Question

An aqueous solution of hydrochloric acid is standardized by titration with a 0.137 M solution of sodium hydroxide. If 16.1 mL of base are required to neutralize 27.9 mL of the acid, what is the molarity of the hydrochloric acid solution

Answer 1

The molarity of the hydrochloric acid, HCl solution given the data is 0.079 M

Balanced equation

HCl + NaOH —> NaCl + H₂O

From the balanced equation above,

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

How to determine the molarity of HCl

• Molarity of base, NaOH (Mb) = 0.137 M

• Volume of base, NaOH (Vb) = 16.1 mL
• Volume of acid, HCl (Va) = 27.9 mL
• Molarity of acid, HCl (Ma) =?

MaVa / MbVb = nA / nB

(Ma × 27.9) / (0.137 × 16.1) = 1

(Ma × 27.9) / 2.2057  = 1

Cross multiply

Ma × 27.9 = 2.2057

Divide both side by 27.9

Ma = 2.2057 / 27.9

Ma = 0.079 M

Thus, the molarity of the HCl solution is 0.079 M

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