Sulfamic acid,HSO₃NH₂(molar mass = 97.1 g/mol),is a strong monoprotic acid that can be used to standardize a strong base: A 0.165-g sample of HSO₃NH₂required 19.4 mL of an aqueous solution of KOH for a complete reaction.What is the molarity of the KOH solution?

Question

Quizplus · Accepted Answer

First, we need to find the number of moles of sulfamic acid used in the reaction: moles of HSO₃NH₂=0.165 g/97.1 g/mol=0.00170 mol Since sulfamic acid is a monoprotic acid, the number of moles of KOH used in the reaction is also 0.00170 mol. Now, we can use the volume of KOH solution and the number of moles of KOH to find its molarity: Molarity of KOH=moles of KOH/volume of KOH solution Molarity of KOH=0.00170 mol/19.4 mL=0.00170 mol/0.0194 L=0.0876 M Therefore, the molarity of the KOH solution is 0.0876 M, which corresponds to choice C.

Sulfamic Acid,HSO3NH2 (molar Mass = 97

Sulfamic Acid,HSO₃NH₂(molar Mass = 97