What is the minimum volume of 5.0 M HCl required to completely dissolve 10.0 g of magnesium metal?
Solution 91P :
Molarity of HCl(Hydrochloric acid) = 5.0 M
Amount of Mg metal = 10.0 g
Volume of HCl to completely dissolve Mg = ?
Let’s write the chemical equation for the given scenario :
Mg(s) + 2HCl → MgCl2 + H2(g)
From the above reaction, we see the ratio of reactants is 1 : 2.
Now, let’s find the number of moles of Mg and HCl :
Number of moles(n) =
Molar mass of Mg = 24.305 g/mol.
Therefore, n =
= 0.411 moles.
We are not given the mass of HCl, but from the reaction, we know that the ratio of Mg and HCl is 1 : 2. Hence, we calculate the moles of HCl as :
= 0.411 2
= 0.822 moles.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
The full step-by-step solution to problem: 91P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 91P from 14 chapter was answered, more than 333 students have viewed the full step-by-step answer. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This full solution covers the following key subjects: completely, dissolve, HCL, magnesium, metal. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The answer to “What is the minimum volume of 5.0 M HCl required to completely dissolve 10.0 g of magnesium metal?” is broken down into a number of easy to follow steps, and 18 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5.