a solution of h2so4 (aq) with a molal concentration of 6.25 m has a density of 1.3 g/mL. what is the molar concentration of this solution?
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To calculate the molar concentration of a solution, we need to convert the molal concentration to molar concentration.
Step 1: Convert the molal concentration to molality (m).
Molal concentration (m) is defined as moles of solute per kilogram of solvent.
Given that the molal concentration is 6.25 m, we can write:
6.25 m = 6.25 moles of solute / 1 kg of solvent
Step 2: Calculate the moles of solute.
To find the moles of solute, we need to know the mass of the solvent. Density can be used to calculate the mass.
Density = mass / volume
Density = 1.3 g/mL
Since the density is in mL, we need to convert it to kg. We know that 1 mL = 1 gram (ignoring the density of water since it is close to 1 g/mL and negligible in this case).
1.3 g/mL = 1.3 kg/L
Now, divide the density by the volume to find the mass:
1.3 kg/L / 1000 L = 0.0013 kg
Step 3: Calculate the molar concentration using the moles of solute and the mass of the solvent.
Molar concentration (c) is defined as moles of solute per liter of solution.
We know the molal concentration (6.25 m) and the mass of the solvent (0.0013 kg).
c = (m * molar mass of solute) / (mass of solvent)
Since H2SO4 is the solute, the molar mass of H2SO4 = 2*1 + 32 + 4*16 = 98 g/mol.
c = (6.25 * 98) / 0.0013
c = 4723.07 mol/L
Therefore, the molar concentration of the H2SO4 solution is approximately 4723.07 mol/L.
To find the molar concentration of a solution, we need to know the density and molal concentration of the solution. The molar concentration, also known as molarity, is expressed in moles of solute per liter of solution (mol/L).
Given:
Molal concentration (m) = 6.25 m (6.25 mol/kg or 6.25 moles of solute per kilogram of solvent)
Density = 1.3 g/mL
To find the molar concentration, we need to convert the given units to the appropriate ones. Let's start by converting the given density to kg/L.
1 mL of solution = 1 cm³ of solution (since 1 mL = 1 cm³)
1 g/mL = 1 g/cm³ (since density is equal to mass/volume)
Now, we can convert to kg/L:
1 g/cm³ = 1 kg/L
So, the density of the solution is also 1.3 kg/L.
Next, we need to consider the molecular weight of sulfuric acid (H₂SO₄), which is given by:
H₂ = 2 * atomic weight of hydrogen (1.008g/mol)
S = atomic weight of sulfur (32.06 g/mol)
O₄ = 4 * atomic weight of oxygen (16.00 g/mol)
Hence, the molecular weight of H₂SO₄ is:
2 * 1.008 g/mol + 32.06 g/mol + 4 * 16.00 g/mol = 98.09 g/mol
Now, we can use the formula to find the molar concentration (M):
M = (molal concentration * density) / molecular weight
M = (6.25 mol/kg * 1.3 kg/L) / 98.09 g/mol
First, we calculate the numerator:
6.25 mol/kg * 1.3 kg/L = 8.125 mol/L
Then, divide the numerator by the molecular weight:
8.125 mol/L / 98.09 g/mol
Calculating this expression, we find that the molar concentration of the solution is approximately 0.083 mol/L (rounded to three decimal places).
Therefore, the molar concentration of the solution is 0.083 mol/L.
6.25 m is 6.25 mol/kg solvent
6.25 mol H2SO4 = 6.25 x molar mass H2SO4 = about 610g but you need to do it more accurately.
So we have 610/(610g + 1000g)soln or
610/1610 g soln.
That 6.25 mol/1610 g soln. Use density to convert 1610g to L, then M = mols/L