Sulfamic acid, HSO₃NH₂ (molar mass = 97.1 g/mol) , is a strong monoprotic acid that can be used to standardize a strong base:
HSO₃NH₂(aq) + KOH(aq) → KSO₂NH₂(aq) + H₂O(l)
A 0) 179-g sample of HSO₃NH₂ required 19.4 mL of an aqueous solution of KOH for complete reaction. What is the molarity of the KOH solution?

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of HSO₃NH₂: n = m/M = 0.179 g / 97.1 g/mol = 0.00184 mol According to the balanced chemical equation, 1 mole of KOH reacts with 1 mole of HSO₃NH₂. Therefore, the number of moles of KOH used in the reaction is also 0.00184 mol. Finally, we can calculate the molarity of the KOH solution: Molarity = moles of solute / volume of solution (in liters) Molarity = 0.00184 mol / 0.0194 L = 0.0950 M Therefore, the correct answer is D) 0.0950 M.

Sulfamic Acid, HSO3NH2 (Molar Mass = 97

Sulfamic Acid, HSO₃NH₂ (Molar Mass = 97