A0.485 g sample of khp was dissolved in water. it took 28.74 ml of naoh solution to reach the endpoint. what is the molarity of the naoh solution?

0.237 M The balanced equation for the reaction is KHP + NaOH ==> H2O + NaKP So for each mole of KHP, it takes 1 mole of NaOH to neutralize. So let's determine how many moles of KHP we had. Start with the atomic weights. Atomic weight potassium = 39.0983 Atomic weight hydrogen = 1.00794 Atomic weight phosphorus = 30.973762 Molar mass KHP = 39.0983 + 1.00794 + 30.973762 = 71.080002 g/mol Moles KHP = 0.485 g / 71.080002 g/mol = 0.006823298 mol Because of the 1 to 1 ratio of KHP and NaOH, we know that we used 0.006823298 moles of NaOH. And since molarity is defined as moles per liter, just divide the number of moles by the number of liters. So 0.006823298 mol / 0.02874 l = 0.237414666 M. Rounding to 3 significant figures gives 0.237 M

Dmight be the correct answer