Acetic acid (HC2H3O2) has a Ka = 1.8 x 105. What is the pKb of its conjugate base?

Q: What is Kb for the conjugate base of HBRO (Ka = 2.5 x 10°)?

A: HBrO Ka = 2.5 * 10-9

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :-  Ka for weak acid (HA) = 1.60 × 10-10  To determine :  Kb of its conjugate base (A-)

Q: The acid dissociation constant Ka of hypobromous acid HBrO is 2.3 x 10^−9. Calculate the pH of a…

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Q: 1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt…

A: Solving only first question in accordance with guidelines. We will first draw ICE table and then…

Q: Methylamine, CH3NH2, has a Kb of 4.4 x 10-4.  What is the pH of a 0.45 M solution of methylamine?…

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Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 × 10 . Calculate the pH of a…

A: When hypobromous acid dissolved in water it gives following Equilibrium -   HBrO + H2O <===>…

Q: Given that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar…

A: Given: Ka of acetic acid = 1.8 x 10-5  [CH3CO2–][CH3COOH] = 110   Calculating pKa pKa=-log (Ka)…

Q: what is the conjugate base of HPO4^2?

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

Q: The K₂ for a base is 15.3 x 10-13. What is the Ka for its conjugate acid?

A: Given :- kb for a base = 15.3 × 10-13  To determine :- value of Ka for its conjugate acid

Q: 4. Give the products from the following acid-base reactions and identify the acid and base on the…

A: The given reactions are represented as follows:

Q: Which of the following acids would have the strongest conjugate base? Acid Ka HIO3 1.7 x101 HCIO2…

A: Given : To find the strongest conjugate base from the given acids.

Q: Kraakenoic acid, when dissolved in 25 °C water, has a Ka of 6.66x10-6.  What is the Kb for the…

A: Relation between Ka and Kb , at 25 degree celcius  Kw = Ka * Kb

Q: The acid dissociation K, of acetic acid (HCH,CO,) is 1.8 x 10. Calculate the pH of a 2.1 x 10 M…

A: Recall the following expression to calculate pH of weak acid              pH=12pKa-12logCGiven…

Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 x 1 Calculate the pH of a…

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Q: The acid dissociation constant K, of hydrocyanic acid (HCN) iS 6.2 x 10 10 Calculate the pH of a…

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Q: The base protonation constant K, of morpholine (C¸H,ONH) is 2.14 × 10 °. Calculate the pH of a 1.0 M…

A:

Q: 4. Give the products from the following acid-base reactions and identify the acid and base on the…

A: Acids are those substances which donates proton i.e H+ ions in the reaction and bases are those…

Q: What is the ionization constant of a weak acid [HA], when its conjugate pair has a Kb value of 4.4 x…

A: In the ionization of a weak acid HA, A- is produced as a conjugated base.  HAAcid →Ionization…

Q: The acid dissociation constant K, of acetic acid (HCH3CO,) is 1.8 x 10. Calculate the pH of a 0.52M…

A: Given that : The acid dissociation Ka of acetic acid = 1.8 x 10-5 We have to calculate the pH of a…

Q: The hydronium ion concentration of an aqueous solution of 0.377 M ethylamine (a weak base with the…

A: Given, Concentration of of ethylamine solution (C) = 0.377 M [H3O+] = ? M ethylamine (C2H5NH2) is a…

Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5 What is…

A: Given: The Ka (acid dissociation constant) value of acetic acid is 1.76 x 10-5 The molarity of…

Q: The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10. Calculate the pH of a 3.2M…

A: PH of weak acid can be calculated by using the relation.  PH = 1/2 [ PKa - logC].

