What is the pH of a solution that has a concentration of hydronium ions that is 1.8 × 10-4 molar H3O+? Show, or explain, the work used to solve this problem.
pH = -log(H^+)
Substitute and solve for pH.
To find the pH of a solution with a given concentration of hydronium ions (H3O+), you can use the formula for pH, which is defined as the negative logarithm (base 10) of the hydronium ion concentration.
The formula for pH is: pH = -log[H3O+]
Given that the concentration of hydronium ions ([H3O+]) is 1.8 × 10-4 M (molar), you can plug this value into the formula.
pH = -log(1.8 × 10-4)
Now, let's break down the steps to solve this problem:
Step 1: Take the negative logarithm of the hydronium ion concentration.
The hydronium ion concentration is 1.8 × 10-4. Take the negative logarithm of this value using a scientific calculator.
-log(1.8 × 10-4) ≈ 3.74
Step 2: Round the answer to two decimal places.
Since pH values are typically expressed with two decimal places, round the answer to 3.74.
Therefore, the pH of the solution with a concentration of hydronium ions of 1.8 × 10-4 M is approximately 3.74.