass HCl) = (1.18g/mL × V mL) × (37/100)
(Mass HCl) = 0.4366 V g (after calculating)
Step 5: Set up an equation using the mole ratio and convert to volume
Since we know the molar mass of HCl (36.46 g/mol), we can convert the moles of HCl to grams using the following equation:
Mass HCl = (Moles HCl) × (Molar Mass HCl)
0.4366 V g = 1.779 mol HCl × 36.46 g/mol
Step 6: Solve for the volume of hydrochloric acid
Rearrange the equation to solve for V:
V = (1.779 mol HCl × 36.46 g/mol) / 0.4366 g
V ≈ 148.76 mL
Therefore, the minimum volume of hydrochloric acid solution needed to dissolve 16g of Al is approximately 148.76 mL.