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

Q: The pOH of an aqueous solution of 0.520 M acetic acid is

A: Given, Concentration of acetic acid (CH3COOH) solution = 0.520 M pOH of the solution = ? Note: Ka…

Q: Calculate the pH of a 0.13 M solution of propanoic acid. K, of propanoic acid is 1.3 x 10-5.

A: pH is defined as negative logarithm of hydrogen ion concentration.

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 an aqueous solution of 0.415 M aniline (a weak base with the formula C,H&NH,) is

A:

Q: The pH of an aqueous solution of 0.354 M hydrofluoric acid is

A: Hydrogen fluoride is a weak acid and its pKa value is = 3.17 The concentration of HF solution is =…

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 0.559 M caffeine (a weak base with the formula C3H10N402) is

A: Given, Caffeine (C8H10N4O2) is a weak base. Concentration of Caffeine solution (C) = 0.559 M pH of…

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

A:

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31.  What is the Ka of the acid?

A: Given  pH = 2.31 Concentration of acid = 1.86 M Ka =?

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

A:

Q: The pOH of a basic solution is 2.65. What is PH?

A: Given, the pOH of a basic solution, pOH =2.65we are asked to calculate the pH of the solution.

Q: The pH of a 0.550 M of weak base, A-,  is 9.93 at 25. What is the Kb of the base?

A: Since the base given is a weak base. Hence it will undergo partial ionisation as per the below…

Q: The pOH of an aqueous solution of 0.528 M hypochlorous acid is

A: Given :-  concentration of hypochlorous acid = 0.528 M  To calculate :-  pOH of solution    pH + pOH…

Q: An aqueous solution at 25 °C is 12.9% HNO, by mass and has a density of 1.049 g/mL. What is the pH…

A: Assuming we have 100 g of solution  hence mass of HNO3 in it = mass % X mass of solution / 100 =…

Q: The pOH of an aqueous solution of 0.587 M hypochlorous acid is

A: The given data is as follows: The concentration of hypochlorous acid = 0.587 M The pOH of the…

Q: The pH of an aqueous solution of 9.69×10- M ammonium chloride, NHĄC1 (aq), is This solution is

A: NH4Cl is a salt of strong acid (HCl) and weak base (NH3) hence pH this solution  is given by the…

Q: The pOH of a basic solution is 2.87. What is pH?

A: We have given that  pOH = 2.87  We know that  pH + pOH =14  pH = 14 - pOH        = 14 - 2.87   pH =…

Q: The pH of an aqueous solution of 0.353 M aniline (a weak base with the formula C¿H2NH,) is

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

Q: The pH and pOH of 0.05 M of NaOH is ..

A:

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

A:

Q: The pH of an aqueous solution of 0.236 M sodium cyanide, NaCN (aq), is This solution is acidic,…

A: NaCN is salt of strong base and and weak acid. The chemical nature of the solution depends on the…

Q: The pH of an aqueous solution of 0.529 M acetic acid is

A: Chemical formula of Acetic acid = CH3COOHAcetic acid is a monoprotic acid which dissociates as:

Q: The pOH of an aqueous solution of 0.598 M hypochlorous acid is

A: We have to find the pOH of given concentration of Hypochlorous acid

Q: The pH of an aqueous solution of 0.530 M methylamine (a weak base with the formula CH3NH2) is…

A:

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: If the pH is 1.4 what is the molarity?

A: We know that, pH is the negative logarithm of hydrogen ion concentration. i.e.,…

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

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 0.532 M nitrous acid is

A: The acid ionization constant, Ka represents the acid strength of a solution and the acid is stronger…

Q: The pH of an aqueous solution of 0.542 M triethylamine (a weak base with the formula (C₂H5)3N) is

A:

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

A:

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: If you measure the pH of a carbonic acid solution to be 5.6, what is the concenration of the H3O+ in…

A: pH of carbonic acid=  5.6[H3O+ ] = ?

Q: The pH of a 0.224 M solution of a weak acid, НВ, is 2.63. What is Ka for the weak acid?

A: Given:  A solution of weak, HB with concentration = 0.224 M pH = 2.63    Weak acid dissociates in…

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

A: Conjugate acid and conjugate base:

Q: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (K,)…

A: Given:   The concentration of acid HA is 0.185 M. The pH of the given acid is 2.95.

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

A:

Q: Provided that a chemist prepared a 1.00 M acetic acid solution (HC2H3O2) wherein he found out that…

A: The weak acids are those that partially dissociate in aqueous solution to give protons. The pH is…

Q: The pH of an aqueous solution of NaCN is 10.38. What is [CN-] in this solution?

A: NaCN is a salt of strong base (NaOH) and a weak acid (HCN). The solution is thus basic in nature.

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: An aqueous solution at 25 C is 110% HNO, by mass and has a density of 1.046 g/mlL. What is the pH of…

A: Molarity of a solution is the number of moles of solute present in 1 liter of solution. The pH scale…

Q: The pOH of an aqueous solution of 0.528 M acetic acid is

A: The solution is as follows:

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: What is the pH of an aqueous solution of 0.005 M C6H5O- at 298 K of the Ka for phenol at the given T…

A: Given: Concentration of C6H5O- = 0.005 M And Ka of C6H5OH = 1.0 × 10-10

Q: The pOH of an aqueous solution of 0.377 M acetic acid is

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 =…

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.