Determining the Molar Concentration of a Nitric Acid Solution

What is the molar concentration of a nitric acid solution with a pH of 1.75? The molar concentration of a nitric acid solution with a pH of 1.75 is approximately 1.78 × 10^-2 M.

Understanding the Relationship between pH and Molar Concentration

pH is a measure of how acidic or basic a solution is and is defined as the negative logarithm (base 10) of the concentration of hydrogen ions [H+] in the solution. The lower the pH value, the higher the concentration of hydrogen ions and the more acidic the solution.

Calculating Molar Concentration from pH

To determine the molar concentration of a nitric acid solution with a pH of 1.75, we can use the pH formula: pH = -log[H+]. By rearranging the formula, we can calculate the hydrogen ion concentration [H+]: [H+] = 10^-pH.

Calculation Steps

1. pH = 1.75

2. [H+] = 10^-1.75

3. [H+] ≈ 1.78 × 10^-2 M

Conclusion

The molar concentration of the nitric acid solution with a pH of 1.75 is approximately 1.78 × 10^-2 M. This value represents the concentration of hydrogen ions in the solution, indicating its acidic nature.

← Structural isomers of pentane and hexane formulas and names Cell potential the driving force behind redox reactions →

More Posts: