Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25

검증된 단계별 안내

Understand that pH is a measure of the acidity of a solution, defined as the negative logarithm (base 10) of the hydronium ion concentration: \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).

To find the \([\text{H}_3\text{O}^+]\) concentration from a given pH, use the inverse of the logarithm function: \([\text{H}_3\text{O}^+] = 10^{-\text{pH}}\).

Substitute the given pH value into the equation: \([\text{H}_3\text{O}^+] = 10^{-14.25}\).

Calculate the power of 10 using the given pH value to find the \([\text{H}_3\text{O}^+]\) concentration.

Ensure that the final answer is expressed with the correct number of significant figures, which should match the number of decimal places in the given pH value.

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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 basicity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.

Hydronium Ion Concentration

The concentration of hydronium ions (H3O+) in a solution is directly related to its pH. The formula to calculate H3O+ concentration from pH is [H3O+] = 10^(-pH). This relationship allows for the conversion of pH values into molarity of hydronium ions, which is essential for understanding the solution's acidity.

Significant Figures

Significant figures are the digits in a number that contribute to its precision. When performing calculations, especially in chemistry, it is crucial to report results with the correct number of significant figures based on the precision of the measurements involved. This ensures that the reported concentration accurately reflects the reliability of the data.