(a) Cu²+ + 4Cl CuCl? (b) Al(OH)3 + 3HNO3 Al³* + 3H,0 + 3NO3 (c) N2 + 3H2 = (d) CN¯ + H2O 2NH3 HCN + OH

Q: Phenylacetic acid (C6H5CH2COOH, simplified here as HPAc) builds up in the blood of persons with…

A: Answer: Given data: pH=2.62α=0.02C=0.12M

Q: Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?

A: Brønsted -Lowry acids or proton donors are the species, that can transfer the proton to another…

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: Calculate the pH of a solution (aq., 25 oC) when 25.00 mL of 0.250 M KOH is added to 25.00 mL of…

A: Answer :-  pH = 4.20  The pH of a solution, when 25.00 mL of 0.250 M KOH is added to 25.00 mL of…

Q: I'm not sure how to solve this.

A: First the equilibrium concentration of H3PO4 is determined.

Q: 27G. A solution that is 0.010 M of the salt triethanolammonium bromide, (CaH,ONHJBr. (Kb, (CsH9OsN)…

A: Nature of salt: 1. If a salt is made by reacting strong base and strong acid then it's nature would…

Q: (a) Is a weak Brønsted-Lowry base necessarily a weak Lewis base? Explain with an example.(b)…

A: (A). Bronsted -Lowry base: The substances which have a tendency to attract the proton are called…

Q: Which of the following has the highest acidity: pH 1, pH 5, or pH 9?

A: To find: Which pH has the highest acidity

Q: Why is (CH3)3Cl considered to be a Lewis Acid?

A: The Lewis concept of acid and bases is the most accepted definition which is used to explain the…

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: Rank the compounds in each of the following groups in order of increasing acidity or basicity, as…

A: (a)

Q: Which of the following species is not a Brønsted-Lowry base? Multinle Cho ice

A: According to Bronsted-Lowry acid is a substance which can give up a proton (H+) while base is a…

Q: Name the corresponding salts of organic acids: (HCOO)2Ca; CH3CH2COOK.

A: Organic salts are salts containing organic ion.  Rules -  In any salt there are two ions present…

Q: The concentration of OH- in a solution of householdbleach is 3.6 × 10-2 M. Calculate the pH of the…

A: Given here the Concentration of OH- in a solution [OH-] = 3.6 ×10-2 M . we are asked to calculate…

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 following diagrams represent aqueous solutions of twomonoprotic acids, HA (A = X or Y). The…

A: a) Since the stronger acid will produce more number of H3O+ ions in the solution  Hence the acid…

Q: equilibrium. You can leave out water self Write the chemical formulas of the species that wil act as…

A: Salt of Strong base and weak acid is acidic and strong base and weak acidic is basic

Q: Which of these may be classified as an Arrhenius base in aqueous solution? О НСІ O CSOH O AgNO3 O…

A: An Arrhenius base is a compound when ionizes in an aqueous solution to produce hydroxide ions (OH-).…

Q: The pH of 0.01 m Potassium hydrogen phthalate is

A:

Q: In a solution of 0.015 mol L-1 HBr(aq) at 25 °C (a) What are the concentrations of the hydronium,…

A: pH stands for the potential of hydrogen ion concentration or power of hydrogen. The pH of an aqueous…

Q: Rank the compounds in each of the following groups in order of increasing acidity or basicity, as…

A: a) HCl < HBr < HI  b) H2O < Cl- < OH- < H-

Q: Given the following acids and K, values: HCIO, HOAC HCN HF Ix 10 1.76 x 105 4.93 x 10-10 3.53 x 10…

A: Given HClO4 = 1×107 HOAc = 1.76×10-5 HCN = 4.93×10-10 HF  = 3.53×10-4

Q: 7. Which of the following species can act both as an acid and a base? a) b) HNO, c) H,SO, d) H,CO,…

A: Since you have asked multiple questions,we will solve the first question for you.If you want any…

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

A:

Q: Using Brønsted-Lowry definitions, designate each of the following as a strong base (SB), a weak base…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: Calculate the molarity of an phosphoricacid (H3PO4) solution if 75.00 mL is completely neutralized…

A:

Q: A 75.00-mL portion of a solution that is 0.0460 M in HClO4 is treated with 150.00 mL of 0.0230 M…

A: Acid reacts with base to form salt and water. The given acid is HClO4 and base is KOH.

