In reactions where acids give up H* ions, they are referred to as proton donors. Explain why

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: of  is added to  of a  solution of  is added to of a solution that is  in both  and we have to write…

Q: 0.292 M hydrochloric acid 0.292 M ammonia 0.584 M barium hydroxide 2.57 M lithium hydroxide 1.25 M…

A: Concentration of solution is defined in M   Correct option is 2.57 molar lithium hydroxide

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: The solutions given are,

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.3 × 10⁻⁵. What is [H⁺]?

A: Given: [OH- ] = 2.3 × 10-5 M

Q: You are given three solutions A, B and C with pH values 2, 10 and 13 respectively. Write which…

A: Given: Three solutions A, B and C with pH values 2, 10 and 13. The concentration of hydrogen ion is…

Q: The pH of rainwater in a polluted area was found to be 3.50. What is the hydrogen-ion concentration…

A: The given data : The pH of rainwater = 3.50 To determine = The concentration of hydrogen ions.

Q: The pH of a 0.551 M solution of sodium methanoate, HCOO°Nª*, is 8.75. Calculate K, for the…

A: Concentration of HCOO-Na+ = 0.551 M pH of the solution = 8.75

Q: You can obtain the pH of a 0.100 M HCl solution by assuming that all of the H3O+ ion comes from the…

A: HCl dissociates completely to its constituent ions as: Auto-ionization of Water: Self ionization of…

Q: The preparation of an aqueous solution is described in the table below. For this solution, write the…

A: Answer:Any specie that loses H+ ion its solution is called as Bronsted-Lowry acid and the specie…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: o simplify the measurement of the acidity or basicity of a solution, the pH (hydrogen potential)…

A: Given[H+] = 0.0000375 pH = To be determined

Q: der these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…

A: In a 0.1 M aqueous solution, the objective is to arrange the chemical species by raising pH. We'll…

Q: What is the relationship between the acid ionization constant for a weak acid ( Ka ) and the base…

A: Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

Q: Calculate the pH and pOH of the following solutions : 1- 0.01 M HBr 2- 0.00005 M HBr 3- 0.00002 M…

A: "To get remaining sub-parts solved please repost the complete question and mention the sub-parts to…

Q: What will happen if you add a small amount of KOH to a solution containing acetic acid and potassium…

A:

Q: The pOH of an aqueous solution at 25°C was found to be 13.00. The pH of this solution is The…

A: The solution is as follows :

Q: What is the [HF] in a solution with a pOH of 12.5? the answer is not listed 3.16 x 10:13 M 0.0316 M…

A:

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: In these question acid or base has been added into a solution and we have to find out the reaction…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 5.3 × 10⁻⁵. What is [H⁺]?

A: The sum of the concentration of hydroxide and hydronium ion is always 10-14. that means,…

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.