Acids donate _______________________ to an aqueous solution, which will lead to a(n) _______________________ in pH. In contrast, bases donate _______________________ to an aqueous solution and will _______________________ the pH. The pH of a solution with more OH⁻
than H⁺ will have a(n) _______________________ pH.

Verified step by step guidance

1. Understand the definition of acids and bases in terms of their behavior in aqueous solutions: acids donate protons (H+ ions), while bases donate hydroxide ions (OH−).
2. Fill in the first blank by recognizing that acids donate \( \text{H}^+ \) ions to an aqueous solution.
3. For the second blank, recall that donating \( \text{H}^+ \) ions increases the acidity of the solution, which causes the pH to decrease.
4. Fill in the third blank by noting that bases donate \( \text{OH}^- \) ions to an aqueous solution.
5. For the fourth and fifth blanks, understand that bases increase the concentration of hydroxide ions, which raises the pH, so the pH of a solution with more \( \text{OH}^- \) than \( \text{H}^+ \) will be higher (alkaline).

Key Concepts

Acids and Proton Donation

Acids are substances that donate hydrogen ions (H⁺) or protons to an aqueous solution. This increase in H⁺ concentration causes the solution to become more acidic, resulting in a decrease in pH.

Bases and Hydroxide Ion Donation

Bases are substances that donate hydroxide ions (OH⁻) to an aqueous solution. The addition of OH⁻ reduces the concentration of free H⁺ ions, causing the solution to become more basic or alkaline, which increases the pH.

pH Scale and Ion Concentration

The pH scale measures the acidity or alkalinity of a solution based on H⁺ concentration. A solution with more OH⁻ than H⁺ ions is basic and has a pH greater than 7, while a solution with more H⁺ than OH⁻ is acidic with a pH less than 7.