Sure, here is the step-by-step explanation:

1. **Definition of Neutralization Reaction**: A neutralization reaction occurs when an acid and a base (alkali) react to form water and a salt. The general equation for this reaction is:
$$ \text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water} $$

2. **Initial pH of Alkali Solution**: An alkali solution has a pH greater than 7, indicating that it is basic. The higher the pH, the stronger the alkali.

3. **Addition of Acid**: When an acid is added to the alkali solution, the hydrogen ions ($ \text{H}^+ $) from the acid react with the hydroxide ions ($ \text{OH}^- $) from the alkali to form water ($ \text{H}_2\text{O} $).

4. **Reaction Process**: As the neutralization reaction proceeds, the concentration of hydroxide ions in the solution decreases because they are being used up to form water.

5. **Change in pH**: As the concentration of hydroxide ions decreases, the pH of the solution also decreases. This is because the solution is becoming less basic (or more neutral).

6. **Approaching Neutrality**: If enough acid is added to completely neutralize the alkali, the pH of the solution will approach 7, which is neutral. At this point, the amounts of hydrogen ions and hydroxide ions are equal, resulting in a neutral solution.

7. **Beyond Neutralization**: If excess acid is added beyond the point of neutralization, the solution will become acidic, and the pH will drop below 7.

In summary, during a neutralization reaction, the pH of an alkali solution decreases as the solution becomes less basic and moves towards neutrality. If the reaction continues beyond the neutral point, the solution can become acidic.

Question

Sure, here is the step-by-step explanation:

1. **Definition of Neutralization Reaction**: A neutralization reaction occurs when an acid and a base (alkali) react to form water and a salt. The general equation for this reaction is:
   $$ \text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water} $$

2. **Initial pH of Alkali Solution**: An alkali solution has a pH greater than 7, indicating that it is basic. The higher the pH, the stronger the alkali.

3. **Addition of Acid**: When an acid is added to the alkali solution, the hydrogen ions ($ \text{H}^+ $) from the acid react with the hydroxide ions ($ \text{OH}^- $) from the alkali to form water ($ \text{H}_2\text{O} $).

4. **Reaction Process**: As the neutralization reaction proceeds, the concentration of hydroxide ions in the solution decreases because they are being used up to form water.

5. **Change in pH**: As the concentration of hydroxide ions decreases, the pH of the solution also decreases. This is because the solution is becoming less basic (or more neutral).

6. **Approaching Neutrality**: If enough acid is added to completely neutralize the alkali, the pH of the solution will approach 7, which is neutral. At this point, the amounts of hydrogen ions and hydroxide ions are equal, resulting in a neutral solution.

7. **Beyond Neutralization**: If excess acid is added beyond the point of neutralization, the solution will become acidic, and the pH will drop below 7.

In summary, during a neutralization reaction, the pH of an alkali solution decreases as the solution becomes less basic and moves towards neutrality. If the reaction continues beyond the neutral point, the solution can become acidic.

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