What's your Laboratory observations using a 10ml graduate cylinder measure 10.0ml of the acid solution and transfer the solution to a 125ml Erlenmeyer flask. Add 2-3 drops of phenolphthalein and titrate to the end point (light pink) with a standardized sodium hydrogen carbonate solutions.
The laboratory procedure described involves measuring and transferring a 10.0 ml acid solution using a 10 ml graduate cylinder into a 125 ml Erlenmeyer flask.
After transferring the acid solution, 2-3 drops of phenolphthalein are added to the flask. Phenolphthalein is commonly used as an indicator in acid-base titrations. It is colorless in acidic solutions and turns pink or magenta in basic solutions. In this case, it will help determine the endpoint of the titration reaction.
To titrate, a standardized sodium hydrogen carbonate solution is added gradually to the acid solution in the Erlenmeyer flask. Sodium hydrogen carbonate (also known as sodium bicarbonate or baking soda) is commonly used as a titrant in acid-base titrations. It reacts with acids and neutralizes them.
The titration continues until the endpoint is reached, which is indicated by the appearance of a light pink color due to phenolphthalein. This color change signifies that the acid has been neutralized by the sodium hydrogen carbonate solution.
Overall, this laboratory procedure allows for the measurement, transfer, and titration of an acid solution using a 10 ml graduate cylinder, 125 ml Erlenmeyer flask, phenolphthalein, and a standardized sodium hydrogen carbonate solution.