Calculate the pH to two decimal places of each of the following solutions at 25 °C for which the substances ionize completely: (a) 0.161 M HCl

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

A: A weak acid are those which does not completely dissociate to liberate H+ ion

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

A:

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

A:

Q: Write the formula for the conjugate base of each of the following acids. а. Н.СО, b. HCO; c. NH,* d.…

A:

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: 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 hydronium ion concentration of vinegar is approximately 4 × 10−3 M. What are the corresponding…

A: Given : hydronium ion concentration i.e [H3O+ ] = 4 X 10-3 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: 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: 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: 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: 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 an aqueous solution of 0.522 M benzoic acid, C6H5COOH is

A:

Q: For the reaction of C5H5N with water, write the base ionization constant expression.

A: we have to write the expression for  base ionization constant for reaction of C5H5N with water

Q: pH of an aqueous solution of 0.355 M acetylsalicylic acid (aspirin) , HC9H7O4, is .

A:

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

A:

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: If the pH of a solution of aluminum hydroxide is 9.85, what is the concentration of the aluminum…

A: Since the aluminium hydroxide completely dissociates. Hence the dissociation reaction will be…

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: A 0.015M solution of cyanic acid has a pH of 2.67. Calculate the ionization constant, Ka, of the…

A: Given: Concentration of Cyanic acid(HCN) solution = 0.015 M pH = 2.67

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 an aqueous KOH solution is 12.38. What is the hydrogen ion concentration of this solution?

A:

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

A: Given solutions, (a) 0.000259 M HClO4(b) 0.21 M NaOH(c) 0.000071 M Ba(OH)2(d) 2.5 M KOH

Q: White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white vinegar is…

A:

Q: By what factor does 3H+4 change for a pH change of 0.50 units?

A: The pH of a solution is related to the concentration of H+ as follows: pH=-log [H+][H+]=10-pH

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 0.144 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: 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: 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: 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: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

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

A: Answer:- This question is answered by using the simple concept of calculation of initial…

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.