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Chapter 2: Problem 13

\(A(n)\) _______ is a chemical partnership between a weak acid or base and its salt.

Short Answer

Expert verified
A buffer is a chemical partnership between a weak acid or base and its salt.

Step by step solution

01

Identify the Type of Chemical Partnership

A chemical partnership between a weak acid or base and its salt is typically referred to as a buffer. Buffers are important because they help maintain a stable pH in a solution even when small amounts of acid or base are added.
02

Recognize the Components

To clarify, a buffer is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. These components work together to resist changes in pH.
03

State the Answer

Given the explanation, the correct term to fill in the blank is 'buffer'. The partnership of a weak acid or base with its salt acts as a buffer to stabilize the pH levels in a solution.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Weak Acids
A weak acid is a type of acid that does not fully dissociate into its ions in an aqueous solution. This means that only a small percentage of the acid molecules release hydrogen ions (H鈦�) into the solution. Because of this partial dissociation, weak acids are not as effective at lowering the pH of a solution compared to strong acids, which fully dissociate.
  • Common examples of weak acids include acetic acid (found in vinegar) and citric acid (found in citrus fruits).
  • The equilibrium in a weak acid solution is described by the acid dissociation constant, known as \( K_a \).
The value of \( K_a \) indicates the strength of the weak acid; the smaller the \( K_a \), the weaker the acid. This characteristic allows weak acids to be part of a buffer system, as they provide a source of hydrogen ions to balance pH changes.
Exploring Weak Bases
In chemistry, a weak base is a base that does not fully ionize in solution. Like weak acids, they partially dissociate鈥攎eaning, they produce fewer hydroxide ions \((OH^鈭�)\) than a strong base, which fully dissociates in solution. This limited ion production results in a less drastic increase in pH when added to a solution.
  • Examples of weak bases include ammonia (\(NH_3\)) and methylamine.
  • The equilibrium constant for the reaction of a weak base with water is called the base dissociation constant, \(K_b\).
The \(K_b\) value gauges the base's strength: a smaller \(K_b\) indicates a weaker base. Weak bases play a crucial role in buffer solutions, where they help neutralize added acids by consuming excess hydrogen ions.
Concept of Conjugate Acid-Base Pairs
A conjugate acid-base pair consists of two species that differ by a single proton. When a weak acid donates a proton, it forms its conjugate base. Conversely, when a weak base accepts a proton, it forms its conjugate acid.
  • For example, in the case of acetic acid \((CH_3COOH)\), the conjugate base is acetate \((CH_3COO^鈭�)\).
  • In the ammonia system \((NH_3)\), its conjugate acid is ammonium \((NH_4^+)\).
These pairs are integral to the buffering action, as they allow the system to resist changes in pH. The weak acid-conjugate base or weak base-conjugate acid pair works together to neutralize added acids or bases, maintaining the solution's pH within a narrow range. This ability helps biological systems like blood plasma, maintain homeostasis.

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Most popular questions from this chapter

An ion is an atom that has _______ a. the same number of electrons and protons b. a different number of electrons and protons c. a and b are correct

Liquid water has _______. a. tracers b. a profusion of hydrogen bonds c. cohesion d. resistance to increases in temperature e. b through d f. all of the above

When dissolved in water, a(n) _______ donates \(\mathrm{H}^{+}\)

\(\mathrm{A}(\mathrm{n})\) _______ forms when atoms of two or more elements bond covalently.

Atoms share electrons unequally in a(n) _______ bond
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