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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?
Moles of H+ present in the final solution = 0.178
The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight/volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.
Molarity shows the number of moles of solute in every 1 liter of solution or mmol in each ml of solution
[tex]\tt M=\dfrac{n}{V}[/tex]
Where
M = Molarity , M
n = number of moles of solute, mol
V = Volume of a solution, L
mol HBr :
= 0.43 L x 0.23 M
= 0.0989
HBr⇒H⁺ + Br⁻
mol H⁺= mol HBr = 0.0989
mol HClO₄ :
= 0.225 x 0.35
= 0.07875
HClO₄ ⇒ H⁺ + ClO₄⁻
mol H⁺ = mol HClO₄ = 0.07875
mol H⁺ total :
= mol H⁺in HBr + mol H⁺ in HClO₄
= 0.0989 + 0.07875
= 0.17765
= 0.178
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