What is the pH of 0.15M solution of acetic acid? Ka of acetic acid (CH3COOH) is (Ka = 1.8x10-5 )

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 solution of 0.20 M hydrazoic acid has a pH of 3.21. What is the Ka of hydrazoic acid?

A: We have to calculate the Ka of acid.

Q: What is the pH of 0.024M acetic acid solution at 25°C? (Ka=1.8×10^-5)

A: Given, [CH3COOH] = 0.024 M Ka = 1.8 × 10-5

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

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Q: What is the pH of a solution that is 0.12 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate,…

A: Given [salt] = [sodium acetate] = 0.5 M [Acid] = [Acetic Acid] = 0.12 M Ka of acetic acid = 1.8*10-5

Q: Acetic acid has a Kₐ of 1.8X10⁻⁵, and ammonia has a K(b) of 1.8X10⁻⁵. Find [H₃O⁺], [OH⁻], pH,…

A: (a) The acetic acid is a weak acid. The weak acid does not fully dissociate into its ions. We need…

Q: What is the Ka of 0.500M acetic acid if its ph is 3.7?

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Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: What is the pH and concentration of OH- of 0.0200 M CH3COONa?

A: The pH calculation from given concentration is as follows,The given compound is a salt in solid…

Q: 0.050 M solution of sodium meta-toluate (NaTol) has a pH of 8.47. What is the Kb of Tol-? What is…

A: Given that,  Concentration of sodium meta-toluate solution, M = 0.050 M pH of the sodium…

Q: What is the pH of a 0.17 M weak acid solution? The KA of the weak acid is 2.1 x 10-5.

A: Given :-  Initial concentration of weak acid = 0.17 M  Ka for acid = 2.1 × 10-5  To be calculated :-…

Q: What is the pH of 0.030 M aqueous formic acid (Ka of HCO2H = 1.8× 10^-6)

A: Formic acid dissociates as follows:                               HCOOH (aq) ⇌ HCOO- (aq) + H+ (aq)…

Q: What is the PH for a solution with [OH^-]=1.0X10^-6??

A: The relationship between the pH and pOH is as follows:                   pH+pOH =14 The formula for…

Q: A 0.050 M solution of sodium meta-toluate (NaTol) has a pH of 8.47. a. What is the Kb of…

A: 0.050M sodium meta-toluate has a pH of 8.47. Kb and Ka is to be found. Sodium meta-toluate is a salt…

Q: Calculate the PH of4.6M formic acid (CHOOH)  solution given a ka value of 1.787*10^-4

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Q: Calculate the pH of a 0.15M solution of sodium acetate (CH3COONa). What is the percent hydrolysis?…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: Calculate the pH of a 0.25M solution of formate ion (HCOO-) at 250 C.  The pKa for formic acid…

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Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

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: Calculate the [H+] and pH of a 4.35×10^−4 M butanoic acid solution. The Ka of butanoic acid is…

A: pH of the butanoic acid = 4.35 × 10-4 M  Ka of the butanoic acid = 1.52 × 10-5  [H+] of the butanoic…

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: What is the pH of a 0.010M solution of acetic acid? Ka for acetic acid is 1.8 x 10-5

A: Given :-  [CH3COOH] = 0.010 M  Ka = 1.8 × 10-5  To calculate :-  pH of solution     Ka is the ratio…

Q: The Ka of formic acid (HCHO) is 1.8 x 10^-4. Calculate the pH with 0.15 M formic acid.

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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 Ka for hydrofluoric acid is 7.1 × 10−4. Calculate the pH of a 0.15-M aqueous solution of…

A: pH: It is defined by saying that power of hydrogen present in any solution. It can be calculated…

Q: a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of…

A: pH + pOH = 14 pOH = -log [OH-] For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

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Q: The Ka of citric acid is 1.9x10-5 at 25.0oC, what is the pH of a 0.30 M aqueous solution of citric…

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Q: 1. Calculate the pH of the following: a. A solution whose pOH = 5.73 b. 12.0 M HNO3 c. 0.076 M…

A: Calculate the pH of the following---

Q: Calculate the pH of a 0.05 M solution of hydrofluoric acid. The Ka of hydrofluoric acid is 6.6x10^-4

A: Given data, Molarity of HF=0.05MKa of HF=6.6×10-4 pH of a solution is given by -log[H+]

Q: What is the Ka of bromoacetic acid if a 0.035 M bromoacetic acid aqueous solution has a pH of 2.22?

A: Let us take a reaction,        HX = H+ + X-  The dissociation constant of the above reaction is,  Ka…

Q: The Ka for cyanic acid HOCN is 3.5 x 10-4. What is the pH of a 0.37 M solution of the acid? What is…

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Q: A solution of acetic acid has a pH of 3.45. What is the concentration of acetic acid in this…

A: Given: The pH of the given acetic acid solution is 3.45 The Ka of acetic acid is 1.8*10-5

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: What is the pH of a solution that is 0.29 M KOCN and 0.14 M HOCN (cyanic acid)? (Ka for HOCN is…

A: Hensderson equation for the calculation of pH of a buffer solution consisting of a solution of weak…

Q: (Q12) Hydrazoic acid (HN3) is a weak acid with a Ka of 2.5 x 10-5. What will be the equilibrium pH…

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Q: A solution of benzoic acid (C6H5COOH) that is 0.20 M has a pH of 2.45. What is Ka for benzoic acid?

A: Benzoic acid is a weak acid. With the help of pH firstly calculate hydronium ion concentration.

Q: What is the pH of a 0.050 M solution of formic acid?

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Q: What is the Ka of hydrazoic acid if a 0.020 M hydrazoic acid aqueous solution has a pH of 3.22?

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

A: 0.015 mol/L acetylsalicylic acid has a Ka of 3.3 × 10-11.We have to calculate the pH and pOH at…

Q: Consider a weak acid "HA". What is the pH of a 0.856 mol L-1 solution of HA? The KA of HA is 1.14 x…

A: Given, HA is a weak acid Concentration of the HA solution (C) = 0.856 mol L-1 Ka for HA = 1.14 ×…

Q: Calculate the Ka of a weak acid if a 0.19-M aqueous solution of the acid has a pH of 4.52 at 25⁰C.

A: pH = 4.52 Concentration of aqueous solution = 0.19 M Ka = ?

Q: What is the pH of a solution that is 0.12 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate,…

A: Given data [sodium acetate]=0.50 M[acetic acid]=0.12 MKa=1.8×10-5   pH of weak acid and their salt…

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

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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: Calculate the pH of a 0.41 M CH3COONa solution. (Ka for acetic acid = 1.8 ×10−5.)

A: The reaction is written below. CH3COO - + H2O ⇌ CH3COOH - + OH- The ICE table is shown below.

Q: What is the pH of a solution that is 0.11 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium…

A: Since the solution is having weak base CH3NH2 and its conjugate acid salt CH3NH3Cl  Hence the…

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.