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Lesson 4: Acids, bases, and pH. Autoionization of water. Arrhenius acids and bases. Brønsted–Lowry acids and bases. Definition of pH. Introduction to buffers. Acids, bases, pH, and buffers.
Definitions of pH, pOH, and the pH scale. Calculating the pH of a strong acid or base solution. The relationship between acid strength and the pH of a solution.
We can calculate the pH of a solution by taking the negative logarithm of the hydronium ion concentration, or pH = -log[H₃O⁺]. At 25°C, a solution with pH < 7 is acidic, a solution with pH > 7 is basic, and a solution with pH = 7 is neutral.
High school biology (DEPRECATED) Course: High school biology (DEPRECATED) > Unit 1. Lesson 4: pH, acids, and bases. Introduction to pH. pH, acids, and bases review.
In general, if something has a pH below seven, we tend to refer to it as acidic. We say it is acidic. So typically when you add acids to neutral water, your pH is going to go down, it's going to get more and more acidic.
In this video, we'll solve for [H₃O⁺] and pH in two different worked examples. First, we'll walk through the possible approaches for calculating [H₃O⁺] from pOH. Then, we'll find the pH of pure water at 50°C from the value of the autoionization constant at 50°C.
Unit 8: Acids, bases, and solutions. Our mission is to provide a free, world-class education to anyone, anywhere. Khan Academy is a 501 (c) (3) nonprofit organization. Donate or volunteer today! About.
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If only the cation reacts with water, the solution will be acidic. If only the anion reacts with water, the solution will be basic. If both species react with water, the pH of the solution will depend on the relative strengths of the cation and the anion.
The concentration of H₃O⁺ in a strong acid solution is therefore equal to the initial concentration of the acid. For example, a solution of 0.1 M HNO₃ contains 0.1 M H₃O⁺ and has a pH of 1.0.