What is the % ionization of a 1.19e-3 M H2S? See reaction below H2S + H2O ↔ HS- + H3O+ Ka = 9.100x10-8

Q: Consider a weak acid "HA". What is the pH of a 0.626 mol L¯' solution of HA? The KA of HA is 6.5 x…

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Q: (a) Calculate the percent ionization of 0.00310 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b)…

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Q: Find the H3O+ concentration of a 0.290 M hypochlorous acid solution (whose acid dissociation…

A: We are givenconcentration of hypochlorous acid = 0.290 MKa = 2.9x10-8We need to calculate the…

Q: Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a…

A: An acid is a species that can donate an H+ ion.The conjugate base of an acid should have one less H…

Q: Consider the weak bases below and their Kö values: C6H₂O CH;NH, C,H,N Kb = 1.3 x 10-10 Kb = 5.6 x…

A: As we know,  Greater is the dissociation constant of the base (Kb), greater is the tendency of base…

Q: What is the pH of a 2.4 M solution of H2CO3? (Ka of H2CO3 = 4.3 x 10-7, Ka of HCO3- = 7x 10-11)

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Q: Which of the following represents the reaction of the weak base, CH3COO", in water? CH3COO + H₂O…

A: Strong acid or base are those which can get completely ionized in water. Weak acid or base ionizes…

Q: 2.69 Label the Lewis acid and Lewis base in each reaction. Use curved arrows to show the movement of…

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Q: What is the % ionization of a 1.72e-4 M HBrO? See reaction below HBrO + H2O ↔ BrO- + H3O+ Ka =…

A: Interpretation -  To determine the % ionization of a 1.72e-4 M HBrO, For given reaction -…

Q: Calculate [OH-] of NaClO, 0.110M; KaHClO = 3.0 x 10-8.

A: Given: Concentration of NaClO is 0.110 M Ka (HClO) is 3.0×10-8 To determine: [OH-]

Q: Part A Find [H3O]* at equilibrium of a 0.110 mol ·L' solution of a weak monoprotic acid (HA) with Ka…

A: (A) Given: The dissociation of HA is written as follows: HA(aq)+H2O(l)------>H3O+(aq) + A-(aq).…

Q: What is the [OH-] (molarity) of a 0.1383 M methylamine? See reaction below CH3NH2 + H2O ↔ CH3NH3+ +…

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Q: ind the p H of a 0.291 M N a A solution. The salt completely dissociates into N aplusand Aminus. N a…

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Q: Calculate the pH and fraction of dissociation (a) for each of the acetic acid (CH3COOH, pKa = 4.756)…

A: We have to calculate PH and fraction of dissociation for acetic acid having PKa = 4.756 A) 0.00221M…

Q: Phosphoric acid, H3PO4, is a triprotic acid, for which Ka1 = 7.2 × 10-3, Ka2 = 6.3 × 10-8 and Ka3 =…

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Q: Determine [H30*] of a 0.250 M solution of formic acid (Ka 1.8 x 10-4).

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Q: What is the concentration of OH- in 0.1863 M HNO2 ?

A: Given :- initial concentration of HNO2 = 0.1863 M  ka = 4.600 × 10-4  To calculate :- [OH-]

Q: Calculate and contrast [OH-] in 0.200 M LIOH and 0.200 M NH3 (K₂ = 1.76 × 10-5).

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Q: Determine the concentration of carbonate, CO3-2, of a 0.18 M H2CO3 solution. Carbonic acid is a…

A: H2CO3 is a weak acid which donates its proton in the solution by step wise manner and the reaction…

Q: What is the [H3O+] of a solution which is 0.1690 M in CH3CO2H and 0.1590 M in NaCH3CO2? CH3CO2H(aq)…

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

Q: For the diprotic weak acid H₂A, Kal = 2.8 × 10-º and K₁2 = 7.5 × 10-⁹. What is the pH of a 0.0650 M…

A: we have to calculate the pH of weak diprotic acid

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.