Question

Potassium hydrogen phthalate, KHP, is a monoprotic acid often used to standardize NaOH solutions. If 0.212 g of KHP are dissolved into 50.00 mL of water and titrated with 35.00 mL of NaOH, what is the molarity of NaOH. Molar mass of KHP

Answer 1

The molarity of the NaOH solution is 0.03 M

We'll begin by calculating the mole of the KHP

• Mass = 0.212 g
• Molar mass = 204.22 g/mol
• Mole of KHP =?

Mole = mass /molar mass

Mole of KHP = 0.212 / 204.22

Mole of KHP = 0.001 mole

Next, we shall determine the molarity of the KHP solution

• Mole of KHP = 0.001 mole
• Volume = 50 mL = 50/1000 = 0.05 L
• Molarity of KHP =?

Molarity = mole / Volume

Molarity of KHP = 0.001 / 0.05

Molarity of KHP = 0.02 M

Finally , we shall determine the molarity of the NaOH solution

KHP + NaOH —> NaPK + H₂O

From the balanced equation above,

• The mole ratio of the acid, KHP (nA) = 1
• The mole ratio of base, NaOH (nB) = 1

From the question given above, the following data were obtained:

• Volume of acid, KHP (Va) = 50 mL
• Molarity of acid, KHP (Ma) = 0.02 M.
• Volume of base, NaOH (Vb) = 35 mL
• Molarity of base, NaOH (Mb) =?

MaVa / MbVb = nA / nB

(0.02 × 50) / (Mb × 35) = 1

1 / (Mb × 35) = 1

Cross multiply

Mb × 35 = 1

Divide both side by 35

Mb = 1 / 35

Mb = 0.03 M

Thus, the molarity of the NaOH solution is 0.03 M

Complete question:

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