ഒക്ട് . 02, 2024 17:49 Back to list

0.5 m naoh ph

Understanding the pH of 0.5% NaOH Solution

Sodium hydroxide (NaOH), commonly known as lye or caustic soda, is a strong base widely used in various industrial and laboratory applications. When dissolved in water, it completely dissociates into its constituent ions sodium (Na⁺) and hydroxide (OH⁻). This dissociation results in an increase in the concentration of hydroxide ions, which is the primary factor influencing the pH of the solution.

A 0.5% solution of NaOH can be prepared by dissolving 0.5 grams of NaOH in 100 milliliters of distilled water. To determine the pH of this solution, we first need to understand that NaOH, being a strong base, fully ionizes in aqueous solution. This means that in a 0.5% NaOH solution, the concentration of OH⁻ ions is directly related to the molarity of the solution.

Calculating the pH

The molarity of a NaOH solution can be calculated using its molecular weight, which is approximately 40 g/mol. Thus, a 0.5% solution (which is equivalent to 0.5 g in 100 mL) translates to a molarity as follows

\[ \text{Molarity} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)} \times \text{volume (L)}} \] \[ \text{Molarity} = \frac{0.5 \, \text{g}}{40 \, \text{g/mol} \times 0.1 \, \text{L}} = 0.125 \, \text{mol/L} \]

0.5 m naoh ph

Since NaOH completely dissociates, the concentration of hydroxide ions [OH⁻] will also be 0.125 mol/L. To find the pOH of the solution, we use the formula

\[ \text{pOH} = -\log[\text{OH⁻}] \] \[ \text{pOH} = -\log(0.125) \approx 0.903 \]

Next, we can find the pH using the relationship between pH and pOH

\[ \text{pH} + \text{pOH} = 14 \] \[ \text{pH} = 14 - \text{pOH} \approx 14 - 0.903 \approx 13.097 \]

Conclusion

In summary, a 0.5% NaOH solution has a pH of approximately 13.1, indicating that it is strongly basic. This pH value is consistent with the characteristics of solutions containing strong bases. Understanding the pH of sodium hydroxide solutions is essential for various applications ranging from chemical manufacturing and waste treatment to laboratory experiments. It is also vital for safety considerations, as such caustic solutions can cause severe chemical burns and must be handled with appropriate precautions. Therefore, knowledge of pH and its implications is crucial for anyone working with NaOH or similar substances.

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