The pH of an aqueous solution of 8.08×10 M sodium hypochlorite, NaCIO (aq), is This solution is

Q: Calculate the pH of the following acid or base: 1. 3.6x10 M HNO,

A: pH stands for hydrogen potential in a solution. Low pH (less than 7.0) - Acidic pH  pH = 7.0 -…

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: The pH of a 0.0081 M solution of HNO₃ is

A: Given values-> [HNO3] = 0.0081M HNO3 ---> H^+ + NO3^- [H^+] = 0.0081M pH =-log [H^+] =…

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: The pH of a 0.225 M weak acid solution, HA, is 4.05, what is the K, of the acid?

A: pH = 4.05 pH = -log[H+] = 4.05 [H+] = 10-4.05          = 8.91 * 10-5 M

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: Consider two solutions, solution A and solution B. 3H+4 in solution A is 250 times greater than that…

A: A solution has pHA  = - log [HA +]  and [HA +] is the concentration of Hydrogen in solution A . B…

Q: Write the formula for the conjugate acid of each of the following bases: (a) HS¯, (b) HCO,, (c)…

A: Conjugate acid is the chemical species which is formed when a weak base accept a proton. For writing…

Q: What is the term used to describe the equilibrium constant for the autoionization of water?

A: An acid is a substance that gives  ions in its solution whereas a basic substance gives  ions in its…

Q: The pH of a 0.0030 M solution of Ca(OH), is

A:

Q: Calculate the pH of the solution, where the acetic acid is x10 stronger than acetate.

A: In chemistry, pH is defined as the potential of hydrogen ion. It is the negative logarithm of…

Q: If the molarity of an unknown substance is expressed as 3.7 x 10-5, what is the pH of the substance?

A:

Q: Calculate the pH of an aqueous solution of 0.0740 M potassium sulfite.

A:

Q: Calculate the pH of an aqueous solution of 0.1340 M potassium sulfite. pH = ||

A:

Q: The pH of an aqueous solution of 3.14×10-2 M ammonium chloride, NH4Cl (aq), is

A: NH4Cl is salt of weak base and strong acid

Q: The pH of a 0.70 mol/L weak base solution is 10.22. What is the Kb of the base?

A:

Q: The pH of an aqueous solution of 0.522 M benzoic acid, C6H5COOH is

A:

Q: How do I calculate pH of a salt? for example in 0.10 M NaClO4(aq)?

A: Salt are produced by the reaction of an acid and a base. For example, The pH of salt is given as :

Q: Write the formula of the conjugate base of HSO,

A: A conjugate acid is that which consists of one extra H-atom and also the positive charge than the…

Q: The ionization constant, K for HCN(aq) is 7.7 x 10 10, What is the pH of a 0.17 molar solution of…

A:

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

Q: calculate the concentration of H + in a solution of hypochlorous acid (I) of 1 mol / liter. In your…

A: Given is Solution of 1M hypochlorous acid. i.e. [HOCl] = 1 M We need to find concentration of [H+]…

Q: The pH of an aqueous solution is 5, what would be the pOH of this solutions

A: pH + pOH = 14

Q: The pH value of the 5L aqueous solution prepared with 6.4 grams of a precious strong acid is 2. So…

A: Given, volume of acid solution = 5L Mass of acid = 6.4 g PH = 2  Molar mass of acid = ?

Q: If a sample of a certain solution is determined to have a [H3O+] concentration of 5.6×10^−12…

A:

Q: The pH of an aqueous solution of 0.124 M ammonium nitrate, NH4NO3 (aq), is ___________. This…

A:

Q: The pH of an aqueous solution of 0.129 M potassium fluoride, KF (aq), is ____________. Therefore,…

A: PH of salt :   The solution is acidic, basic or neutral can be predicted as : If pH = 7, the…

Q: The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.

A: Since pKa for phenol is 9.98 and concentration of phenol is 0.508 M (given)

Q: The pH of an aqueous solution of 0.458 M pyridine (a weak base with the formula C5H5N) is ?

A:

Q: What is the pH of a solution prepared by dissolving 1.10 g of solid sodium hydroxide in 815 mL of…

A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration.    pH = -log[H3O+]…

Q: A solution is prepared by adding 0.0231 moles of H3O+ ions to 3.33L of water. What is the pH of this…

A: Given : moles of H3O+ ions = 0.0231 mol And volume of solution = volume of water approximately =…

Q: Write the formula of the conjugate base of CoHsSH.

A: Conjugate acid and conjugate base:

Q: The pOH of an aqueous solution of 0.423 M benzoic acid, C¿H;COOH is

A:

Q: The pH of an acidic solution is 6.75. What is pOH?

A:

Q: The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated…

A: [CH4N2O] = 1.00 M pH = 7.050 Calculating the [H3O+] from the given pH value, pH = -log[H3O+] [H3O+]…

Q: The pH of an aqueous solution of 0.470 M methylamine (a weak base with the formula CH3NH2) is

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: The pH of an aqueous solution of 0.144 M ammonium perchlorate, NH4ClO4 (aq), is . This solution is

A:

Q: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

A:

Q: A carbonated beverage was found to have a hydrogen ion concentration of 3.67x 104 mol/L. What are…

A:

Q: The pH of a solution of M(OH)2 is 13.08 .  What is the molarity of the M2+ ion?

A:

Q: The pH of an aqueous solution of 0.506 M benzoic acid , C6H5COOH is

A:

Q: The pH of an aqueous solution of 0.223 M ammonium bromide, NH,Br (aq), is This solution is

A: In this question, we want to determine first the pH of the aqueous solution of NH4Br(aq) and then…

Q: The ionization constant Ka, for HCN(aq) is 4.3 x 10^-10. What is the pH of a 0.22 molar solution of…

A:

Q: If a sample of a certain solution is determined to have a [H3O^+] concentration of 4.89×10^−1…

A: Given: [H3O+ ] = 4.89 × 10-1 M.

Q: The pOH of an aqueous solution of 0.468 M formic acid, HCOOH is _____  .

A:

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial…

A: Weak acid or base are those substance which does not dissociate 100%. The value of degree of…

Q: The pH of an aqueous solution of 0.176 M ammonium bromide, NH Br (aq), is This solution is

A: 1. Solution - According to the question - pH = pH stand for potential of hydrogen, since pH is…

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.