For a weak diprotic acid H2X, what is the relationship between [X2-] and Ka2? Under what conditions does this relationship exist?

Q: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10¯11. What is the pH…

A: The Ka1 is greater than Ka2 by a fraction of 10-4.  In a diprotic acid, firstly the first hydrogen…

Q: 1) A 0.45M aqueous solutionof creatine, (C4H9N3O2), has a pH of 1.49. Calculate the value of the…

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Q: H2CO3 is a diprotic acid with pKa1 = 6.36 and pKa2 = 10.33. What are the equilibrium concentrations…

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Q: Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration…

A: Given: Concentration of both the acids = 20 mM or 20×10-3 M To find: pKa, pH and percent…

Q: 1. Complete and balance the following equations for acid-base reactions: NH3 HNO3 > NaHCOз HCI ->…

A: Interpretation -  To complete and balance the following equation for acid -base reactions -…

Q: When scandium chloride, ScCls, is dissolved in water, which best describes the pH of the solution?…

A: Answer :- a) below 7  When Scandium chloride ScCl3 is dissolved in water, the pH of solution is…

Q: What are the [H3Oʻ] and pH of 0.085M weak base C2HSNH2?

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Q: Like any equilibrium constant, Kw changes with temperature. (a) Given that autoionization is…

A: The equilibrium constant Kw is called the dissociation constant or ionization constant of water.…

Q: Phosphoric acid (H3PO4) is tribasic, with pKa's of 2.14, 6.86, and 12.4. The charge of the ionic…

A: Given: pKa's of phosphoric acids are 2.14, 6.86 and 12.4. And the pH of the solution = 8

Q: Calculate the pH of a 0.350 M solution of benzoic acid. Benzoic acid is a weak monoprotic acid with…

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Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

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Q: 21. ASA (also known as Aspirin™) contains acetylsalicylic acid, C16H12O6. Acetylsalicylic acid is a…

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Q: Calculate the fraction of the weak base in each of its forms at pH 9.62.

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Q: Calculate the pH for a mixture of one mole of benzoic acid andone mole of sodium benzoate. The pKa…

A: When a weak acid and its conjugate base are present, it forms a buffer solution similar to the…

Q: Concentration of Na2CO3 solution: I00 N Calculated pKa of HCO3: (show calculations) C2. Measured pH:…

A: Since Na2CO3(aq) or CO32-(aq) is a weak base, it undergoes hydrolysis to form HCO3-(aq) and OH-(aq).…

Q: A diprotic base (B) has pK, values of 3.33 (pKpi) and 6.66 (pK82). Which of the equalities is true…

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Q: When a weaker acid is added to a salt of stronger acid,... a) No reaction takes place b) The weak…

A: Given statement is : When a weaker acid is added to a salt of stronger acid,…

Q: Phosphoric acid (H3PO4) is a triacid (pKa1 = 2.2 ; pKa2 = 7.2 ; pKa3 = 12.3). Write the balanced…

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Q: If enough of a monoprotic acid is dissolved in water to produce a 0.0124 M solution with a pH of…

A: Consider the general reaction of a monoprotic acid. HAl⇌H+aq+A-aqwater also go auto…

Q: If the kb NH3 = 1.8x10^-5, calculate the mass of NH3 in a 1.0 L ammonia solution whose pH is 11.10

A: Ammonia is weak base hence it dissociated less in aqueous solutions

Q: What is the pH of a solution that is 0.125 M in maleic acid, a DIPROTIC acid with Ka1=1.2x10-2 and…

A: Maleic acid dissociates in two steps. The major concentration of hydrogen ion is released in the…

Q: Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the…

A: We are given a combination of acidic, basic, and neutral salts.  Each salt has a concentration of…

Q: 10. Which one of the following species is not likely to react as a Lewis acid? H3C* AIH3 HaAl AICI3

A: Lewis’s acid-base theory:According to the Lewis acid-base theory, the substance that done a lone…

Q: What would the predominant form of the following species be in a solution with a set pH = 12.0? pK =…

A: Find the pI (iso electric point) for the given species .  pI =( pKa1 +pKa2 ) / 2  pKa + pKb = 14…

Q: Calculate the ratio [NH3]/[NH4+] in ammonia/ammonium chloride buffered solutions with the following…

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Q: Which correctly shows the ionization of H2CrO4 in water?

