The density of 95.2 % (weight percent) of H2SO4 is 1.53 g/ml.calculate the molarity of this solution.
molarity= moles/literSolution
So in 1000ml (onr liter) of solution , the mass is 1530grams, of that 95.2percetn is H2SO4, or
Molarity= (1530*0.952)/98*1liter= 14.9M moles/liter
Well, isn't this a fun chemistry question!
To find the molarity of the solution, we need to first calculate the number of moles of H2SO4 present in 1 liter (1000 ml) of the solution.
So, let's start with the density of the solution, which is 1.53 g/ml. This means that if we had 1 liter of the solution, it would weigh 1.53 kg, or 1530 grams.
Now, the question tells us that the solution is 95.2% (weight percent) H2SO4. To find the amount of H2SO4 in grams, we multiply the total weight of the solution by the weight percent:
(1530 grams) * (95.2%) = 1458.96 grams
Next, we need to determine the molar mass of H2SO4. H2SO4 is made up of 2 hydrogen atoms (H), 1 sulfur atom (S), and 4 oxygen atoms (O). The molar masses of these elements are approximately:
H = 1 g/mol
S = 32 g/mol
O = 16 g/mol
So, the molar mass of H2SO4 is:
(2 * 1 g/mol) + (1 * 32 g/mol) + (4 * 16 g/mol) = 98 g/mol
Now we can calculate the number of moles of H2SO4 in the solution by dividing the grams of H2SO4 by its molar mass:
(1458.96 grams) / (98 g/mol) = 14.89 moles
Finally, to find the molarity, we divide the number of moles of H2SO4 by the volume of the solution in liters. Since there are 1000 ml in 1 liter, the volume of the solution is 1 liter:
14.89 moles / 1 liter = 14.89 M
So, the molarity of this H2SO4 solution is approximately 14.89 M. Now, that's a lot of moles swimming around in there!
To calculate the molarity of a solution, we need to know the density of the solute and its molar mass.
First, let's determine the molar mass of H2SO4 (sulfuric acid):
The molar mass of hydrogen (H) is approximately 1 g/mol.
The molar mass of sulfur (S) is approximately 32 g/mol.
The molar mass of oxygen (O) is approximately 16 g/mol.
Hence, the molar mass of H2SO4 is:
2(1 g/mol) + 32 g/mol + 4(16 g/mol) = 98 g/mol
Now, we can calculate the molarity using the given density (1.53 g/ml):
Molarity (M) is defined as the number of moles of solute per liter of solution.
First, we need to convert the given density into g/L:
1.53 g/ml * (1000 ml/1 L) = 1530 g/L
Next, we can calculate the molarity using the formula:
Molarity (M) = (weight percent * density) / (molar mass * 10)
Molarity (M) = (95.2% * 1530 g/L) / (98 g/mol * 10)
Molarity (M) = (0.952 * 1530) / (980)
Molarity (M) = 1.487 M (rounded to three significant figures)
Therefore, the molarity of the solution is 1.487 M.
To calculate the molarity (M) of a solution, you need to know the molecular weight (MW) of the solute and the volume of the solution.
In this case, the solute is H2SO4, which has a molecular weight of:
MW(H2SO4) = (2 x MW(Hydrogen)) + MW(Sulfur) + (4 x MW(Oxygen))
= (2 x 1) + 32 + (4 x 16)
= 2 + 32 + 64
= 98 g/mol
The density of the solution is given as 1.53 g/mL. This means that 1 mL of the solution has a mass of 1.53 g.
To calculate the molarity, you need to convert the density to grams per liter (g/L). Since there are 1000 mL in a liter, the density in g/L is:
Density = 1.53 g/mL
= 1.53 g / 1 mL
= 1.53 g / (1 mL / 1000 mL/L)
= 1.53 g / 0.001 L
= 1530 g/L
Now, you can use the formula for molarity:
Molarity (M) = (Mass of solute in grams) / (Molecular weight of solute in g/mol) / (Volume of solution in L)
In this case, the mass of the solute is obtained by multiplying the density by the weight percent of the solute:
Mass of H2SO4 = (Density of solution) x (Weight percent of H2SO4 / 100)
= 1.53 g/mL x (95.2 / 100)
= 1.53 g/mL x 0.952
= 1.458 g
Now, you can substitute the values into the molarity formula:
Molarity (M) = (1.458 g) / (98 g/mol) / (1 L)
Calculating this, you will get:
Molarity (M) ≈ 0.0148 mol/L
Therefore, the molarity of the solution is approximately 0.0148 M.