Write the formula for the conjugate acid for each of the following bases:
c. H₂PO₄^-

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Identify the base provided in the problem. In this case, the base is the dihydrogen phosphate ion, represented as

H_{2} {PO}_{4} -

Recall the definition of a conjugate acid. A conjugate acid is formed when a base accepts a proton (H⁺).

Add a proton (H⁺) to the base. This involves increasing the number of hydrogen atoms in the formula by one and adjusting the charge accordingly. The formula becomes

H_{3} {PO}_{4}

Verify the charge of the conjugate acid. Since the base

H_{2} {PO}_{4} -

has a charge of -1, adding a proton (H⁺) neutralizes this charge, resulting in a neutral molecule.

Write the final formula for the conjugate acid, which is

H_{3} {PO}_{4}

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Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two species that differ by the presence or absence of a proton (H⁺). When a base accepts a proton, it forms its conjugate acid. Understanding this relationship is crucial for identifying the conjugate acid of a given base, as it directly influences the acid-base equilibrium in chemical reactions.

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Base Pairing Concept 1

Phosphate Ion Chemistry

Phosphate ions, such as H₂PO₄⁻, are part of a family of polyatomic ions that play significant roles in biological systems and chemical reactions. The H₂PO₄⁻ ion is the dihydrogen phosphate ion, which can act as a weak acid or a base. Recognizing its structure and behavior is essential for determining its conjugate acid when it gains a proton.

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Polyatomic Ions

Protonation Process

Protonation is the process by which a molecule or ion gains a proton (H⁺), resulting in the formation of a conjugate acid. This process is fundamental in acid-base chemistry, as it alters the charge and reactivity of the species involved. Understanding how protonation affects the properties of ions like H₂PO₄⁻ is key to predicting the resulting conjugate acid.

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