An aqueous stock solution is 85.0% H2SO4 by mass and its density is 1.83 g/mL. What volume of this solution is required to make 1.00 L of 1.35 mol/L H2SO4(aq)? Give your answer in millilitres, accurate to three significant figures.
Well, that's quite a mouthful! Let's break it down and see if we can make it more fun.
First, we need to figure out the mass of the aqueous stock solution that we need. We know it's 85.0% H2SO4 by mass, but we also know the density is 1.83 g/mL. So, we can think of it as a really dense liquid. Maybe it's been hitting the gym and lifting weights!
Now, we want to make 1.00 L of a 1.35 mol/L H2SO4(aq) solution. It's like mixing up a fancy chemistry cocktail! But instead of shaking it, we're going to calculate the volume.
To find the volume, we need to calculate the mass of the H2SO4 we want in the final solution. We know that the molar mass of H2SO4 is approximately 98.09 g/mol. So, 1.35 mol/L times 98.09 g/mol gives us the mass of H2SO4 we need.
Now, we can divide this mass by the density of the stock solution to find the volume. Do a little math dance, and voila! You should end up with your answer in millilitres, accurate to three significant figures.
I hope that made it a little more entertaining for you!
To determine the volume of the stock solution required to make 1.00 L of 1.35 mol/L H2SO4(aq), we can use the following steps:
Step 1: Determine the molar mass of H2SO4.
The molar mass of H2SO4 is calculated by adding up the atomic masses of its elements:
2(atomic mass of hydrogen) + atomic mass of sulfur + 4(atomic mass of oxygen)
= 2(1.00784 g/mol) + 32.06 g/mol + 4(15.999 g/mol)
= 98.09 g/mol
Step 2: Calculate the amount of H2SO4 needed in grams.
To find the amount of H2SO4 needed, we multiply the desired concentration (1.35 mol/L) by the desired volume (1.00 L) and the molar mass of H2SO4:
1.35 mol/L x 1.00 L x 98.09 g/mol = 132.32 g
Step 3: Determine the volume of the stock solution needed.
To find the volume of the stock solution needed, we will divide the mass of H2SO4 by the density of the stock solution:
132.32 g ÷ (1.83 g/mL) = 72.32 mL
Therefore, 72.32 millilitres (mL), accurate to three significant figures, of the stock solution is required to make 1.00 L of 1.35 mol/L H2SO4(aq).
To find the volume of the 85.0% H2SO4 stock solution needed to make 1.00 L of a 1.35 mol/L H2SO4 solution, we can use the equation:
(mass/volume) × volume = mass
First, we need to find the mass of H2SO4 needed to make 1.00 L of a 1.35 mol/L solution. The molar mass of H2SO4 is:
(2 × atomic mass of H) + atomic mass of S + (4 × atomic mass of O) = (2 × 1.01 g/mol) + 32.07 g/mol + (4 × 16.00 g/mol) = 98.09 g/mol
So the mass of H2SO4 needed for a 1.00 L solution is:
mass = concentration × volume
mass = (1.35 mol/L) × (1.00 L) × (98.09 g/mol) = 132.4135 g
Now, we can calculate the volume of the stock solution needed using the equation:
(mass/volume) × volume = mass
Let's assume the volume of the stock solution needed is V mL.
(0.85 × 1.83 g/mL) × V mL = 132.4135 g
0.85 × 1.83 × V = 132.4135
V = 132.4135 / (0.85 × 1.83)
V ≈ 96.47 mL
Therefore, approximately 96.47 mL of the 85.0% H2SO4 stock solution is required to make 1.00 L of a 1.35 mol/L H2SO4(aq) solution.
What's the molarity of the H2SO4 you have?
That's 1.83 g/mL x 1000 mL x 0.85 x (1 mol/98g) = approx 16 M but you need a more accurate answer.
Then c1v1 = c2v2
16M*v = 1.35M x 1000mL
Solve for v in mL but remember to get a better answer for that 16M.