Final answer:
The mass of KHP required to react with 26.0 mL of 0.115 M NaOH solution is approximately 0.59 grams. This is calculated by first finding the moles of NaOH and then using the stoichiometry of the reaction to find the corresponding mass of KHP needed.
Step-by-step explanation:
The question is asking what mass of solid potassium hydrogen phthalate (KHP) would be required to react completely with a given volume and concentration of sodium hydroxide (NaOH) solution. The reaction between KHP and NaOH is a common titration process in chemistry. The molar mass of KHP is provided, which is necessary to calculate the mass.
To find the amount of KHP needed, first calculate the number of moles of NaOH in the 26.0 mL of 0.115 M solution:
Moles of NaOH = Volume (L) × Concentration (M)
Moles of NaOH = 0.026 L × 0.115 M = 0.00299 mol
The balanced chemical equation for the reaction between KHP and NaOH is:
KHP (aq) + NaOH (aq) → KNaP (aq) + H₂O (l)
Since the ratio is 1:1, the moles of NaOH will be the same as moles of KHP. Next, convert moles of KHP to grams:
Mass of KHP = Moles × Molar Mass
Mass of KHP = 0.00299 mol × 204.2 g/mol = 0.610 g
The closest answer to 0.610 g from the options is 0.59 g (Option B).