To determine the concentration of the strong acid using the provided data, we can use the formula based on the titration principles:

$C_a \times V_a = C_b \times V_b$

where:

• $C_a$ is the concentration of the acid (unknown),
• $V_a$ is the volume of the acid (25.0 mL given),
• $C_b$ is the concentration of the base (1.0 M),
• $V_b$ is the volume of the base added at the equivalence point (25.2 mL).

Step-by-Step Solution:

1. Convert all volumes to liters:

   • Volume of acid, $V_a = 25.0 \, \text{mL} = 0.025 \, \text{L}$.
   • Volume of base, $V_b = 25.2 \, \text{mL} = 0.0252 \, \text{L}$.

2. Set up the equation: $C_a \times 0.025 = 1.0 \times 0.0252$

3. Solve for $C_a$: $C_a = \frac{1.0 \times 0.0252}{0.025} = 1.008 \, \text{M}$

Therefore, the concentration of the acid, $C_a$, is approximately $1.008 \, \text{M}$ or, rounded to three significant figures, $1.01 \, \text{M}$.

Would you like further details on this calculation, or do you have any additional questions?

Here are five related questions that build upon this problem:

1. How would the concentration of the acid change if the volume of the acid were different?
2. What would happen to the endpoint volume if a weaker base was used?
3. How would using a different indicator impact the titration process?
4. Why is it important to reach the equivalence point in a titration?
5. How does the pH change around the equivalence point in a strong acid-strong base titration?

Tip: Always ensure that units are consistent, especially in titration calculations where volumes should be in liters to match the molarity unit.