Question

An antacid tablet containing Mg(OH)₂(s) (molar mass 58.3 g/mol) is titrated with a 0.100 M solution of The end point is determined by using an indicator. Based on the data in the able above, what was the mass of the Mg(OH)₂(s) in the antacid tablet?

(A) 0.0583 g
(B) 0.583 g
(C) 5.83 g
(D) 58.3 g

Answer 1

To find the mass of Mg(OH)₂(s) in the antacid tablet, we need to use the stoichiometry of the reaction and the volume and molarity of the titrant.

Step-by-step explanation:

To find the mass of Mg(OH)2(s) in the antacid tablet, we need to use the stoichiometry of the reaction and the volume and molarity of the titrant. From the balanced equation, we can see that 1 mole of Mg(OH)2(s) reacts with 2 moles of NaOH(aq). Therefore, the moles of Mg(OH)2(s) in the antacid tablet is half of the moles of NaOH(aq) used in the titration. The moles of NaOH(aq) can be calculated using the volume and molarity of the titrant. Finally, we can convert moles of Mg(OH)2(s) to grams using its molar mass.

Mass of Mg(OH)2(s) = (moles of NaOH(aq) / 2) x molar mass of Mg(OH)2(s)