You add 50.0 mL of 0.100 M HCl to 50.0 mL of 0.100 M AgNO3. What are the final concentrations

step 1 In question 109, we need to know the KSP value for the precipitate that forms, this being silver

You add 50.0 mL of 0.100 M HCl to 50.0 mL of 0.100 M...

You add $50.0 \mathrm{~mL}$ of $0.100 M \mathrm{HCl}$ to $50.0 \mathrm{~mL}$ of $0.100 M$ $\mathrm{AgNO}_{3}$. What are the final concentrations of $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{Cl}^{-}$ in the solution?

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Key Concepts

Spectator Ions and Complete Ion Dissociation

Spectator ions are those that do not participate in the actual chemical reaction and remain unchanged in solution. In reactions involving strong electrolytes that dissociate completely, recognizing which ions are spectators is important in determining the net change in the solution's composition.

Dilution and Mixing of Solutions

When two solutions are combined, their volumes add together, causing the concentrations of dissolved species to change. Understanding dilution is essential for calculating the final concentration of ions after mixing different solutions.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows one to determine which reactant limits the reaction and how much of each product is formed, which is crucial in predicting the outcome of a reaction scenario.

Precipitation Reaction

A precipitation reaction occurs when two aqueous solutions react to form an insoluble solid, known as the precipitate. This process removes specific ions from solution, thereby affecting the overall ionic concentration in the final mixture.

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