The pH of an aqueous solution of 0.393 M nitrous acid is

Q: Calculate the pH of weak acid HNO2 in .35M of aqueous solution.

A:

Q: Calculate the pH of the following solutions. 5.00 g of HBr in 100 mL of the aqueous solution

A: Given, mass of HBr = 5.00 g            volume of HBr = 100 mL Now, let us calculate the moles of…

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 0.413 M triethylamine (a weak base with the formula (C2H3)N) is

A: The value of base dissociation constant ,Kb, of ethylamine is 5.6 . 10-4  ethylamine is a weak base…

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 0.0068 M solution of Ca(OH)₂ is?

A: pH + pOH = 14 pOH = -log[OH-]

Q: Calculate the pH of an aqueous solution; 0.015 M KOH

A: Given: Concentration of KOH = [OH-] =  0.015 M

Q: The pH of an aqueous solution of 0.377 M triethylamine (a weak base with the formula (C2H5)3N) is

A:

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A:

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−], of 1.35×10−8 M.

A:

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A: Given Hydrogen ion concentration is [H+]=4.5×10-10M As we know, pH=-log[H+] pH=-log[4.5×10-10]use…

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

A:

Q: Calculate the pH of an aqueous solution that is 0.70 M sodium hypochlorite.

A: The given compound Sodium hypochlorite (NaClO) is a strong electrolyte. So, it dissociates…

Q: A solution of sulfuric acid (H2SO4) has a concentration of 0.0075 M. Calculate the pH of this…

A: Given, Concentration of H2SO4 solution = [H2SO4] =  0.0075 M pH of the solution = ? Note:  Sulfuric…

Q: Calculate the pH of an aqueous solution of 0.0448 M potassium sulfite.

A: PH is defined as negative logarithms of hydrogen ion concentration.

Q: Determine the pH of a solution that contains 6.5x10-3 mol/L of OH- ions

A: pH :- It is defined as the negative logarithm to the base 10 of hydronium ion concentration…

Q: Determine the pH and pOH of a solution at 30 degree Celsius that has 0.32 mols of hydroxyl ions in…

A: Acidity of solution can be calculated from the value of pH.  Now, pH of solution can be calculate…

Q: what is the pH of a 0.00761 molar solution of HNO3?

A: Nitric acid is a strong acid that dissociates completely in aqueous solution.

Q: The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39. What is the Ka of the acid?

A: pH is the universal indicator , that not only help in detecting the acidic/ basic character but also…

Q: The pH of an aqueous solution of 0.552 M triethylamine (a weak base with the formula (C2H5)3N) is

A:

Q: What is the pH of a 0.0050 M solution of hydrochloric acid?

A: The pH of a solution is calculated by,

Q: The hydronium-ion concentration of a solution is 7.0 × 10-6 M. What is the solution pH?

A: pH of the solution is =   -log [H+]

Q: what is the ph of a solution whose hydrogen ion concentration is 0.015?

A: As we know, HCl is a stong acid. It dissociates completely into H+ and Cl—in a chemical equation –

Q: The pH of a 0.0042 M solution of HNO is

A:

Q: Calculate of pH of a 0.0026 mol/L solution of hydrochloric acid

A:

Q: Calculate the pH of a solution that has [H 3O +] = 5.2 × 10 –7 M.

A: pH is the potential of the hydrogen which is usually used to predict how strong an acid is. The pH…

Q: Calculate the pH of an aqueous solution of 0.2100 M potassium sulfite. pH =

A:

Q: solution is made by dissolving 0.0699 mole of calcium hydroxide (Ca(OH)2) in 500 mL of water.…

A: Given: moles of calcium hydroxide Ca(OH)2 = 0.0699 mol Volume = 500mL = (500/1000)L = 0.5L Thus,…

Q: The pH of a 0.0047 M solution of HNO, is

A: As HNO3 is a strong acid, it completely ionises in the solution.

Q: The pH of an aqueous solution of 0.555 M methylamine (a weak base with the formula CH3NH2) is .

A: Here we have to determine the pH of 0.555M aqueous solution of CH3NH2 ,Kb (CH3NH2) = 4.47×10^-4 .

Q: Calculate the pH of an aqueous solution of 0.2100 M potassium carbonate. pH

A:

Q: The pH of a solution with a [OH–] concentration of 1.20 x10–6 M are___, respectively.

A:

Q: Determine the pH of a 1.00×10¯7 M aqueous solution of HBr.

A: Given : concentration of HBr solution = 1.00 × 10-7 M  To calculate :- pH of solution

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

A:

Q: Calculate the pH of the following solutions.  - 0.10 M pyridine

A:

Q: The pH of an aqueous solution of 0.430 M aniline (a weak base with the formula C,H-NH,) is

A:

Q: Calculate the pH of an aqueous solution of 0.141 M potassium sulfite. pH = .

A:

Q: Calculate the pH of an aqueous solution

A: Given :- concentration of sodium sulfite = 0.360 M  concentration of sodium hydrogen sulfite = 0.330…

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: The pH of a 0.0071 M solution of HNO3 is

A:

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: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A:

Q: Determine the pH of a 1.2 M solution of NaF. The K, of HF is 7.2 x 104.

A:

Q: The pH of a 0.0077 M solution of Ca(OH)₂ is?

A:

Q: Estimate the pH of a 0.016 M aqueous lead (II) chloride.

A:

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=2.1×10−7 M?

A:

Q: Calculate the pH of the following solutions 0.0040 M Ba(OH)2

A:

Q: The pH of an aqueous solution of 0.470 M hydrocyanic acid is

A: Given :- concentration of hydrocyanic acid = 0.470M  To be calculated :-  pH of solution  pH =…

Q: Determine the pH of an aqueous solution where [OH] = 6.0 x 10 10 M.

A: Given data : [OH-] = 6.0 × 10-10 M.  To find : pH

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.