If the Ka of the conjugate acid is 7.68 × 10-4 , what is the pKb for the base?

Q: What is the pH of a solution that contains 0.10 M HCl and 0.10 M acetic acid (HC2H3O2)? Ka for…

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Q: The weak acid, HA, has a Ka of 3.00 x 10-8. What is the Kb of its conjugate base, A"? 1.39x10-12 O…

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Q: On acidity and basicity of aqueous solutions, the following relationships are valid, except…

A: Given : We have to tell the incorrect statement.

Q: What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Given: Ka of HC2H3O2 =…

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Q: Calculate the Ka of weak acid.  The initial concentration of the weak acid is 4.93 x 10-4 M.  The…

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Q: The Ka of a weak acid is 3 x 10^-12 What is the pKa of this acid?

A: Ka which is dissociation constant of acid is given  3*10^-12  Pka = ?

Q: 9) HB has a Ka of 5.2 x 10-5 and HC has a Ka of 4.6 x 10-4 . Which solution will have a lower pH,…

A: Given : Ka of HB = 5.2 X 10-5  Ka of HC = 4.6 X 10-4  And concentration of HB = concentration of HC…

Q: The Ka of formic acid (HCHO2) is 1.8 x 10^-4. What is the pH of a 0.35M solution of sodium formate…

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Q: A weak base has Kp 6.5x10-6. Calculate the pKa of the conjugate acid. Express your answer to two…

A: The dissociation constant of an aqueous solution of weak acid is known as the acid ionization…

Q: The pKa of acid HX is 6.02, and the pka of acid HY is 3.76. We can conclude that the Kp value of…

A: The larger the PKa value, stronger is the Acid and a weak base. Smaller the PKa value weaker is the…

Q: What is the Kb for the conjugate base of an unknown acid with a Ka of (7.1x10^-3)

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Q: Calculate the percent ionization of ascorbic acid (HC6H7O6) in solutions of each of the following…

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Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: Hydrogen cyanide, HCN, also called hydrocyanic acid is a weak acid with a pKa near 10. What would be…

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Q: What is the pH of a solution

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Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid?…

A: pKa of any acid can be calculated as: pKa=-logKa Ka is dissociation constant of an acid. Larger the…

Q: The Ka of acetic acid is 1.80 x 10-5.  A. What is the pH of a 0.0010 M solution of acetic acid? B.…

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Q: A weak base has K, = 2.4 x 10-4 at 25°C. By adding a strong acid to solution, there is an acid-base…

A: Weak base = B Kb = 2.4×10-4

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: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: calcualate the pH of a 0.15 M solution of pyruvic acid ka of pyruvic acid is 4.1x10^-3

A: Given: Molarity or concentration of pyruvic acid = 0.15M Ka of pyruvic acid = 4.1 × 10-3

Q: What is the value of pKb for the cyanide anion, CN- at 25⁰C? Ka(HCN) = 6.2 ´ 10^-10?

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Q: Determine whether the statements are true or false. ( a. The stronger the base, the smaller the pKp.…

A: The pH scale range and the acid character of an acid or base can be known using Pka and PKb or just…

Q: If the Ka of the conjugate acid is 2.78 × 10-7 , what is the pKb for the base

A: Based on Bronsted theory, whenever a base accepts a proton that is H+, the formation of conjugate…

Q: Acetic acid has a Ka = 1.8 x 10- 2 points 5 Determine the pH of a O.2 M acetic acid solution *…

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Q: Calculate the pH of an aqueous solution containing the following: a) 0.80 M lactic acid and 0.40 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: Determine the pka of an acid whose concentration is 0.100M and pH is 2.86.

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Q: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa + log ([A–]/[HA])…

A: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa +log[salt][acid]…

Q: to be 1.48 at 25°C. Calculate the Ka for the acid. 3. What is the original molarity of an aqueous…

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Q: If the Ka of a weak acid is 1.6 x 10-8, the Kb of its conjugate base partner must be which of the…

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Q: acid, Ka = 7. The value of Ka for acetylsalicylic acid (aspirin) is 3.00x10-4. What is the value of…

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Q: A weak acid has KA = 1.59 x 10-8. What is the pKB of its conjugate base?

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Q: If a weak acid has a Ka of 2.04 x 10-7 what is the value of pKb?

A: Given  Ka value of weak acid = 2.04 × 10-7 PKb = ?

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: What is the pH of a 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8x10-5 ?

A: Given, Concentration of sodium acetate = 0.20 M Ka of acetic acid = 1.8 x 10-5 Formula used, [OH-] =…

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: The concentration of an unknown acid is 1.2M with a pH of 1.60. What is the pk the acid?

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Q: Calculate the pH of a solution that is 0.195M in sodium formate (NaHCO2) and 0.24 M in formic acid…

A: Given: Concentration of  sodium formate (NaHCO2) = 0.195 M            formic acid (HCO2H)  = 0.24M…

Q: Calculate the expected pH of a 0.100 M acetic acid solution.     Ka for acetic acid is 1.76 x 10-5…

A: Given data, Concentration of acetic acid = 0.100 M  Ka for acetic acid = 1.76 × 10-5

Q: The Keq for the reaction:  A + B ↔ AB is 2.03 What is the Keq for AB ↔ A + B Keq = ?

A: The equilibrium constant, Keq for the reaction:  A + B ⇌ AB is 2.03 The equilibrium constant, Keq…

Q: If the Ka of the conjugate acid is 4.39 × 10-8 , what is the pKb for the base?

A: Acid dissociation constant  (Ka) and base protonation constant (Kb) can be mathematically expressed…

Q: What is the pH of an acetic acid solution with a K a of 1.76 x 10 -5 of 0.05 M?

A: Given  K a of acidic acid 1.76 x 10 -5 of 0.05 M

Q: What is the pH of a 0.040 M solution of benzoic acid (Ka = 6.3 × 10-5) at 25ºC?

A: Given : Concentration of benzoic acid i.e C6H5COOH = 0.040 M And Ka of C6H5COOH = 6.3 X 10-5  Since…

Q: The pK, of a particular weak acid is 5.17. What is the pH of the weak acid solution when exactly…

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Q: . What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Ka of HC2H3O2 = 1.8 x…

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Q: The Ka of acetic acid is 1.8 X 10-5.  The Kb of the acetate ion is

A: Acetic acid is a weak acid and its conjugate base is acetate ion. The reaction of conjugate acid-…

Q: Calculate the pH of a 0.05 mol dm3 CH;COOH solution: the dissociation constant Ka for CH;COOH is…

A: An acid which will not dissociate completely to furnish hydrogen ion is called weak 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.