what mass of NaOH would be dissolved in 1dm3 of water to obtain 0.5 moles of the NaOH solution
a solution which contians one mole of the mass of; the compound in one dm3 of the solution is called what?
a solution which contains one mole of a solute dissolved in one liter is a one Molar solution.
For you first question, dissolve 1/2 mole into the solvent. That, as I recall is about 20grams of NaOH. Check it.
To determine the mass of NaOH needed to dissolve in 1 dm^3 of water to obtain 0.5 moles of NaOH:
Step 1: Find the molar mass of NaOH.
The molar mass of NaOH is calculated by summing up the atomic masses of its atoms. In this case:
Na (sodium) = 22.99 g/mol
O (oxygen) = 16.00 g/mol
H (hydrogen) = 1.01 g/mol
Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
Step 2: Calculate the mass of NaOH needed.
The given quantity is 0.5 moles. The molar mass of NaOH is 40.00 g/mol.
Using the formula:
Mass = Moles * Molar mass
Mass of NaOH = 0.5 moles * 40.00 g/mol = 20.00 g
Therefore, to obtain 0.5 moles of the NaOH solution in 1 dm^3 of water, you would need to dissolve 20.00 grams of NaOH in the water.
To determine the mass of NaOH that would be dissolved in 1dm^3 (or 1 liter) of water to obtain 0.5 moles of the NaOH solution, we'll need to use the molar mass and the formula:
1. Find the molar mass of NaOH:
- Sodium (Na) has an atomic mass of 22.99 g/mol.
- Oxygen (O) has an atomic mass of 16.00 g/mol.
- Hydrogen (H) has an atomic mass of 1.01 g/mol.
By adding up the atomic masses, we find:
Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol.
2. Use the molar mass to calculate the mass of NaOH:
- Molar mass = mass (g) / moles.
- Rearranging the formula:
- mass (g) = Molar mass × moles.
- Plugging in the given values:
- mass (g) = 40.00 g/mol × 0.5 mol = 20.00 g.
Therefore, to obtain 0.5 moles of a NaOH solution, you would need to dissolve 20.00 grams of NaOH in 1 dm^3 of water.