If the density of pure acetic is 1.005g/cm3, what is it's molarity
I assume you mean acetic acid.
density = 1.005 g/cc
So that has a mass of 1.005 x 1000 cc = 1005 g pure acetic acid/L
molarity = M = mols/L. 1005 g x (1 mol/60 g) = ? mols/L = ?M
Well, since you're talking about density and molarity, I just have to say - this is going to be a "concentrated" answer!
To find the molarity of a substance, we need to know the molar mass, which is the amount of grams in one mole. For acetic acid (CH3COOH), the molar mass is about 60.052 g/mol.
Now, if the density of pure acetic acid is 1.005 g/cm3, we can use this information to calculate its molarity. But before we do that, let me just ask - why did the acetic acid go to therapy? Because it had too many "dissociative" tendencies!
To calculate the molarity, we need to convert the density to grams per liter (g/L). Since there are 1000 cm3 in 1 L, we can say that the density of acetic acid is 1.005 g/cm3 * 1000 cm3/L = 1005 g/L.
Next, we use the equation: Molarity (M) = (mass of solute in grams) / (volume of solution in liters). In this case, the mass of the solute is 1005 g and since we don't have the volume of the solution, we can't calculate the molarity.
So, unfortunately, without the volume of the acetic acid solution, we can't give you a precise molarity. Just like a clown without his red nose, we are left without the key information to complete the calculation.
To determine the molarity of a substance, we need to know its molecular weight. The molecular weight of acetic acid (CH3COOH) is 60.052 g/mol.
Given that the density of pure acetic acid is 1.005 g/cm3, we can use the following relationship:
Density = mass/volume
To calculate the volume (V) of acetic acid:
V = mass/density
Since the units of density are grams per cubic centimeter (g/cm3) and we need the mass in grams (g), we can use the following relationship to convert volume to liters:
1 cm3 = 1 mL = 0.001 L
Now, let's calculate the volume (V) in liters:
V = (mass in grams) / (density in g/cm3)
V = 1 / 1.005 = 0.994 L
Next, we can use the molarity formula:
Molarity = moles / volume
Since we know the molecular weight of acetic acid and the volume in liters, we can calculate the moles of acetic acid using the formula:
moles = mass / molecular weight
The mass of acetic acid can be found by multiplying the density (1.005 g/cm3) by the volume (0.994 L):
mass = density x volume = 1.005 g/cm3 x 0.994 L = 0.9989 g
Now, let's calculate the molarity:
moles = mass / molecular weight = 0.9989 g / 60.052 g/mol = 0.0166 mol
Molarity = moles / volume = 0.0166 mol / 0.994 L = 0.0167 M
Therefore, the molarity of pure acetic acid is approximately 0.0167 M.
To find the molarity of a solution, we need to know the molar mass of the solute and the volume of the solution. In this case, we have the density of pure acetic acid (CH3COOH), which is 1.005 g/cm3.
To find the molar mass of acetic acid, we can look up its atomic masses and calculate it. The molar mass of carbon (C) is 12.01 g/mol, the molar mass of hydrogen (H) is 1.008 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol.
Since there are two hydrogens and two oxygens in acetic acid, the molar mass of acetic acid can be calculated as follows:
(2 × molar mass of H) + molar mass of C + (2 × molar mass of O)
= (2 × 1.008 g/mol) + 12.01 g/mol + (2 × 16.00 g/mol)
= 2.016 g/mol + 12.01 g/mol + 32.00 g/mol
= 46.026 g/mol
Now that we have the molar mass of acetic acid, we can calculate its molarity using the equation:
Molarity (M) = (mass of solute in grams) / (molar mass of solute in g/mol) / (volume of solution in liters)
However, we only have the density of acetic acid, not the volume. The density is given as 1.005 g/cm3, but we need to convert it to the volume in liters.
Density = mass / volume
=> volume = mass / density
=> volume = 1 g / 1.005 g/cm3
=> volume = 0.994 cm3
Now, we can convert the volume to liters:
volume = 0.994 cm3 × (1 mL/1 cm3) × (1 liter/1000 mL)
volume = 0.000994 L
Now that we have the volume in liters, we can calculate the molarity of acetic acid:
Molarity = (mass of solute in grams) / (molar mass of solute in g/mol) / (volume of solution in liters)
Molarity = 1 g / 46.026 g/mol / 0.000994 L
Molarity ≈ 21.288 M
So, the molarity of pure acetic acid is approximately 21.288 M.