Determine the pH for the following solutions:c. [H3O+] = 0.0001 M

Ch.10 Acids and Bases and Equilibrium

Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 14th Edition

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Timberlake 14th Edition

Ch.10 Acids and Bases and Equilibrium

문제 88c

10장, 문제 88c

Determine the pH for the following solutions:
c. [H₃O⁺] = 0.0001 M

검증된 단계별 안내

Step 1: Recall the formula for calculating pH, which is given by:

pH = - \log ({[H}_{3 O}])

. This formula relates the hydronium ion concentration to the pH of the solution.

Step 2: Identify the given value for the hydronium ion concentration,

{[H}_{3 O}]

, which is 0.0001 M.

Step 3: Substitute the given value of

{[H}_{3 O}

into the pH formula:

pH = - \log (0.0001)

Step 4: Simplify the logarithmic expression. Recall that

\log (10^- 4)

simplifies to -4, so

- \log (0.0001)

becomes 4.

Step 5: Conclude that the pH of the solution is equal to 4. This indicates that the solution is acidic, as pH values less than 7 correspond to acidic solutions.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

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53s

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주요 개념

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pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate alkalinity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.

Hydronium Ion Concentration

Hydronium ions (H₃O⁺) are formed when an acid donates a proton to water. The concentration of hydronium ions in a solution directly influences its pH. For example, a higher concentration of H₃O⁺ results in a lower pH, indicating a more acidic solution.

Calculating pH

To calculate pH from hydronium ion concentration, the formula pH = -log[H₃O⁺] is used. This formula allows for the conversion of the molarity of hydronium ions into a pH value. For instance, if [H₃O⁺] = 0.0001 M, the pH can be calculated as 4, indicating an acidic solution.