Q: 16.110 Arrange the following 0.10 M solutions in order of increas- ing acidity: (i) NH,NO3, (ii)…

A: The salt hydrolysis can be explained as the reaction in which the acidic solution is generated if…

Q: 6.7 x 10, What is the pH of A solution at 25 °C has [OH] = the solution?

A: Number 1 :- Given :- [OH-] = 6.7 × 10-3  To calculate :- pH of solution

Q: Arrange the substances based on their relative acid strength. CIO C,H,0, strongest acid C,H,CO0…

A: Strong acids are those which dissociate rapidly in water to gibe H+ ions. The dissociation of these…

Q: Carbonic acid, H,CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 x 10-1". What is the pH…

A:

Q: 9. The base ionization constant K, describes which of the following reactions for a weak base, B, in…

A: Base dissociation constant ( Kb ) is the equilibrium constant that refers to the ionisation or…

Q: Citric acid, which is present in citrus fruits, is a triprotic acid Is the concentration of citrate…

A: To find: Whether citrate ion is equal to, less than or greater than the H+ ion concentration.

Q: Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid,…

A: According to the Brønsted-Lowry concept :-  An acid is a proton donor  A base is a proton acceptor

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: NH3 is a weak base (?b=1.8×10−5Kb=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

A:

Q: The methoxide ion, CH₃O⁻, and amide ion, NH₂⁻, arevery strong bases that are “leveled” by water.…

A: Methanol has the conjugate base called CH3O- ion whereas NH2- ion is the conjugate base of ammonia.…

Q: Aluminum hydroxide is an amphoteric substance. It can act either as a Brønsted-Lowry base or a Lewis…

A: Aluminium hydroxide is amphoteric in nature. In acids, it acts as a Bronsted- Lowry base .It…

Q: Lemon juice has a pH of about 2. What [H3O+] is this?

A: Given that the pH of lemon juice is 2. To calculate the concentration of H3O+ ions in the lemon…

Q: Calculate the pH of a solution (aq., 25 oC) when 50.00 mL of 0.150 M HClO4 is added to 30.00 mL of…

A: Normality = n factor * Molarity  for HClO4 , n factor =1  for Ba(OH)2 , n factor =2

Q: Which one of the following 0.1 M aqueous solutions has pH = 7? OA. NaF O B. NHẠNO3 O C. NaHSO, D.…

A: pH is defined as the negative logarithm of the H+ion concentration.                       pH =…

Q: If the normal physiological concentration of HCO3- is 24 mM, what is the pH of blood if PCO2 drops…

A: pH = 7.45

Q: The hydronium ion concentration of an aqueous solution of 0.558 M isoquinoline (a weak base with the…

A:

Q: When SO2 dissolves in water to form sulfurous acid, H2SO3(aq), that acidcan donate a hydrogen ion to…

A: The balanced equation will be,SO2 (aq) + H2O (aq) → H2SO3  (aq) A Bronsted acid can donate a proton…

Q: A truck transported 400 liters of HCl approximately 7.4M a) Is it a strong or weak acid? b) What is…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: 15D.5. What is the difference between (a) monoprotic acid and a diprotic acid, (b) a weak acid and a…

A: Since you have posted a question with multiple subparts, we can only first three subparts. To get…

Q: The hydroxide ion concentration of an aqueous solution of 0.532 M phenol (a weak acid), C,H;OH, is…

A:

Q: Which of the following cannot be used to measure the pH of a solution?

A: a] a . PH meter is used to measure the PH of a solution           where the hydrogen activity (…

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.