A solution is prepared by adding 0.10 mol of ammonium chloride, NH4Cl, to 1.00 L of water.  Which statement about the solution is correct? A. The solution is neutral B. The solution is basic C. The Ka for the species in solution must be known before a prediction can be made D. The Kb for the species in solution must be known before a prediction can be made E. The solution is acidic

Q: Determine whether each salt forms an acidic, basic, or neutral solution when it dissolves in water.…

A: I am instructed to answer only three subparts please to repost for the rest.

Q: What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF? Select…

A: Percent ionization is a measure of the strength of an acid. The value of percent ionization of a…

Q: Which one of the following 0.1 M aqueous solutions has pH = 7?   A.  NH4NO3   B.  NaClO4   C.…

A: pH of 7 will only be given by a neutral solution.

Q: At a certain temperature the Ka for the hydrogen sulfite ion, HSO," is 6.2 × 10⁹. Which of the…

A: Given,the molarity of NaHSO3 = 0.100 mol.L-1Ka = 6.2 x 10-8

Q: 22. A solution for which [OH-] = 3.0 x 10-10 is classified as a. acidic b. basic c. neutral

A: Given, [OH-] = 3.0 x 10-10 pOH = -log [OH-] pOH = -log[3.0 x 10-10] pOH = 9.52

Q: The molar concentration of H+ ions in a solution is 5.8 x 10-9. The pH is a. 9.00 b. 5.80 c.…

A: pH can be calculated as pH = -log [H+]

Q: For each strong base solution, determine [OH-], [H3O+], pH, and pOH.a. 0.15 M NaOH b. 1.5 * 10-3 M…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

Q: A 0.1 M solution of has a pH = 7.0 A. KF B. NaF C. NANO3 D. Na2S E. NH4CI

A: The given pH of the salt solution is 7.0, which is neutral. Thus, the salt which upon hydrolysis…

Q: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

Q: Identify the conjugate acid and conjugate base of the following acids and bases. Then, write the…

A: e.

Q: 8. Calculate the pH for each of the following solutions from the information given. a. [H]=4.78 x…

A: Since you have posted a question with multiple sub-parts, we will provide the solution only to the…

Q: a. A solution of HINO, has a pH of 3.57. What is the molarity of the solution? Molarity = M b. A…

A: pH = -log[H+]  Log [H+] = -pH  [H+] = 10-pH

Q: 1. What is the pH of 0.25L of chicken soup? How about 0.5L? Is it acidic or basic? 2. Does the pH…

A:

Q: A week diprotic acid H2A has Ka1 = 4.2 × 10–7 and Ka2 = 4.8 × 10–11. Determine the pH of a 0.17 M…

A: Ka1 = 4.2 × 10–7     pKa1 = 6.376 and Ka2 = 4.8 × 10–11    pKa2 = 10.319

Q: 5. Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCOOH b. 0.185 M in HCOOH…

A: A measure of how acidic or basic a substance or solution is. pH is measured on a scale of 0 to 14.…

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.