Q: The value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of Kp, for its conjugate…

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Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

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Q: The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7 . Calculate the pH…

A: Given acid is organic weak acid so it will dissociates partially into [Alloxanate] and [H3O+].…

Q: The base protonation constant K, of morpholine (C¸H¿ONH) is 2.14 × 10 °. 9- Calculate the pH of a…

A: Since morphine is a weak base. Hence the base dissociation reaction of morphine is  C4H8ONH (aq) +…

Q: What is Kb for the conjugate base of HCN (Ka = 4.9 × 10⁻¹⁰)?

A: We have given that  What is Kb for the conjugate base of HCN (Ka = 4.9 × 10⁻¹⁰)?  Acid : Acid is…

Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 x 10 '. 4 Calculate the pH…

A: Alloxanic acid is organic weak acid and it dissociates partially into [Alloxanate] and [H3O+].

Q: The Ka of a weak acid is 5.42 x 10-5. What is the pKb of its conjugate base?

A: Ka = 5.42 × 10-5 (given )  pKa = - log [Ka]  pKa = - log ( 5.42 × 10-5 )  pKa = 4.266

Q: The base protonation constant K₁ of morpholine (C₂H₂ONH) is 2.14 × 100. Calculate the pH of a 0.41 M…

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Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Sodium acetate is a salt of weak acid (CH3COOH) and strong base(NaOH).CH3COONa →  CH3COO- +…

Q: Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution…

A: For weak base CH3NH2 : [OH-] = Kb×C          = 4.4×10-4×0.20           = 9.38 x 10-3 M pOH = - log…

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

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Q: Which of the following relationships in INCORRECT? Assume T = 25°C. O pH + pOH = 14.00 %3D…

A: pH is the indicator of acidic nature of a solution. Any solution with pH equal to 7 is considered…

Q: The acid-dissociation constant, Ka, for maleic acid, H2C4H¼Os , is 7.56x10-7. What is the…

A: Ka of maleic acid = 7.56× 10-7

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (CH3O;)? CsH2Or(aq) +…

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Q: The acetate ion is the conjugate base of acetic acid. The Ka of acetic acid is 1.76×10–5. What is…

A: Kb for the acetate ion is determined as follows,

Q: The base protonation constant K, of lidocaine (C4H2 NONH) is 1.15 x 10 . Calculate the pH of a 1.0 M…

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Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 x 10. Calculate the pH of a 1.8…

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Q: What is Kb for the conjugate base of CH3COOH (Ka = 1.8 x 10)?

A: The relation between dissociation constant for acid, base and water is given as follows, Kw = ka ×…

Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 × 10 Calculate the pH of a 2.0 M…

A: Given: [HBrO] = 2.0 M Ka = 2.3×10-9 The hypobromous acid, HBrO is a weak monoprotic acid,…

Q: The acid dissociation constant K of hypobromous acid (HBRO) is 2.3 x 10. Calculate the pH of a 0.27M…

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Q: The base protonation constant K, of morpholine (C,H,ONH) is 2.14 x 10 °. Calculate the pH of a 0.41…

A:

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: Construct the expression for Ka for the weak acid, CH,COOH. CH,COOH(aq) + H,O(1) = H,0*(aq) +…

A: Expression  of Ka The equilibrium constant expression is the ratio of the concentrations of a…

Q: The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7. Calculate the pH of a…

A: Alloxanic acid is organic weak acid and it dissociates partially into [Alloxanate] and [H3O+].

Q: Consider the following acid-base pairs: H2CO/ HCO K 42 x 107 H;PO4/HPO K, = 6.2 x 10 NH/ NH3 K, =…

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Q: Lithium dihydrogen borate (LIH2BO3) is the lithium salt of the conjugate base of boric acid. The Ka…

A: Given that -  Ka for Boric acid, H3BO3 = 5.8×10-10    Then, from following formula -  Ka . Kb = Kw =…

Q: The hydronium ion concentration of an aqueous solution of 0.393 M caffeine (a weak base with the…

A: Caffeine is a weak base with formula C8H10N4O2. Hence it will dissociate partially as per the…

Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…

A: Ans. 3.33*10-11

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.