To design an experiment that demonstrates the concepts of acid-base neutralization and calculates the molarity of an unknown acid solution with limited resources, you can perform a simple titration using a base of known concentration and some basic equipment. Here's a step-by-step guide for the experiment:Materials needed:1. Unknown acid solution2. Base solution with known concentration e.g., 0.1 M NaOH 3. Graduated cylinder or burette to measure volume 4. pH indicator e.g., phenolphthalein or pH paper5. Small beaker or Erlenmeyer flask6. Dropper or pipette7. Safety goggles and glovesProcedure:1. Put on your safety goggles and gloves to ensure safe handling of chemicals.2. Measure a specific volume e.g., 10 mL of the unknown acid solution using a graduated cylinder or pipette, and transfer it to the beaker or Erlenmeyer flask.3. Add 2-3 drops of phenolphthalein indicator or note the initial pH using pH paper.4. Fill the burette or another graduated cylinder with the base solution e.g., 0.1 M NaOH .5. Slowly add the base solution to the acid solution while stirring. Keep track of the volume of base added. If using phenolphthalein, the endpoint is reached when the solution turns faint pink and remains so for 30 seconds. If using pH paper, the endpoint is reached when the pH is around 7.6. Record the volume of base solution added to reach the endpoint.Calculations:1. Use the formula for titration: M1 V1 = M2 V2 , where M1 is the molarity of the acid, V1 is the volume of the acid, M2 is the molarity of the base, and V2 is the volume of the base.2. Rearrange the formula to solve for the molarity of the unknown acid: M1 = M2 V2 / V1.3. Plug in the values for M2, V2, and V1, and calculate the molarity of the unknown acid solution M1 .This experiment demonstrates the concept of acid-base neutralization, as the acid and base react to form water and a salt. Additionally, it allows you to calculate the molarity of the unknown acid solution using a simple titration method with limited resources.