What is the pH of a 0.36 M Sodium acetate solution (CH3COONa)                                               Ka of CH3COOH = 1.8x10-5  42 85 57 15 67

Q: Calculate the pH of 0.50 M sodium acetate, CH3COONa. Ka(CH3COOH) = 1.8 x 10-5 5.72 11.48 2.52…

A: Given;

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: A 0.045 0 M solution of HA has a pH of 2.78. Find pKa for HA.

A: Given, initial concentration of HA = 0.0450 M             pH = 2.78 We know that, pH can be…

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: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2)…

A: The given data contains, Concentration of methylamine = 0.0341 M. Kb of CH3NH2 is 4.47×10−4.

Q: A 11 mM solution of a compound with a pKa = 6.5(1L total) has a pH of 7.5.If a biochemist adds 9…

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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: What is the pH of a solution that is 0.01M in picric acid and 0.1M in sodium picrate. (pKa=0.38)

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Q: Calculate the pH of a 0.512 M solution of a triprotic weak acid, H3A, given the acid ionization…

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Q: 3. 0.9206 grams of acetic acid is dissolved in enough water to make 60.0 mL of solution. Solve for…

A: Molarity :-  The number of moles of solute dissolved in 1 litre of solution is defined as molarity…

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: A 1.00 L solution contains propanoic acid (C3 H5 O2 H) with a concentration of 0.350 mol/L, and…

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Q: What will be the [H*] in a 0.50 M solution of HCIO? The Ka of HCIO = 3.5 x 10-8 A) 1.8 x 10-8 M B)…

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Q: Calculate pH for 0.0750 M C5H5NHCl (Ka=5.90 * 10^-6 for C5H5NH)

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Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?

A: Given concentration of CH3COOH = 1.75 × 10-5

Q: What is the pH of a 0.25M NaCH3COO solution? (the Ka value for acetic acid is 1.76 x 10^-5)

A: Sodium acetate is a salt of a weak acid (CH3COOH) and a strong base (NaOH). Therefore, the pH…

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: 4 A solution is made by dissolving 24.7 g of LIC3H5O2 in 500.0 mL of water. a Does Li have any…

A: We are authorised to solve first three subparts of a question. Please post rest of the subparts…

Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…

A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…

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 has 0.125 M CH3COOH and 0.125 M H3BO3? Ka of CH3COOH = 1.8 × 10−5…

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Q: Find the pH and percent ionization of a 0.200 M HNO2 solution Ka of HNO2= 4.6 x 010-4

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Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

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Q: a weak acid from pH The pH of a 0.41 M solution of benzoic acid (HC,H,CO,)is measured to be 2.29.…

A: Benzoic aicd is weak monoprotic acid. hence it will dissociate partially as per the reaction…

Q: 3. Calculate the pH of a 0.400 M KC2H3O2 (Ka for HC2H3O2 is 1.8 x 10-5)

A: In this question we have to tell the PH of the solution.

Q: 6. What is the pH of a solution containing 0.550 M HOAc and 0.460 M LiOAc? (ka of HOAc = 1.80 x…

A: The Henderson-Hasselbalch equation shows how the concentrations of an acid and its conjugate base…

Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4  The dissociation…

Q: Calculate the pH of a 0.236 M solution of a triprotic weak acid, H3A, given the acid ionization…

A: Given,   The pH of a 0.236 M solution of a triprotic weak acid, H3A is:   the acid ionization…

Q: Determine the pH of a solution that is 0.50 M in Ch3COOH and 0.75M in NaCH3COO Ka for CH3COOH =…

A: Given:- Determine the pH of a solution that is 0.50 M in Ch3COOH and 0.75M in NaCH3COO Ka for…

Q: HC5H4NCOO(aq) + H2O(l)⬄ H3O+(aq) + C5H4NCOO-(aq) 2.) Niacin, HC5H4NCOO, ionizes in water according…

A: Niacin is a weak acid it does not dissociate completely rather it dissociates partially.  From the…

Q: Calculate the molar concentration of OH- in a 0.075 M solutionof ethylamine (C2H5NH2; Kb = 6.4 x…

A: The reaction taking place is  => C2H5NH2 (aq) + H2O (l) -----> C2H5NH3+ (aq) + OH- (aq)  Hence…

Q: If vinegar contains 4% (w/v) of acetic acid (Ka= 1.8x10-5), calculate the pH of solution made by…

A: Q.1:  Before dilution:  concentration, C1 = 4%(w/v)  Volume, V1 = 50 mL  After dilution:…

Q: The sodium salt of propanoic acid, NaCH3CH2CO2, is used as an antifungal agent by veterinarians.…

A: Given, Sodium sat\lt of propanoic acid NaCH3CH2CO2 Concentration Of propanoic acid = 0.72 M Kb of…

Q: 2. Solution of ammonium chloride, NH4CI has a pH = 5.05. Calculate the volume of water to be added…

A: NH4Cl is a salt of strong acid and weak base.Initial pH of solution is 5.05 and final ph of solution…

Q: The sodium salt of propanoic acid, NaCH3CH2CO2, is used as an antifungal agent by veterinarians.…

A: Given: The Kb for CH3CH2CO2- = 7.7 × 10-10 We have to calculate the concentrations of H3O+ and OH-,…

Q: 5. The pH of 0.800 M aqueous benzenesulfonic acid is 0.51. What is the value of Ka for…

A: Benzenesulfonic acid is a monobasic acid which means it has only one removable proton. Given data,…

Q: Calculate the pH of a 0.20 M solution of NH4NO3 Kb(NH3) = 1.8x10^-5 Thank you :)

A: A pH scale is a scale that is used to determine the acidic and basic nature of a solution. If the pH…

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: 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 and percent ionization for a hydrocyanic acid (HCN) solution of concentration 2.0 X…

A:

Q: Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2) and 0.205 M in formic acid…

A: Given:Concentration of sodium formate [HCOONa] = 0.295 MConcentration of formic acid [HCOOH} = 0.205…

Q: Calculate the pH of a 0.075-M  Al(NO3)3 solution. The Ka value for Al(H2O)63+ is 1.4x10 -5

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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: 1. a. Tris (C4H6(OH)3NH2) has a Ka of 7.94 x 10−9. Calculate the Kbfor this compound. b. If a…

A: 1. a. Given that : Ka of Tris (C4H6(OH)3NH2) = 7.94 x 10−9 We have to calculate the Kb for this…

Q: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5.

A: Given,Concentration = 0.461M.Ka = 6.5×10-5Then,

Q: Calculate the pH of a 0.300 M solution of lactic acid, for which the Ka value is 1.40 x 104. A. 8.67…

A: Lactic acid is a weak acid. Given data is: concentarion of solution = 3.00 M Ka=1.40×10-4 Now, next…

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: 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

Q: Determine the pH of a 0.24 M solution of sodium acetate (CH3COONa) at 25°C.(Ka of acetic acid = 1.8…

A: Equation for the ionization of CH3COONa is: [CH3COONa] is 0.24 M. It implies 0.24 mols of CH3COONa…

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.