Hydrogen ion concentration of the following acidic solution?

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What is the hydrogen ion concentration of the following acidic solution? 2.34L containing 3.45 grams of HCl hydrochloric acid. This is all I have been given. I am so confused how to find hydrogen ion concentration when I only have the compound, the grams, and the liters. Please help.

Sample Solution

Certainly, let’s solve for the hydrogen ion concentration (H+) of the hydrochloric acid solution you described. Here’s how we can find it:

  1. Calculate the molarity (M) of the HCl solution:
    • Molarity (M) = moles of solute (HCl) / liters of solution (L)

We need to find the moles of HCl first.

  1. Convert grams of HCl to moles of HCl:
    • Moles of HCl = grams of HCl / molar mass of HCl

The molar mass of HCl is 36.46 g/mol (1 atom H + 1 atom Cl).

  1. Plug the values into the equations:
    • Moles of HCl = 3.45 grams / 36.46 g/mol = 0.0946 mol
    • Molarity (M) of HCl solution = 0.0946 mol / 2.34 L = 0.0404 M

Important Note:

Hydrochloric acid (HCl) is a strong acid, meaning it dissociates completely in water. This implies that for every molecule of HCl that dissolves, it releases one H+ ion and one Cl- ion.

Therefore, the hydrogen ion concentration (H+) is equal to the molarity of the HCl solution (since each HCl molecule dissociates into one H+ ion).

 

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