Determine the moles of H+ reacting with the metal based on the following experimental data. 10.00 mL of 1.00 M HCl solution is added to a sample of Mg metal. The reaction goes to completion and all of the Mg metal is gone. 21.80 mL of 0.30 M NaOH solution is required to reach the end point when titrating the remaining HCl.

0.01 mol of H+.

Explanation:

Equation of reaction:

Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g)

Molar concentration = number of moles/volume

= 1*0.01

= 0.01 mol.

Dissociation:

2HCl --> 2H+ + 2Cl-

By stoichiometry,

If 2 mole of HCl dissociates to guve 2 moles of H+

Number of moles of H+ = 0.01 mol.

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