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A chemist reacts 30.0 mL of 5.6 M HCl with an excess of Mg(OH)2 How many grams of magnesium will be produced

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Answer:

2.042 g

Explanation:

The reaction that takes place is:

  • 2HCl + Mg(OH)₂ → Mg²⁺ + 2Cl⁻ + 2H₂O

First we calculate how many HCl moles were added, using the given volume and concentration:

  • 30 mL ⇒ 30 / 1000 = 0.030 L
  • 5.6 M * 0.030 L = 0.168 mol HCl

Then we convert HCl moles into Mg²⁺ moles, using the stoichiometric coefficients:

  • 0.168 mol HCl * [tex]\frac{1molMg^{+2}}{2molHCl}[/tex]= 0.084 mol Mg⁺²

Finally we convert Mg moles into grams, using its molar mass:

  • 0.084 mol Mg⁺² * 24.305 g/mol = 2.042 g

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