What is the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution co

step 1 Let's first figure out what the initial pH is when we have a buffer solution that is .169 molar

What is the pH change when 20.0 mL of 0.100 M NaOH is added...

What is the $\mathrm{pH}$ change when $20.0 \mathrm{~mL}$ of $0.100 \mathrm{M}$ $\mathrm{NaOH}$ is added to $80.0 \mathrm{~mL}$ of a buffer solution consisting of $0.169 \mathrm{M} \mathrm{NH}_3$ and $0.183 \mathrm{M} \mathrm{NH}_4 \mathrm{Cl}$ ?

Key Concepts

Buffer Solutions

Buffer solutions are mixtures that consist of a weak acid and its conjugate base, or a weak base and its conjugate acid. They resist changes in pH upon the addition of small amounts of acids or bases by shifting the equilibrium between the two components, thereby maintaining a relatively constant pH.

Henderson–Hasselbalch Equation

The Henderson–Hasselbalch equation is a mathematical formula that relates the pH of a buffer solution to the pKa of the acid and the ratio of the concentrations of the conjugate base and acid. It simplifies the calculation of the pH of buffer solutions after changes in composition due to added acid or base.

Acid–Base Neutralization in Buffers

When a strong acid or base is added to a buffer, it reacts preferentially with either the conjugate base or acid, respectively. This neutralization reaction alters the ratio of the buffer components, which, while still maintaining some buffering capacity, results in a change in the pH of the solution.

Stoichiometry in Titrations

Stoichiometry in titrations involves calculating the amounts of reactants and products based on their molar relationships during chemical reactions. In the context of buffer solutions, it is used to determine how an added volume of titrant, such as a strong base or acid, will alter the concentrations of the buffer components and, consequently, the pH.

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