Sep . 30, 2024 17:58 Back to list

Exploring the pH of a 0.05% Sodium Hydroxide Solution

Understanding the pH of 0.05% NaOH Solution

Sodium hydroxide (NaOH) is a strong base widely used in various industries, laboratories, and even household cleaning products. When NaOH is dissolved in water, it dissociates completely into sodium (Na⁺) and hydroxide ions (OH⁻). This dissociation is the basis for understanding the pH level of sodium hydroxide solutions, particularly a dilute solution like 0.05% NaOH.

The Concentration of the Solution

First, let’s break down what a 0.05% NaOH solution means in practical terms. A 0.05% solution indicates that there are 0.05 grams of NaOH in every 100 milliliters of water. To convert this weight/volume percentage to molarity, we need to know the molar mass of NaOH, which is approximately 40 g/mol.

Calculating the molarity involves the formula

\[ \text{Molarity (M)} = \frac{\text{Mass of solute (g)}}{\text{Molar mass (g/mol)} \times \text{Volume of solution (L)}} \]

For our 0.05% NaOH solution

\[ \text{Mass of solute} = 0.05 \text{ g} \] \[ \text{Volume of solution} = 100 \text{ mL} = 0.1 \text{ L} \]

Using the molar mass to find the molarity

\[ \text{Molarity} = \frac{0.05 \text{ g}}{40 \text{ g/mol} \times 0.1 \text{ L}} = \frac{0.05}{4} = 0.0125 \text{ M} \]

Thus, a 0.05% NaOH solution translates to a molarity of 0.0125 M.

Determining the pH

The pH scale ranges from 0 to 14, with 7 being neutral. Values below 7 indicate acidic solutions, while those above 7 indicate basic solutions. The pH of a solution can be calculated using the concentration of hydroxide ions in the solution. The relationship is given by

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

Since NaOH is a strong base, it completely dissociates in solution. Thus, the concentration of hydroxide ions [OH⁻] in the 0.0125 M NaOH solution is also 0.0125 M.

0.05 m naoh ph

Calculating the pOH

\[ \text{pOH} = -\log(0.0125) \approx 1.9 \]

To find the pH, we can use the relationship between pH and pOH

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

Thus

\[ \text{pH} = 14 - \text{pOH} = 14 - 1.9 = 12.1 \]

Implications of the pH Value

A pH of 12.1 indicates that a 0.05% NaOH solution is quite basic. Such a pH level has several implications

1. Corrosive Nature Solutions with a pH significantly above 7 can exhibit corrosive properties. Precautions must be taken when handling NaOH solutions, as they can cause skin burns and eye damage.

2. Applications in Laboratories Due to its basic nature, NaOH is often used in titrations, neutralization reactions, and as a standard base in various chemical analyses.

3. Role in Industry In industrial applications, NaOH is used in the manufacture of soaps, detergents, and various chemicals, stressing the importance of pH in product formulation.

4. Environmental Considerations The release of NaOH into the environment can alter pH levels in water bodies, affecting aquatic life.

Conclusion

Understanding the pH of a 0.05% NaOH solution is crucial for safely handling and utilizing this powerful chemical. The basic pH of 12.1 not only reflects its strong alkaline nature but also highlights the importance of awareness and precautions in both laboratory and industrial settings. Whether for practical applications or environmental safety, knowledge of this basic compound plays a vital role across various fields.

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