The reaction of neutralization of magnesium hydroxide by hydrochloric acid is:
Mg(OH)2 + 2HCl→ MgCl2 + 2H2O.
Therefore, 1 mol of magnesium hydroxide reacts with 2 mol of hydrogen chloride:
n(Mg(OH)2)=2n(HCl) .
The number of the moles of magnesium hydroxide can be calculated as its mass divided by its molar mass (58.32 g/mol):
n(Mg(OH)2)=Mm=58.32 g/mol12.0⋅10−3 g=2.058⋅10−4 mol.
The number of the moles of HCl is then the double of this value:
n(HCl)=n(Mg(OH)2)⋅2=4.115⋅10−4 mol .
Finally, the volume of the HCl solution would be neutralized is:
V=cn=0.010 mol/L4.115⋅10−4 mol=41.2 mL.
Answer: the volume of 0.010 mol/L HCl would be neutralized by a teaspoon of antacid is 41.2 mL.
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