1.) In a 0.100M aqueous solution of a weak acid, the acid is 3.7% dissociated. What is the Ka for this acid?

Q: Consider a solution which is 0.10M in CH3COOH and 0.20M in NaCH3COO. Choose ALL 81 O If Ca(CH3COO)2…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: What is the pH of a solution that is 0.200 M ammonia (NH3) and 0.150 M ammonium chloride (NH4Cl)?…

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Q: A solution is prepared that is initially 0.39M in hypochlorous acid (HC10) and 0.28M in sodium…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.528 M aqueous solution of…

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Q: A solution is prepared that is initially 0.42M in hydrofluoric acid (HF) and 0.28M in potassium…

A: HF  +  H2O  ----->   F-   +  H3O+

Q: HA is a weak acid. B1 and B2 are weak bases. Two acid/base neutralization experiments are performed…

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Q: Aspirin, a drug that is used to relieve minor aches and pain, is a weak monoprotic acid. What is the…

A: we know that pH = -log [H+] so -log [H+] = 3.12 [H+] = 0.000758

Q: None

A: Step 1:Since H2A is a weak diprotic acid, it can donate two H+ ions. We will find the concentration…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31.  What is the Ka of the acid?

A: Given  pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: Many important bio chemicals are organic acids, such as pyruvic acid (pKa = 2.50) and lactic acid…

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Q: What would be the pH of a solution of hypobromous acid (HOBr) prepared by dissolving 9.7 grams of…

A: given:  mass of HOBr = 9.7 g molar mass of HOBr = 96.91 g/mo moles of HOBr = 9.796.91= 0.1 moles…

Q: HA is a weak acid. B1 and B2 are weak bases. Two acid/base neutralization experiments are performed…

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Q: How many ml of 0.5 M HCl must be added to 100.0 ml of a 0.2 M Imidazole (C3H4N2 ; Kb=6.3x10-8)…

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Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: A 0.0720 M solution of a monoprotic acid is known to be 1.52% ionized. What is the pH of the…

A: Concentration of solution of monoprotic acid = 0.0720 M Percent ionization = 1.52%

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.150 M solution…

A: Answer :

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: The ionization of NH4Cl as follows,

Q: What is the value of Ka of this acid? What is the percent ionization of this acid?

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Q: Acrylic acid, whose formula is HC; HOz or HO, CCH-CH2, is used in the manufacture of plastics. A…

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Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?

A: Given data,pH=2.13Molarity of HA=0.45

Q: Quinine, an alkaloid derived from a tree that grows in tropical rain forests, is used in the…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

A: Aniline is a weak base , lets find its pOH  pH +pOH = 14 (at 25oC)  9.305 + pOH = 14  pOH = 14 -…

Q: What is the pH of a solution that is 0.32 M KOCN and 0.10 M HOCN (cyanic acid)?

A: Since cyanic acid is a weak acid with pKa = 3.46  And the solution is having HOCN i.e cyanic acid…

Q: Calculate the pH of the following solutions. (1)Tap water after boiling       (2)  0.0010 M NaOH…

A: Note - Since you have asked a question with multiple sub-parts, we will do the first three sub-parts…

Q: 2.) A 3.90 g sample of aniline (C.H$NH2, K» = 4.3 x 100 at 25°C) is dissolved in sufficient water to…

A: ·Mass of Aniline = 3.90 g·Volume of solution = 100 mLAs we know that,·Molar mass of aniline = 93…

Q: Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What…

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Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: In the laboratory, a general chemistry student measured the pH of a 0.429 M aqueous solution of…

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Q: 19.00 mL of 0.100 M sodium hydroxide is added to 39.00 mL of a 0.100 M acetic acid solution. The Ka…

A: Since sodium hydroxide is a strong base.  hence it will react with the acetic acid as  NaOH +…

Q: what is the pH of a solution prepared by adding 63.6 mL of 0.100 M sodium hydroxide to 69.37 mL of…

A: Given that : The volume of sodium hydroxide = 63.6 mL The molarity of sodium hydroxide = 0.100 M The…

Q: Calculate the K₂ for a monoprotic acid, HX, if a 0.100000 M solution has a pH of 3.333. The data is…

A: The given reaction is : HX     +     H2O      ⇔       X-     +     H3O+ The answer is as follows:

Q: How to calculate the ph? What would be the result if the acid was a di or tripotic? How do the…

A: All of your concerns are discussed; please go through each step.Explanation:Step 1: Let's learn…

Q: The K₂ of a weak acid HA at 25.0 °C is 2.6x10-6. What is the pH of a 0.63 M aqueous solution of HA?…

A: Given,Molarity of weak acid, HA = 0.63 MKa at 25.0 0C

Q: Consider 0.10 M solutions of the following compounds: Sr(OH)2, Ca(OCl)2, FeCl3, Ca(C3H5O3)2, and…

A: Sr(OH)2 is a strong base and will have the highest pH. Ca(C3H5O3)2 is a weak base and will have a…

Q: Aniline is a weak base. The pH of a 0.010 M aqueous solution of aniline is 8.32. What is the percent…

A: The percentage of dissociation of  aniline can be calculated as follows

Q: A solution is prepared that is initially 0.087M in benzoic acid (HC H,CO,) and 0.11M in potassium…

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Q: The pH of a 0.100 M aqueous solution of an unknown monoprotic acid, HX, is 5.26 at 25 ºC Which of…

A: Given The pH of a 0.100 M aqueous solution of an unknown monoprotic acid, HX, is 5.26 at 25 ºC Ka =…

Q: A 2.00 L solution contains 0.545 M NH3 and 0.641 M NH4A.  (The Kb of NH3 is 1.86⋅10−51.86⋅10-5).…

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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.