Acid Base perchloric acid HCIO, CIO, perchlorate ion sulfuric acid H2SO, HSO, hydrogen sulfate ion Undergo complete acid Do not hydrogen iodide undergo base HI iodide ion hydrogen bromide HBr ionization ionization Br bromide ion hydrogen chloride HCI in water in water Cr chloride ion nitric acid HNO3 NO, nitrate ion hydronium ion H20 water hydrogen sulfate ion HSO, so?- sulfate ion phosphoric acid H,PO4 H,PO, dihydrogen phosphate ion hydrogen fluoride HF fluoride ion nitrous acid HNO2 NO, nitrite ion CH;CO,H H,CO3 acetic acid CH,CO, acetate ion carbonic acid HCO5 hydrogen carbonate ion hydrogen sulfide H,S HS hydrogen sulfide ion ammonium ion NH HN3 ammonia hydrogen cyanide HCN CN cyanide ion hydrogen carbonate ion HCO, co- carbonate ion water H20 OH hydroxide ion hydrogen sulfide ion HS s2- sulfide ion Undergo complete base ionization ionization Do not ethanol C2H,OH C2H,O ethoxide ion undergo ammonia NH3 acid NH, amide ion hydrogen H2 in water H in water hydride ion methane CH4 CH, methide ion Figure 14.8 The chart shows the relative strengths of conjugate acid-base pairs. Increasing acid strength Increasing base strength

Q: Write a net ionic equation to show that hydrocyanic acid , HCN , behaves as an acid in water. + H20…

A: The answer to the following question is-

Q: aan EtAICI2 (Lewis acid)

A: Given reaction is Diels-Alder reaction. Diels-Alder reaction is [4+2] cycloaddition reaction.

Q: What is the equilibrium constant of the HSO4-ion, if [H3O+] = 0.027 M; [HSO−4] =0.29 M; and [SO2−4]…

A: The Complete and balanced chemical equation is given as,

Q: Calculate the pH for the following concentration: [H3O+] = 2.19 x 10-5 M.

A:

Q: Calculate the hydroxide ion concentration for a solution with (H3 O+)eq = 0.00004 M

A: Given hydronium ion concentration is = 0.00004 M

Q: Write the balanced equation for the following: Al(s) + NaOH(aq) + H2O(l)  ⇌ Na(Al(OH)4(aq) + H2(g)

A: A chemical reaction in which the elements present on the reactant side and product side are equal is…

Q: Complete the table. (All solutions are at 25 °C.) Solution [H3O+] [OH-] pH 1 3.19 2 3 4 3.2 x 10-9…

A:

Q: The reaction of ammonia with copper(II) ions is an example of a Lewis Acid–Lewis Base reaction.…

A:

Q: Predict the products from the following chemical reactions.   HNO3   +    Ba(OH)2

A:

Q: Arrange the oxides B2O3, Al2O3, BaO, CO2, Cl2O7, SO3 in order from the most acidic through…

A: In the periodic table in periods the electronegativity increased from left to right.In groups the…

Q: Calculate the H+] and pH of a 3.05 x 10¬4 M nitrous acid solution. The Ka of nitrous acid is 7.10 x…

A:

Q: Calculate [H3O+] when pOH is 8.90

A: First, from given pOH value the value of pH is calculated.

Q: Calculate the pH of a 0.022 M RbOH solution.

A:

Q: Write an equation to show that hydrochloric acid, HCI, behaves as an acid in water. + H₂O(l) +

A:

Q: Use Le Châtelier's Principle and the following table to predict the change in enthalpy and sign for…

A: The correct option with explanation is  given below:

Q: Using the literature Ka for theCH3NH3+ ion, calculate the theoretical pH of a 0.147 M solution of…

A: Concentration of methylammonium chloride = 0.147 MKa for CH3NH3+ is = 2.3×10-11   from literature

Q: Sn(NO2)2(aq) + KCl (aq) -->

A:

Q: Which of the following salts is considered basic when dissolved in water? Which of the following…

A: Given salts :  NaF  KCl  BaBr2 (NH4)2SO4 NaNO3  when a salt is dissolved in water , it gives acid…

Q: The F- ion is a weaker base in water than NH3 is. Explain what this means.

A:

Q: Given - 1 NiCI2 + 2 NaOH -> 1Ni(OH)2 + 2 NaCl Q. Calculate the moles of Ni(OH)2 that forms if the…

A: As we know that in a reaction, (No. of moles of substance reacted ÷ stoichiometric coefficient) =…

Q: is HC2H3O2 an acidic ionic or a covalent bond?

A: HC2H3O2 this is a chemical formula of acetic acid (CH3COOH).It has one double bond between Carbon…

Q: Calculate the pH of a 0.11 M solution of HCIO, with Ka = 3.5x10-8.

A:

Q: What coefficients (in order) are needed to balance the equation: Na₂O(s) + H₂O(l) →→→→→→ NaOH(s)? 1,…

A: Given, ___Na2O(s) + ___H2O(l) →  ___NaOH(s) Coefficients are needed to balance the above equation =…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A:

Q: In the following chemical reaction identify the acid. Don't worry about the charges and no need for…

A: Given [Al(H2O)6]3+ + 3H2O →  [AI(H2O)3(OH)3]2+ +  3H3O+

Q: What is the [H*] and pH of a sample with [OH] = 1 x 105?

A: Given,  [OH-] = 1 × 10-5 We know that  [H+][OH-] = 10-14

Q: For  K w, the product of [H 3O +] and [OH -] is

A: Kw is the water constant and is defined as product of hydronium ion and hydroxyl ion  Kw = [H3O+]…

Q: Which one is more acidic and  why?

A: In the given question, we are asked about the acidity of the following compounds: A.…

Q: Explain why the ionization constant, Ka, for HNO3 is larger than the ionization constant for HNO2

A: The question is based on the concept of acidity. the ease with which a molecule can donate proton is…

Q: Choose the correct answer: Which of the following is the strongest acid? HO. HO. HOH CI Br II II Но…

A: COMPOUND SHOWN IN - OPTION -II (FLUORINE DERIVATIVE) IS THE MOST ACIDIC ONE AMONG THE MENTIONED…

Q: The ionization constant of nitrous acid is 4.5 x 10-4. Calculate the pH of 0.04 M solution of…

A: Ka of HNO2 = 4.5*10-4[HNO2] = 0.04 MpH = ?

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.