An acid HA has Ka = 2.28 x 10 -4. The % ionisation of this acid ina 0.170 M solution of the acid in water is closest to? a 2.930 % b 3.662 % c 2.564 % d 0.498 % e 0.436 % f 0.623 % Show step-by-step solution

Q: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

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Q: Pentanoic acid is another example of a weak acid. d. Calculate the value of Ka for a solution of…

A: Given: Concentration of pentanoic acid = 0.05mol/L pH = 3.05

Q: Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.222 M in formic acid…

A: The pH of the solution is calculated in accordance with the Henderson-Hasselbach- equation.

Q: The enthalpy of neutralization for a strong acid and a strong base is -57.3 kJ mol". Select an…

A: When one mole of H+ from strong acid and 1 mole of OH- from strong base reacts, -57 kilo joule per…

Q: What is the percent ionization of a 0.25 M HC2H3O2 solution (Ka = 1.8 x 10-5) at 25°C? O 0.60 % 0.42…

A: We have to find percent ionisation

Q: Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic…

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Q: Determine the [SO3²-] in a 0.020 mol L-1 solution of sulfurous acid, H2SO3 H20(1) = HSO3 (aq) +…

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Q: Halpinious acid, H2JHO3, is a weak diprotic acid with Ka1 = 2.40 x 105 and Ka2 = 4.79 × 10-11 at…

A: Given Ka2 <<<< Ka1 so, [H+] = Ka1.C [H+] = 2.40 × 10-5×0.500 = 3.46 × 10-3 M  pH = -log…

Q: cidic solutions have O (H;O*) > [OH]and pH > 7 O H,0*] > [OH] and pH 7 O H;0') < [OH ] and pH < 7

A: Acidic solutions can be defined as solution which has a higher concentration of hydrogen ions than…

Q: What is the pH of a bleach solution that has a OH = 2.3 x 10-3 M? %3D pH %3D Is bleach acidic,…

A: pH is a method to determine the concentration of hydrogen ions present in a solution. It helps in…

Q: A weak acid has Ka of 4.82 x 10-5.  What is pKa for this weak acid? Enter a numerical value in the…

A: Given: Ka = 4.82 × 10-5

Q: 10. A solution containing 1.75 M citric acid (H3C6H5O7) is prepared. Enough hydroiodic acid (HI;…

A: Given that : Molarity of citric acid = 1.75 M The final concentration of HI = 0.25 M The acid…

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: Calculate the percent ionization of 1.45 M aqueous acetic acid solution. For acetic acid, Ka = 1.8 *…

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Q: determine the percent ionization of the following solutions of formic acid at 25°C: (a) 0.066 M _%…

A: Given: Formic acid.

Q: 1. The Ka of boric acid, H3B03, is 5.8 x 10-10. Calculate the [H*], [OH¯], pH, pOH, Kb and percent…

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Q: I. True or False. Write TRUE if the statement is correct and FALSE if it is incorrect _1. The…

A: We are authorized to answer three subparts at a time since you have not mentioned which part you are…

Q: The [OH-] = 1.3 x 10-° M for a 0.025 M solution of a weak base. Calculate the value of Kb for this…

A: Consider reaction for the weak base is as follows; Reaction:      BOH aq        +        H2Ol…

Q: What is the percent ionization of a 0.50 M HC2H3O2 solution (Ka = 1.8 x 10-5) at 25°C? O 0.15 % 0.38…

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Q: 7, Calculate the [H3O+] of a 0.110 M acid solution; Ka=5.45 x 10-7 Group of answer choices 4.55 x…

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Q: True or False. Write TRUE if the statement is correct and FALSE if it is incorrect. ___________1.…

A: 1. False,  higher the pH, lower is the acidity  2. True 3. True

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

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Q: he pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka = 1.8 × 10-⁵) with 45 ml…

A: Answer :-  (b) 5.7  The pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka =…

Q: What is the concentration of X2 - in a 0.150 M solution of the diprotic acid H2X? For H2X, Ka1 = 4.5…

