I'll give you 100%rating if you answer all questions. They are interconnected with each other that's why I can't post them separately Once upon a time, Rasmus and her brother Simone are doing titration to assess the molarity of the sample's total acid content. Using the pH measurements to report acidity, they were ordered to study a clear aqueous solution of an unknown monoprotic acid. They decided to use two methods of experiments to gather essential data for their Chemistry Class. The first method is through a pH strip. To estimate the pH of the sample, Rasmus used a pH strip. Rasmus collected 1 mL of the sample, which came out to have a pH of around 3.3. Furthermore, Rasmus made a new setup in which 1 mL of the same sample was diluted with 9 mL of water, and the pH taken was now around 3.8. The second method is Titration, and Simone used this method. Simone prepared a 10 mL aliquot of the sample and diluted it with 25mL of distilled water. After this, Simone added 2 drops of phenolphthalein, and it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint. Using the data in the titration method, compute the molarity of the acid. Predict the pH of the sample, assuming that the titrated unknown is a strong acid. Calculate the [H+] concentration in the sample before dilution using the values from the pH strip method. Comparing the results from the two methods, deduce if the unknown is really a strong acid, or if it’s a weak acid. Defend in one sentence. Rationalize the two pH readings in the pH strip test before and after dilution. Is this to be expected?
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
I'll give you 100%rating if you answer all questions. They are interconnected with each other that's why I can't post them separately
Once upon a time, Rasmus and her brother Simone are doing titration to assess the molarity of the sample's total acid content. Using the pH measurements to report acidity, they were ordered to study a clear aqueous solution of an unknown monoprotic acid.
They decided to use two methods of experiments to gather essential data for their Chemistry Class.
The first method is through a pH strip. To estimate the pH of the sample, Rasmus used a pH strip. Rasmus collected 1 mL of the sample, which came out to have a pH of around 3.3. Furthermore, Rasmus made a new setup in which 1 mL of the same sample was diluted with 9 mL of water, and the pH taken was now around 3.8.
The second method is Titration, and Simone used this method. Simone prepared a 10 mL aliquot of the sample and diluted it with 25mL of distilled water. After this, Simone added 2 drops of phenolphthalein, and it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.
- Using the data in the titration method, compute the molarity of the acid.
- Predict the pH of the sample, assuming that the titrated unknown is a strong acid.
- Calculate the [H+] concentration in the sample before dilution using the values from the pH strip method.
- Comparing the results from the two methods, deduce if the unknown is really a strong acid, or if it’s a weak acid. Defend in one sentence.
- Rationalize the two pH readings in the pH strip test before and after dilution. Is this to be expected?
Step by step
Solved in 4 steps
