what is the molarity of Cl^- in each solution? a. 0.200 M NaCl

Verified step by step guidance

1. Determine the dissociation of NaCl in water: NaCl (aq) \rightarrow Na^+ (aq) + Cl^- (aq)
2. Recognize that the stoichiometry of the dissociation shows a 1:1 ratio between NaCl and Cl^-
3. Understand that the initial concentration of NaCl is 0.200 M
4. Since the dissociation is 1:1, the concentration of Cl^- ions will be the same as the concentration of NaCl
5. Conclude that the molarity of Cl^- in the solution is equal to the initial molarity of NaCl, which is 0.200 M

Key Concepts

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (M). Understanding molarity is essential for calculating the concentration of ions in a solution, as it directly relates to the amount of solute dissolved in a given volume of solvent.

Dissociation of Ionic Compounds

Ionic compounds, such as sodium chloride (NaCl), dissociate into their constituent ions when dissolved in water. In the case of NaCl, it separates into Na⁺ and Cl^- ions. This dissociation is crucial for determining the concentration of specific ions, like Cl^-, in a solution based on the initial concentration of the ionic compound.

Stoichiometry of Solutions

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. In the context of solutions, it helps in calculating the amounts of ions produced from a given concentration of an ionic compound. For example, knowing that one mole of NaCl produces one mole of Cl^- allows for straightforward calculations of ion concentration from the molarity of the salt solution.