A: The acid given is H2CrO4.

Q: Provide the corresponding conjugate acid for the following substances: a. NH, b. H c. HPO,?

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Q: What is the dominant ionic form of phosphoric acid in a solution at pH 6.0?

A: Phosphoric acid is a triprotic acid with three dissociable protons and their pka are given as,

Q: 9. What molarity of ammonia solution would have pH = 10.92?

A: NH3 + H2O ⇌ NH4+ + OH- pH=10.92 pH+pOH=14 pOH = 14 - 10.92 = 3.08 pOH=-log [OH-]

Q: When 2.0 x 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH…

A: Nicotine is a weak monoprotic acid so it dissociated in less amount. So we can denotes it by HA .

Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa).   Kb for HCOO− = 5.9 × 10−11

A: Given :-  [HCOONa] = 0.31 M  Kb for HCOO- = 5.9 × 10−11  To calculate :-  pH of solution

Q: Will HNO2 act as a Bronsted-Lowry acid or base when reacting with water?

A: Identify Bronsted Lowry acid or base ---

Q: If enough of a monoprotic acid is dissolved in water to produce a 0.0122 M solution with a pH of…

A: The dissociation of a monoprotic acid is represented as follows: HA(aq)+H2O(l) ↔ H3O+(aq)+A-(aq)…

Q: Calculate 3OH-4 and pH for each of the following strong base solution 10.0 mL of 0.0105 M Ca1OH22…

A: volume of Ca(OH)2 = 10 mL concentration of Ca(OH)2 = 0.0105 M the calculation of moles is shown…

Q: If enough of a monoprotic acid is dissolved in water to produce a 0.0124 solution with a pH of 6.72,…

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Q: The acid dissociation reaction for the weak acid butyric acid, HC4H¬O2 is given below. Its Ka is…

A: The dissociation reaction given is Assuming y concentration of HC4H7O2 dissociates as per the…

Q: What is the predominant form of ammonia in a solution at pH 7.0? Approximately what fraction is in…

A: pH of compound is the negative logarithm of its hydrogen ion concentration. The pH  of a compound…

Q: 21. Identify the Lewis acid in the reaction. wwo O A) SO3 O B) o2- OC so,?- O DJ None of these.

A: lewis acids are those which are electron pair acceptors as they are electron deficient species.

Q: At 25°C, the Ka of pentafluorobenzoic acid (C6F5COOH) is 0.033. Suppose 0.100 mol of…

A: Given, Ka for C6F5COOH = 0.033 moles of C6F5COOH = 0.100 mol Volume of water = 1.00 L pH = Unknown

Q: Would a solution of NH,Y be acidic or basic at equilibrium and 25°C? The K, value for NH, is 5 x 10…

A: e) NH4Y is salt of weak base NH3 and weak acid HY .  Ka of NH4+ = 5 ×10-10 So,Kb of NH3 = 10-14 ÷…

Q: A weak acid HA, has a pKa of 5.0. If 1.0 mol of this acid and 0.1 mol of NaOH were dissolved in one…

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Q: If an acidic solution is more concentrated, does it mean that it produces more H+ ions than if the…

A: Acidic solutions are those which have a pH of less than 7.

Q: The most basic solution from the following is: * Pb(CH3C00)2 O CH3COONA O FECL3 O Al(CN)3

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: A solution is prepared using the ammonium/ammonia (NH4+/NH3) acid base pair. The ratio of acid to…

A: Given: Ka = 5.6 x 10-10 ammonium/ammonia (NH4+/NH3) = 0.18

Q: Calculate the pH of 0.050 M aqueous solutions of the compounds below at 25 °C: a. NaOH b. CH3NH2…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Carbonic acid (H2CO3) is a diprotic weak acid that undergoes the following dissociation reactions:…

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Q: The most basic solution from the following is: Pb(CH3CO0)2 FECL3 CH3COONA Al(CN)3

A: Basic solution are those which are good proton acceptor or hydroxide donors.

Q: What is the 3rd stepwise equilibrium constant expression (Ka3) for phosphoric acid H3PO4?

A: Given polyprotic acid is phosphoric acid, The general equilibrium constant expression is given by,…

Q: Calculate K, and pK, for water. H₂O acid (HA) + H₂O solvent H₂O+ + OH conjugate base (A)

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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.