What volume of a 0.550 M solution of potassium hydroxide can be made with 18.3 g of potassium hydroxide? (Ignore significant figures for this problem.)
To find the volume of a solution, we need to use the equation:
Molarity (M) = moles of solute / volume of solution (in liters)
We can rearrange this equation to solve for the volume:
Volume = moles of solute / Molarity
First, we need to calculate the moles of potassium hydroxide (KOH) using its molar mass:
Molar mass of KOH = 39.1 g/mol (for K) + 16.0 g/mol (for O) + 1.01 g/mol (for H) = 56.11 g/mol
Moles of KOH = mass of KOH / molar mass of KOH
= 18.3 g / 56.11 g/mol ≈ 0.326 mol
Next, we can substitute the values into the equation to find the volume of the solution:
Volume = moles of solute / Molarity
= 0.326 mol / 0.550 M
≈ 0.592 L
Therefore, the volume of a 0.550 M solution of potassium hydroxide that can be made with 18.3 g of potassium hydroxide is approximately 0.592 liters.
To determine the volume of a 0.550 M solution of potassium hydroxide that can be made with 18.3 g of potassium hydroxide, we need to use the formula:
moles = mass / molar mass
First, let's find the molar mass of potassium hydroxide (KOH).
K (potassium) has a molar mass of 39.10 g/mol.
O (oxygen) has a molar mass of 16.00 g/mol.
H (hydrogen) has a molar mass of 1.01 g/mol.
Now, sum up the molar masses to find the molar mass of KOH:
39.10 g/mol (K) + 16.00 g/mol (O) + 1.01 g/mol (H) = 56.11 g/mol (KOH)
Next, convert the mass of potassium hydroxide to moles using the formula:
moles = mass / molar mass
moles = 18.3 g / 56.11 g/mol ≈ 0.326 moles
Now, we can use the definition of molarity (M) to find the volume of the solution:
Molarity (M) = moles of solute / volume of solvent (in liters)
Rearranging the formula to solve for volume:
Volume = moles of solute / Molarity
Volume = 0.326 moles / 0.550 M ≈ 0.592 L
So, the volume of a 0.550 M solution of potassium hydroxide that can be made with 18.3 g of potassium hydroxide is approximately 0.592 liters (or 592 mL).
def
mols KOH = grams/molar mass =
18.3/approx 56 = approx 0.33 but you need a more accurate number.
Then M = mols/L solution. You know M and mols, solve for L.