Question

in a standardization reaction between khp and naoh, initial and final buret readings were 3.70 and 13.95 ml respectively. if the titration involved 0.2501 g of khp, what is the concentration of naoh? molar mass of khp: 204.22 g/mol

Answer 1

To find the molarity of the NaOH solution, the volume of NaOH solution used is calculated, the mass of KHP is converted to moles, and since the reaction has a 1:1 molar ratio, the moles of NaOH are equal to the moles of KHP. Finally, the molarity is found by dividing the moles of NaOH by the volume of the NaOH solution.

Step-by-step explanation:

To determine the concentration of NaOH, first, we calculate the volume of NaOH solution used during the titration. This is done by subtracting the initial buret reading from the final buret reading: 13.95 mL − 3.70 mL = 10.25 mL or 0.01025 L.

Next, we need to calculate the moles of KHP that reacted with NaOH. Since the molar mass of KHP is given as 204.22 g/mol, we convert the mass of KHP used in the titration to moles: 0.2501 g KHP × (1 mol KHP / 204.22 g KHP) = 0.001225 mol KHP.

The balanced equation for the reaction of KHP with NaOH is: KHP + NaOH → KP + H₂O. This indicates a 1:1 molar ratio between KHP and NaOH. Therefore, the moles of NaOH are the same as the moles of KHP, which is 0.001225 mol.

We can now calculate the molarity of the NaOH solution by dividing the moles of NaOH by the volume of NaOH solution in liters: 0.001225 mol NaOH / 0.01025 L NaOH = 0.1195 M NaOH.