Mass of "KHP" to neutralize 18 mL of 0.20 M NaOH?
To find the mass of potassium hydrogen phthalate (KHP) required to neutralize 18 mL of 0.20 M NaOH, you can use the concept of stoichiometry.
The balanced chemical equation for the reaction between KHP and NaOH is:
KHP + NaOH -> KNaP + H2O
From the balanced equation, we can see that the stoichiometric ratio of KHP to NaOH is 1:1. This means that 1 mole of KHP reacts with 1 mole of NaOH.
To calculate the mass of KHP, we need to determine the number of moles of NaOH in 18 mL of the solution.
First, convert the volume of the solution from milliliters (mL) to liters (L):
18 mL = 18/1000 L = 0.018 L
Next, calculate the number of moles of NaOH using the formula:
moles = volume (L) x concentration (M)
moles = 0.018 L x 0.20 M = 0.0036 moles
Since the ratio of KHP to NaOH is 1:1, we need 0.0036 moles of KHP to neutralize 0.0036 moles of NaOH.
Finally, we can find the molar mass of KHP from the periodic table, which is approximately 204.22 g/mol.
To calculate the mass of KHP needed, multiply the number of moles (0.0036 moles) by the molar mass (204.22 g/mol):
mass of KHP = 0.0036 moles x 204.22 g/mol ≈ 0.737 g
Therefore, approximately 0.737 grams of KHP is needed to neutralize 18 mL of 0.20 M NaOH.