Compare the relative acidity of 1-molar aqueous solutions of the following acids.NH4Cl CH3COOH BrCH2COOH F3CCOOH H2SO4 HCl HBrpKa = 9.26 pKa = 4.74 pKa = 2.9 pKa = 0.2 pKa = -5 pKa = -7 pKa = -9

Q: Which of the following salts would produce the most basic aqueous solution? NH4ClO4 NaCN K2SO4…

A: Acidity and basicity of salt -> Strong acid + strong base => Neutral Strong acid + weak base…

Q: For the following weak base, write a bronsted Lowry acid base reaction with water showing the…

A:

Q: How would you categorize a solution that has a concentration of hydroxide ions equal to 3 x 102 M? O…

A: A solution is acidic if pH<7 Basic if pH>7 Neutral if pH=7 pH is the -log[H+] pOH = -log[OH-]…

Q: Calculate the [H30+]value of{OH-}=1.2x10-11M

A: We have to calculate the [H3O+]

Q: CH3NH2 reacts with H3O*, resulting in CH3NH3* and H₂O. Which statement is true? CH3NH2 is a base…

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Q: What is the principle form of a triprotic acid (HSA) at pH 8? What is the pH of a 0.500M Solution of…

A: Note: As you have posted multiple questions, the first question is solved by us. Please post the…

Q: 1. Identify the acids and bases in the following reactions: (al CH3OH + H* - CH3OH;+ (b) CH3OH + NH3…

A: Since here multiple question have been posted so I am going to solve question 2 ,3 and 4. if you…

Q: Which compound below is the stronger acid in aqueous solution? W 5.0M H2SO3 or 0.020M H2SO4…

A: To find: Which is stronger acid in solution, 5.0 M H2SO3 or 0.020 M H2SO4?

Q: Which of the following shows an increase in the acid strength (from the weakest to strongest) in an…

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Q: Calculate the concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data:  Ka1 = 4.2×10-7…

Q: Question 5 What is the best amount (in mol) of OH¯ used at the 2nd stoichiometric point of tl…

A: Diprotic acid is one which can release 2 hydrogen ions of a molecule in aqueous solution.…

Q: If the pKa of HCHO 2 is 5.74 and the pH of an HCHO 2/NaCHO 2 solution is 6.11, which of the…

A: A buffer solution is a that type of solution in which if we add a small amount of acid or base then…

Q: Which of the following salts may be obtained by the reaction of a weak acıd With a strong base?…

A: a) LiClO4  Made by strong base : Li(OH)  Made by strong acid: HClO4   b) NaCl Made by strong base :…

Q: Arsenic acid, a triprotic acid, has 3 pKa values (2.24, 6.96, and 11.50). What is the predominate…

A: We will see the predominant form of arsenic acid at a pH = 4.00  You can see below details…

Q: Each of these three molecules contains an OH group. When dissolved in water one solution has a pH7.…

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Q: this reaction what is the Bronsted-Lowry acid? HO⁻ + H₃C-I

A: According to Bronsted-Lowry theory, acid is a substance which donates an H+ ion or a proton and…

Q: In the following neutralization reaction, which compound is the salt? Н3РОД + 3 LiOн LizPO4 + 3 H20…

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Q: Rank the following solutions according to their acidity: Solution 1 pH = 12 Solution 2 [H3O+] = 106…

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Q: What is the OH- concentration of a solution  with a H3O+ concentration of 8.47x 10-8

A: Given concentration of H3O+ is 8.47 × 10-8  [H3O+] = 8.47 × 10-8

Q: Which base would be the best choice for preparing a pH = 9.50 buffer? pyridine ethylamine aniline…

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Q: why, during an experiment, was the initial pH of HCl, a strong acid, 2.12, while the weak acid,…

A: During an experiment,  the initial pH of HCl, a strong acid, 2.12, while the weak acid, acetic acid,…

Q: Which of the following solutions has a p

A: Salt hydrolysis : the process in which cation (or) anion (or) both of a salt reacts with water to…

Q: What is the pH of a water at 25oC that contains 0.5 mg/L hypochlorous acid? Assuming equilibrium has…

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Q: Which is the conjugate acid in the following reaction? HCI H20 H,0 II II IV

A: Given :-  HCl + H2O <-----> Cl- + H3O+  To identify :-  Conjugate acid in above reaction

Q: What will happen to this equilibrium when NaOH is added? NH3 + H+ NH4+

A: Given-> NH3 + H+ <------> NH4+

Q: F[OH-] = 1.45 x 102, find the pOH.

A: pOH is the measure of acidity or basicity. Lesser the value of pOH more basic is the solution. pOH…

Q: Explain why the hydrogen ion (H+) concentration of a 1x10-3 M solution of H2So4 is 2x10-3

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Q: Rank the following solutions according to their acidity: Solution 1 pH = 12 [H3O+] = 10-8 M Solution…

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Q: Carbonic acid, H₂CO3, is a very weak diprotic acid. In a 0.10 M solution of this acid, which of the…

A: Carbonic acid is a weak acid and it dissociates as follows:

Q: Hi can someone please help with these?

A: As you have asked question with multiple subparts we will solve the first few parts for you. If you…

Q: Which of the following acids would be able to neutralize the most base? 200 mL of 0.5 M H2SO4 O 100…

A: An acid can neutralise base to give salt and water.  1 H+ ion of acid reacts with 1 OH- ion of base…

Q: The hydronium ion concentration of an aqueous solution of 0.56 M phenol (a weak acid), C6H5OH, is…

A: Given,  Molarity of phenol (C6H5OH) = 0.56 M.  Ka of phenol is : 1.00 × 10-10 (from reference)  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.