Sodium acetate is a chemical compound with the formula CH3COONa. It is a salt formed by the neutralization of acetic acid (CH3COOH) with sodium hydroxide (NaOH). Sodium acetate is commonly used in various applications, including as a food preservative, a buffer solution, and a deicing agent.
In the context of the chapter on 14.4 Hydrolysis of Salts, sodium acetate is an important example of a salt that undergoes hydrolysis, a chemical reaction where a salt reacts with water to produce an acidic or basic solution.
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Sodium acetate is a white, crystalline solid that is highly soluble in water and has a slightly salty, sweet taste.
When dissolved in water, sodium acetate undergoes hydrolysis, producing a basic solution with a pH greater than 7.
The hydrolysis of sodium acetate is an example of a salt of a weak acid and a strong base, which results in a basic solution.
Sodium acetate is commonly used as a food preservative to prevent the growth of microorganisms and extend the shelf life of foods.
In the context of 14.4 Hydrolysis of Salts, sodium acetate is a key example of how the hydrolysis of salts can produce acidic or basic solutions.
Review Questions
Explain how the hydrolysis of sodium acetate results in a basic solution.
When sodium acetate (CH3COONa) is dissolved in water, it undergoes hydrolysis. The acetate ion (CH3COO-) from the salt reacts with water to form a basic solution. This is because the acetate ion is the conjugate base of the weak acetic acid (CH3COOH), and it accepts a proton from water, producing hydroxide ions (OH-) and increasing the pH of the solution. The overall reaction can be represented as: CH3COO- + H2O ⇌ CH3COOH + OH-, resulting in a basic solution with a pH greater than 7.
Describe the role of sodium acetate as a buffer solution and explain how it can maintain a stable pH.
Sodium acetate is commonly used as a buffer solution due to the equilibrium between the acetate ion (CH3COO-) and acetic acid (CH3COOH). When small amounts of acid or base are added to a sodium acetate solution, the buffer system resists changes in pH by shifting the equilibrium to neutralize the added acid or base. This is because the acetate ion can accept protons from added acid, forming acetic acid, or donate protons to added base, forming water. This buffering capacity allows sodium acetate solutions to maintain a relatively stable pH, making them useful in various applications where pH control is important, such as in biological systems or in the food industry.
Evaluate the importance of understanding the hydrolysis of salts, such as sodium acetate, in the context of chemistry and its real-world applications.
Understanding the hydrolysis of salts, like sodium acetate, is crucial in chemistry because it helps explain the behavior of various compounds in aqueous solutions and their impact on pH. The ability to predict the acidic or basic nature of salt solutions is essential for many applications, such as in the formulation of buffer solutions, the preservation of food products, and the control of pH in biological systems. By comprehending the principles of salt hydrolysis, chemists can design and manipulate solutions to achieve desired pH levels, optimize reaction conditions, and develop effective strategies for various industries and research areas. This knowledge is fundamental for understanding the broader implications of chemical equilibria and their practical relevance in the real world.