Question

One liter of a solution is found to contain 0.022 moles of HCl. Calculate the pH of the solution. Assume complete dissociation.

Answer 1

Answer:

The pH of the solution is 1.66

Explanation:

Step 1: Data given

Number of moles HCl = 0.022 moles

Molar mass of HCl = 36.46 g/mol

Step 2: Calculate molarity of HCl

Molarity HCl = moles HCl / volume

Molarity HCl = 0.022 moles / 1 L = 0.022 M

[HCl] = [H+] = 0.022 M

Step 3: Calculate pH

pH = -log [H+]

pH = -log(0.022)

pH = 1.66

The pH of the solution is 1.66

Answer 2

Answer: 1.66

Explanation:

First, we calculate for the molarity of HCl as follows:

Number of mole HCl = 0.022mol

Volume = 1L

Molarity = mole /Volume

Molarity = 0.022mol /1L = 0.022mol/L

The dissociation equation of HCl is given below

HCl <==> H^+ + Cl^-

Since 1mole of HCl dissociate to produce 1 mol of H^+, therefore, 0.022mol/L HCl will also produce 0.022mol/L of H^+

We can obtain the pH is a solution using:

pH = - Log [H^+]

pH = - Log 0.022

pH = 1.66