A 430. ML solution of 0.230 M HBr (aq) is mixed with a solution of 225 mL of 0.350 M HClO4 (aq). How many moles of H + (aq) are present in the final solution?

Given:

volume of HBr = 430 ml = 0.430 L

Molarity of HBr = 0.230 M

Volume of HClO4 = 225 ml = 0.225 L

Molarity of HClO4 = 0.350 M

To determine:

Total moles of H + when HBr and HClO4 are mixed

Explanation:

HBr and HClO4 are strong acids. Hence:

Concentration of H + from HBr = 0.230 M

Concentration of H + from HClO4 = 0.350 M

Now:

# moles of H + from HBr = 0.430 L * 0.230 moles/L = 0.0989 moles

# moles of H + from HClO4 = 0.225 L * 0.350 moles/L = 0.0788 moles

Total moles of H + = 0.0989 + 0.0788 = 0.1777 moles

Ans: Total # moles of H + is 0.178