What is the pH of a solution that has a concentration of hydronium ions that is 4.7 × 10-4 molar H3O+? Show, or explain, the work used to solve this problem.
pH = -log(H3O^+)
To determine the pH of a solution, you need to use the formula pH = -log[H3O+], where [H3O+] represents the concentration of hydronium ions in moles per liter (M). In this case, the concentration of hydronium ions is given as 4.7 × 10^-4 M H3O+.
Step 1: Plug the given concentration of hydronium ions into the equation:
pH = -log(4.7 × 10^-4)
Step 2: Calculate the logarithm of the concentration using the base 10 logarithm:
pH = -log(4.7 × 10^-4)
= -log(4.7) - log(10^-4)
≈ -0.672 + 4
Note that since the concentration is given in scientific notation, you can split it into two logarithms and then sum them.
Step 3: Subtract the logarithms:
pH ≈ 3.328
Therefore, the pH of the solution with a hydronium ion concentration of 4.7 × 10^-4 M is approximately 3.328.