A volume of 10 ml of a strong acid solution of pH=2.0 are mixed with 990 ml of a buffer solution

step 1 So in this question, H plus after mixing, after mixing, mixing is equal to 10 a step up minus 2

A volume of 10 ml of a strong acid solution of pH=2.0 are...

A volume of $10 \mathrm{ml}$ of a strong acid solution of $\mathrm{pH}=2.0$ are mixed with $990 \mathrm{ml}$ of a buffer solution of $\mathrm{pH}=4.0$. The $\mathrm{pH}$ of the resulting solution will be
(a) $4.2$
(b) $6.0$
(c) $4.002$
(d) $4.0$

Key Concepts

pH and Hydrogen Ion Concentration

pH is a measure of the acidity of a solution, defined as the negative logarithm of the hydrogen ion concentration. This concept allows one to convert between pH and [H+], which is essential in understanding how addition or dilution of acid or base affects a solution's acidity.

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resist changes in pH when small amounts of strong acid or base are added. This property makes buffers crucial in maintaining a stable pH in many chemical and biological systems.

Buffer Capacity

Buffer capacity is a measure of a buffer's ability to neutralize added acid or base without a significant change in pH. It depends on the concentrations of the buffering agents; a higher concentration generally provides a greater capacity to maintain a stable pH when small amounts of strong acid or base are mixed in.

Dilution and Mixing Effects

When mixing solutions of differing pH values, particularly when one is a buffer, the overall change in pH is influenced by the relative volumes and concentrations of the components. Understanding dilution and the relative amounts of acid or base introduced is essential to predict the outcome of mixing, especially in buffered systems where the buffer components counteract the pH change.

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