What mass of water must be used to make a 1.35m solution that contains 8.20 moles NaOH?
1.35=8.2/kgwater
6.07
To determine the mass of water needed to make a 1.35M solution containing 8.20 moles of NaOH, we can use the formula:
Molarity (M) = Moles of solute / Volume of solution (in liters)
To find the volume of the solution, we rearrange the formula:
Volume of solution (in liters) = Moles of solute / Molarity
Given:
Moles of NaOH = 8.20 moles
Molarity (M) = 1.35 M
Let's substitute these values into the formula to find the volume of the solution:
Volume of solution = 8.20 moles / 1.35 M
Volume of solution ≈ 6.07 liters
Since we want to find the mass of water, we need to subtract the volume of NaOH solution from the total volume:
Volume of water = Total volume - Volume of NaOH solution
Volume of water ≈ 6.07 liters - 6.07 liters
Volume of water ≈ 0 liters
Therefore, no water is needed to make a 1.35M solution containing 8.20 moles of NaOH.
To determine the mass of water needed to make a 1.35m solution containing 8.20 moles of NaOH, you need to use the formula for molarity:
Molarity (M) = Moles of solute / Volume of solution (in liters)
Given:
Molarity (M) = 1.35 M
Moles of NaOH = 8.20 mol
First, rearrange the formula to solve for the volume of the solution:
Volume of solution (in liters) = Moles of solute / Molarity
Substitute the given values into the equation:
Volume of solution (in liters) = 8.20 mol / 1.35 M
Now, you need to convert this volume to mass of water. Since water has a density of 1 g/mL, you can assume that 1 liter of water has a mass of 1000 grams:
Mass of water = Volume of solution (in liters) x Density of water
Substitute the calculated volume of solution into the equation:
Mass of water = (8.20 mol / 1.35 M) x 1000 g/L
Now, perform the calculation:
Mass of water = 6074.07 g
Therefore, you would need approximately 6074.07 grams of water to make a 1.35m solution containing 8.20 moles of NaOH.