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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Chapter 3, Problem 14d

Balance the following equations: (d) KOH1aq2 + H3PO41aq2 ¡K3PO41aq2 + H2O1l2

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Identify the reactants and products in the chemical equation: Reactants are KOH and H_3PO_4, and products are K_3PO_4 and H_2O.
Write the unbalanced chemical equation: KOH + H_3PO_4 \rightarrow K_3PO_4 + H_2O.
Balance the potassium (K) atoms: There are 3 K atoms in K_3PO_4, so place a coefficient of 3 in front of KOH.
Balance the phosphate (PO_4) groups: There is 1 PO_4 group on both sides, so they are already balanced.
Balance the hydrogen (H) and oxygen (O) atoms: Adjust the coefficient of H_2O to balance the remaining H and O atoms.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Coefficients are used to adjust the number of molecules or formula units to achieve balance.
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Acid-Base Reactions

The reaction between KOH and H3PO4 is an example of an acid-base reaction, where KOH acts as a base and H3PO4 as an acid. In such reactions, the base donates hydroxide ions (OH-) while the acid donates protons (H+), leading to the formation of water and a salt. Understanding the properties of acids and bases is crucial for predicting the products of these reactions.
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Ionic Compounds and Solubility

The products of the reaction, K3PO4 and H2O, involve ionic compounds. K3PO4 is a soluble salt formed from potassium ions (K+) and phosphate ions (PO4^3-). Knowledge of solubility rules helps determine whether the products will remain in solution or precipitate out, which is important for understanding the overall reaction dynamics.
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