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0.5 m naoh ph

Understanding the pH of 0.5% Sodium Hydroxide Solution

Sodium hydroxide (NaOH), commonly known as lye or caustic soda, is a strong base that plays a significant role in various industrial and laboratory processes. A 0.5% sodium hydroxide solution represents a concentration of 0.5 grams of NaOH dissolved in 100 mL of water, which is a relatively dilute solution. Understanding the pH of this solution is essential for many practical applications, from chemical manufacturing to laboratory experiments and even certain household tasks.

To comprehend the pH of a 0.5% NaOH solution, we first need to understand what pH is. The pH scale, which ranges from 0 to 14, is a logarithmic scale used to measure the acidity or basicity of a solution. A pH of 7 is considered neutral, while values below 7 indicate acidity, and values above 7 indicate basicity. Since sodium hydroxide is a strong base, one would expect its solution to have a pH significantly greater than 7.

When NaOH is dissolved in water, it ionizes completely into sodium ions (Na⁺) and hydroxide ions (OH⁻). The hydroxide ions produced are responsible for the basic properties of the solution. To calculate the pH of a 0.5% NaOH solution, we must first determine its concentration in moles per liter (molarity).

The molecular weight of NaOH is approximately 40 g/mol. Therefore, a 0.5% solution contains 0.5 g of NaOH per 100 mL, which translates to

\[ \text{Molarity (M)} = \frac{\text{grams}}{\text{molecular weight} \times \text{liters}} = \frac{0.5 \, \text{g}}{40 \, \text{g/mol} \times 0.1 \, \text{L}} = 0.125 \, \text{M} \]

With a hydroxide ion concentration of 0.125 M, we can now calculate the pOH of the solution. The pOH is determined using the formula

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

Thus,

0.5 m naoh ph

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

Since the pH and pOH of a solution are related through the equation

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

we can find the pH of our solution

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

This indicates that the pH of a 0.5% sodium hydroxide solution is approximately 13.1, confirming that it is indeed a highly basic solution.

The high pH of a 0.5% NaOH solution has significant implications in various applications. In laboratories, it is commonly used for titration experiments, where it serves as a reagent to neutralize acidic solutions. In industrial settings, NaOH solutions are integral in the manufacturing of soaps, detergents, and various chemical products. Additionally, the basicity of NaOH makes it effective in cleaning agents, especially for breaking down grease and organic compounds.

Safety is a crucial consideration when handling sodium hydroxide solutions. Due to its corrosive nature, even a dilute solution can cause skin irritation and damage if not handled properly. Appropriate personal protective equipment, such as gloves and eye protection, should be worn to mitigate the risk of accidents.

In conclusion, a 0.5% sodium hydroxide solution exhibits a pH of approximately 13.1, making it a strong base with various practical applications. Understanding the properties of this solution is vital for its safe and effective use in both industrial and laboratory environments. Whether it be in chemical synthesis, cleaning applications, or educational experiments, knowing the pH and safe handling practices of sodium hydroxide solutions ensures effective outcomes and minimizes risks.

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