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10 naoh ph

Understanding the pH of 10% Sodium Hydroxide (NaOH) Solution

Sodium hydroxide (NaOH), commonly known as caustic soda or lye, is a highly versatile compound with a wide range of applications in industrial and laboratory settings. It is a strong alkaline substance, and its solutions can exhibit significant changes in pH depending on their concentration. A 10% solution of NaOH is particularly noteworthy due to its strong basicity and corresponding pH level, which can have profound implications for various applications, from chemical manufacturing to everyday household cleaning.

Chemical Properties of Sodium Hydroxide

Sodium hydroxide is an ionic compound composed of sodium (Na⁺) and hydroxide (OH⁻) ions. When NaOH is dissolved in water, it dissociates completely into these ions, resulting in a highly alkaline solution. The dissociation can be represented by the following chemical equation

\[ \text{NaOH (s)} \rightarrow \text{Na}^+ (aq) + \text{OH}^- (aq) \]

As a strong base, NaOH is capable of increasing the concentration of hydroxide ions (OH⁻) in solution, which significantly raises the pH. The pH scale, which ranges from 0 to 14, measures the acidity or basicity of a solution. A pH of 7 is considered neutral, values below 7 indicate acidity, and values above 7 indicate alkalinity.

Calculating the pH of a 10% NaOH Solution

The pH of a 10% NaOH solution can be calculated using the concentration of hydroxide ions produced. A 10% NaOH solution typically contains 10 grams of NaOH in 100 milliliters of water. Since the molar mass of NaOH is approximately 40 g/mol, the number of moles in a 10-gram sample can be calculated as follows

\[ \text{Moles of NaOH} = \frac{10 \, \text{g}}{40 \, \text{g/mol}} = 0.25 \, \text{mol} \]

In 100 mL (0.1 L) of solution, this corresponds to a concentration of

\[ \text{Concentration (mol/L)} = \frac{0.25 \, \text{mol}}{0.1 \, \text{L}} = 2.5 \, \text{mol/L} \]

Next, we can determine the pOH of the solution. Since the pOH is calculated as

\[ \text{pOH} = -\log[\text{OH}^-] \]

10 naoh ph

For a 2.5 mol/L NaOH solution, the pOH can be calculated as

\[ \text{pOH} = -\log(2.5) \approx -0.4 \]

To find the pH, we can use the relationship

\[ \text{pH} + \text{pOH} = 14 \]

Thus,

\[ \text{pH} = 14 - (-0.4) = 14 + 0.4 = 14.4 \]

Given this calculation, the pH of a 10% NaOH solution is significantly above the neutral range, indicating a highly alkaline environment.

Implications of High pH

The high pH of a 10% NaOH solution has numerous implications for its use. In industrial applications, such as soap making, textile processing, and water treatment, the strong basicity of NaOH facilitates chemical reactions that neutralize acids, saponify fats, or adjust pH levels. However, the high pH also requires caution. NaOH is corrosive, and proper handling is essential to prevent chemical burns or damage to materials.

In laboratory settings, sodium hydroxide is frequently used as a reagent for titrations and other chemical reactions. Its strong basicity allows chemists to quickly neutralize acids and maintain alkaline conditions during experiments. Understanding the pH of solutions is crucial for conducting experiments effectively and safely.

Conclusion

In summary, a 10% sodium hydroxide solution is characterized by its strong basicity, resulting in a pH significantly above 14. Its applications range from industrial to laboratory uses, but its high pH also necessitates careful handling due to its corrosive nature. Understanding the properties and implications of such solutions is essential for safe and effective use in various fields.

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