Answer to Question #339533 in General Chemistry for ann

Question

1. Write the hydrolysis reaction for pyridine. identify and define the Bronsted-Lowry acid and base.

2. Why is water considered a Bronsted-Lowry base in the reaction between water and HCI?

3.Define pH and explain how it is related to pOH.

4. The measured pH of the H2SO4 solution in water is 1.8. Calculate the volume of water needed to add to 1.00 L of this solution to increase the pH to 2.55 (The pH scale problem)

5. Determine the concentrations of the hydronium ion in pure water at 50 C if the ion-product of water at 50 C is 3.0x 10^13 ( the acid base properties of water problem )

Answer 1

Because water accepts a proton from HClstart text, H, C, l, end text, water is acting as a Brønsted-Lowry base. When water accepts a proton, H 3 O + \text{H}_3\text{O}^+ H3O+start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript is formed.

pH refers to the “potential of hydrogen”. It can be used to determine whether a solution is acidic, basic or neutral. In contrast, pOH is a measure of hydroxide ion (OH–) concentration. The key difference between pH and pOH is that pH is a measure of hydrogen ions whereas pOH is a measure of hydroxide ions.