e acid (A), the base (B), the conjugate acid (CA

Q: Which would be a stronger Lewis acid, explain.   (a) BF3 or BCl3 (b) Fe2+ or Fe3+

A:

Q: The pH of a solution is defined as the negative logarithm of the molar concentration of hydrogen…

A: Given:  pH = -log[H+]  [H+] = 10-pH  For pure water , pH = 7  For HCl , pH = 1  [H+] for water =…

Q: Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

A: Conjugate pairs are acids and bases that differ only by a proton (H+).

Q: The pH of a 0.0039 M solution of Ca(OH), is

A: Provided concentration 0.0039M One Ca(OH)2 gives two OH-  So, 1 M Ca(OH)2 gives= 2M Ca(OH)2 Hence,…

Q: 12.9 g of NaOH was dissolved in water affording a final volume of 250 mL. What is the pH of the…

A: Given :-  mass of NaOH = 12.9 g  volume of solution = 250 mL  To calculate :-  pH of solution

Q: Calculate the pH and % ionization for a .44 molar solution of CN-(aq).

A: Cyanide ion hydrolyzes in water to form HCN and hydroxide ion. The concentration of hydroxide ion…

Q: Which of the following is a strong acid? (a) KHSO4(aq)           (b) HClO4(aq)             (c)…

A: Strong acids dissociate completely in aqueous solution, while weak acids partially or incompletely…

Q: The value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of K,, for its conjugate…

A: In this question given ka is 10-10 Kw=ka×kb

Q: The pH of an aqueous solution of 0.528 M benzoic acid , C,H;COOH is

A: Benzoic acid is a weak organic acid. It does not dissociates completely rather maintains equilibrium…

Q: Predict whether the solution NH,CN (aq) is acidic, basic, or neutral, and explain the basis of your…

A: NH4CN is a salt which is made by neutralisation reaction between an acid and a base.

Q: The pH of an aqueous solution of 4.45x102 M ammonium bromide, NH,Br (aq), is This solution is

A: NH4Br is a salt of weak base and strong acid. We have to determine pH of an aqueous solution of…

Q: Determine the percent ionization of the following solutions of phenol at 25°C: (a) 0.821 M (b) 0.360…

A:

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: 16.20 (a) Write an equation for the reaction in which H,C,H,O5 (aq) acts as a base in H20(1). (b)…

A: According to Bronsted acid-base  theory, An acid is a substance which can donate a proton to other…

Q: Which of the following salts (ionic compounds) forms an acidic solution in an aqueous solution?…

A: When a ionic compound is dissolved in water, and solution gets acidic means, ionic compound is…

Q: Calculate the pH and the pOH of each of the following solutions at 25°C for which the substances…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: NH3 is considered to be.  (a) amphiprotic (b)an Arrhenius base only (c)bronsted- Lowry base only

A: Amphiprotic substances are those substances which can act as both acid and base depending on the…

Q: provide reasonin

A: The reaction of HCl with alkenes results in the addition reactions. The addition of the HCl to the…

Q: alculate the pH of a solution that is (a) 1.50 x 10^-1 M NaOCl (b) 1.50 x 10^-2 M NaOCl (c) 1.50 x…

A: To calculate the pH of following :(a) 1.50 x 10^-1 M NaOCl (b) 1.50 x 10^-2 M NaOCl(c) 1.50 x 10^-4…

Q: An important step in many industrial processes is the slaking of lime, in which water is added to…

A: Lewis theory of Acids and Bases:- Lewis Acid- The electron pair acceptor substance is called as…

Q: 2.3 7 (a) Describe what happens when each of the following molecules is separately dissolved in…

A: A question based on equilibrium concept. 3 subdivision questions are given that are to be answered…

Q: As the pH of a solution increases (gets higher), what happens to the acidity of the solution?(a) The…

A: pH is defined for measure of free hydrogen ions or hydroxyl ions present.

Q: Give the formula for the conjugate acid of each species: (a) H₂O; (b) I; (c) HCO3. (a) (b) (c)

A: Acid and Base:• Acid: acids are proton (H+) donor.• Base: bases are proton (H+) acceptor.2)…

Q: Consider the following reaction: HF(aq) + NH3(aq) 2 NH4*(aq) + F'(aq) In this reaction NH4*(aq) is:…

A:

Q: Which of the following is false regarding the reaction below? H2SO3(aq) + H20(1) – HSO3 (aq) +…

A:

Q: The pH of an aqueous solution of 0.325 M hydrocyanic acid is

A: The concentration of hydrocyanic acid (HCN) = 0.325 M Ka of hydrocyanic acid = 6.2×10−10

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.