I need to figure out the molarity in the problem.
A) 3.60g of sulfuric acid in 450.0mL of solution
I was going to take 3.60 / 450.0mL = 0.008
B) 2.0 x 10-3 mol Iron(II)nitrate in 12.0mL of Solution
10 *3=30 then I was going to take 30*2.0 =60
60/12.0= 5
I am not sure if this is correct.
A). M = mols/L. You took g/L.
Convert 3.60 g H2SO4 to mols. mol = grams/molar mass; then mols/L solution.
B)
I believe you are over thinking these problems. Just remember the definition. molarity = M = mols/L You have mols in B already. You have volume in mL, convert to L, then substitute into mols/L = M.
To determine the molarity in these problems, you need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
Let's calculate the molarity for each problem step-by-step:
A) 3.60g of sulfuric acid in 450.0mL of solution
1. Convert the mass of sulfuric acid to moles:
To do this, use the molar mass of sulfuric acid (H2SO4). It consists of two hydrogen (H) atoms, one sulfur (S) atom, and four oxygen (O) atoms.
The molar mass of H2SO4 = (2 * atomic mass of H) + atomic mass of S + (4 * atomic mass of O)
You can find the atomic masses on the periodic table.
2. Calculate moles of H2SO4:
moles = mass / molar mass
moles = 3.60g / molar mass of H2SO4
3. Convert mL to liters:
volume of solution in liters = 450.0mL / 1000
4. Calculate molarity:
Molarity (M) = moles / volume of solution in liters
B) 2.0 x 10-3 mol Iron(II)nitrate in 12.0mL of Solution
1. Convert mL to liters:
volume of solution in liters = 12.0mL / 1000
2. Calculate molarity:
Molarity (M) = moles / volume of solution in liters
Let's calculate the molarity for each problem more accurately. Please provide the molar masses of sulfuric acid and Iron(II)nitrate.
To determine the molarity of a solution, you need to divide the number of moles of solute by the volume of the solution in liters. Let's go through your calculations for both problems:
A) 3.60g of sulfuric acid in 450.0mL of solution
First, you need to convert the mass of sulfuric acid to moles. To do this, divide the mass by the molar mass of sulfuric acid (H2SO4), which is approximately 98.09 g/mol.
moles of H2SO4 = 3.60g / 98.09 g/mol ≈ 0.0367 mol
Next, convert the volume of the solution to liters by dividing it by 1000:
volume of solution = 450.0 mL / 1000 = 0.450 L
Now, divide the moles of H2SO4 by the volume in liters to find the molarity:
molarity = 0.0367 mol / 0.450 L ≈ 0.0813 M
So, the molarity of the solution is approximately 0.0813 M.
B) 2.0 x 10^-3 mol of Iron(II)nitrate in 12.0 mL of solution
First, there is no need to multiply anything by 10 or 3 in this case.
Next, convert the volume of the solution to liters by dividing it by 1000:
volume of solution = 12.0 mL / 1000 = 0.012 L
Now, divide the moles of Iron(II)nitrate by the volume in liters to find the molarity:
molarity = (2.0 x 10^-3) mol / 0.012 L ≈ 0.167 M
So, the molarity of the solution is approximately 0.167 M.
In summary, both of your calculations for the molarity are incorrect. Remember to convert grams to moles by dividing by the molar mass, and convert milliliters to liters by dividing by 1000 when calculating molarity.