A: Given : Concentration of H2X = 0.150 M Ka1 of H2X = 4.5 X 10-6  And Ka2 of H2X = 1.2 X 10-11  The 2…

Q: pH

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Q: pH

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Q: What is the percent ionization of a 0.50 M HC2H3O2 solution (Ka = 1.8 x 10-5 ) at 25°C? O 0.15 %…

A: Given: Concentration of HC2H3O2 = 0.50 M And Ka of HC2H3O2 = 1.8 X 10-5  Since HC2H3O2 is a weak…

Q: Calculate the Ka of an acid, HX, whose ionization is 31% when CHX= 0.60 M (Note that the %…

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Q: Be sure to answer all parts. Determine the percent ionization of the following solutions of phenol…

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Q: A solution of 2.5 M weak acid is 1.52% ionized. What is the Ka value of ?this acid 3.6 x 10-4 3.2 x…

A: Assuming that the weak acid is monoprotic acid i.e HA. Given : Concentration of weak HA = 2.5 M And…

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: Calculate [H3O+] of the following polyprotic acid solution: 0.125 M H2CO3 (Ka = 4.3*10^-7, Ka2 =…

A: We have given that  Calculate [H3O+ ] of the following polyprotic acid solution: 0.125 M H2CO3 (Ka =…

Q: 2A04 H2AO4 is a weak acid. What is [AO4J in a 0.30M (Ka1 = 6.2 x 10-7; K a2 = 5.2 x 10-10 O^21x 10-5…

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Q: What is the percent dissociation of a weak acid with pH of 2.59 ? ka = 6.5 × 10-5. 0.50% 2.5% 1.5%…

A: Given values-&gt; pH = 2.59  Ka = 6.5×10^-5

Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C. Acidic Basic Neutral Answer…

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Q: Use the following acid ionization constants to identify the correct decreasing order of base…

A: The relationship between the Ka of acid and Kb of its conjugate base is Ka X Kb = 10-14 = Kw

Q: 1) Determine the [H30t] and pH of a 0 020 M weak acid solution with a Ka = 3.10 X10 . 2) A 0 34 M…

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Q: Calculate the concentration of each species present in a 0.025 M solution of phthalic acid,…

A: Pthalic acid is a weak acid and Ka is an equilibrium expression. The Ka is calculated by the…

Q: What is the pH of a 0.0319 M aqueous benzoic acid solution (Ka = 6.3×10-5)? Periodic Table and…

A: Given: Concentration of benzoic acid solution = 0.0319 M Ka for benzoic acid = 6.3×10-5 We have to…

Q: What is the pH and percent ionization for a hydrocyanic acid (HCN) solution of concentration 2.0 X…

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Q: A 1.2: 10-2 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of_ O 4.2. 10-13 O 2.4. 10-2 O 12.38 O…

A: pH value is used to measure the basicity or acidity of the aqueous solution.  If the pH values is…

Q: What is the percent ionization of a 0.50 M solution of pyruvic acid, HC3H3O3? (Ka 4.1 x 10-3

A: Pyruvic acid is a monoprotic acid. When it reacts with water, it releases H+ ions and forms H3O+ .…

Q: Hydrofluoric acid has a Ka value of 7.2*10^-4. What is the pH of a 0.04M solution of hydrofluoric…

A: Given information, Ka of hydrofluoric acid = 7.2*10-4 Initial concentration of hydrofluoric acid =…

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (CgHgO7)? CSH307(aq) +…

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Q: Which statement is true if an aquous solution is not neutral at 25°C. ? Explain your reasoning in a…

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Q: Find the pH of a 0.300M HNO2 solution. Ka = 4.9 x 10-10

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Q: The hypothetical weak acid H2A ionizes as shown below. Calculate the [HA-] in 0.20M H2A. H2A ↔ H+ +…

A: Given:  The initial concentration of H2A = 0.20 M Ka1 = 1× 10-7 Ka2 = 5×10-11

Q: 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: In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was…

A: Given : Initial concentration of acid = 0.37 M ka for HNO2 = 4.5 × 10-4

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.