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Exploring the pH Level of 0.001% Sodium Hydroxide Solution

Understanding the pH of 0.001% NaOH Solution

When we discuss the properties of solutions in chemistry, one of the most essential aspects is their pH level, which is a measure of the acidity or basicity of a solution. In this article, we will explore the pH of a 0.001% sodium hydroxide (NaOH) solution, delve into the implications of its basicity, and discuss the practical applications of such a solution.

Introduction to Sodium Hydroxide

Sodium hydroxide, commonly known as lye or caustic soda, is a strong base that dissociates completely in aqueous solutions. When NaOH dissolves in water, it separates into sodium ions (Na⁺) and hydroxide ions (OH⁻). The presence of hydroxide ions is primarily responsible for elevating the pH of the solution above 7, indicating its basic nature.

Calculating the pH of 0.001% NaOH

To convert the percentage concentration into molarity, we need to understand that 0.001% w/v (weight/volume) means that there are 0.001 grams of NaOH in 100 milliliters of the solution. The molecular weight of NaOH is approximately 40 grams/mol. Therefore, in 0.001 g of NaOH

\[ \text{Moles of NaOH} = \frac{0.001 \text{ g}}{40 \text{ g/mol}} = 0.000025 \text{ mol} \]

Given that this is in 100 mL of solution, the molarity (M) is

\[ \text{Molarity} = \frac{0.000025 \text{ mol}}{0.1 \text{ L}} = 0.00025 \text{ M} \]

In a strong base like NaOH, we can directly relate the hydroxide ion concentration to the pH. The concentration of hydroxide ions (\([OH^-]\)) is equal to the molarity of the NaOH solution, which is 0.00025 M.

To find the pOH of the solution, we can use the formula

\[ \text{pOH} = -\log([OH^-]) = -\log(0.00025) \approx 3.60 \]

0.001 m naoh ph

The relationship between pH and pOH is given by the equation

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

Thus, we can calculate the pH

\[ \text{pH} = 14 - \text{pOH} = 14 - 3.60 \approx 10.40 \]

Therefore, the pH of a 0.001% NaOH solution is approximately 10.40, indicating it is basic.

Practical Implications and Uses

Given its basicity, a 0.001% NaOH solution has several practical applications. It is commonly used in laboratory settings for titrations and pH adjustments, as well as in various chemical analyses. Additionally, it serves as a cleaning agent in a diluted form, effectively helping to remove grease and stains.

Moreover, understanding the pH of sodium hydroxide solutions is crucial in industries such as pharmaceuticals and food processing, where maintaining the appropriate pH is essential to ensure product quality and safety.

Safety Considerations

While a 0.001% NaOH solution is relatively safe to handle compared to more concentrated solutions, it is essential to exercise caution. Sodium hydroxide can cause irritation to the skin, eyes, and respiratory system. Proper personal protective equipment (PPE), such as gloves and safety goggles, should always be used when handling even dilute solutions of strong bases.

Conclusion

In conclusion, a 0.001% NaOH solution has a pH of approximately 10.40, reflecting its basic nature. Understanding the properties and implications of this solution is crucial for various scientific and industrial applications. As with all chemical substances, it is vital to handle sodium hydroxide with care to ensure safety in practical applications. The knowledge of pH and its role in chemical solutions remains a fundamental aspect of studying and working within the field of chemistry.

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