Final answer:
To provide 5.36 g of KOH using a 0.619 M KOH solution, one would need to calculate the moles of KOH required and then use the molarity to find the volume, which comes out to approximately 154 mL.
Step-by-step explanation:
To calculate how many milliliters of a 0.619 M KOH solution would be needed to provide 5.36 g of KOH, you first need to determine how many moles of KOH you have using its molar mass.
One mole of KOH has a molar mass of approximately 56.11 g/mol. Using the formula:
moles = mass (g) / molar mass (g/mol),
moles of KOH = 5.36 g / 56.11 g/mol = 0.0955 mol.
Now that we know the moles of KOH, we use the molarity (M) of the solution to find the volume:
Volume (L) = moles / molarity (mol/L),
Volume (L) = 0.0955 mol / 0.619 mol/L = 0.154 L,
which converts to milliliters (1 L = 1000 mL):
Volume (mL) = 0.154 L × 1000 mL/L = 154 mL.
Therefore, you would need approximately 154 mL of the 0.619 M KOH solution to provide 5.36 g of KOH for the chemical reaction.