Consider the following illustrations: H* A B

Q: 2. One mole of H* is always neutralized by mole of OH-.

A: -> If water form from combination of ions  then it is neutralization .

Q: Determine the [H], [OH-], and pOH of a solution with a pH of 11.02 at 25 °C. [OH-] = РОН= Determine…

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Q: Choose the correct answers from among the alternatives; For the sentence to be correct: they are…

A: Weak acid : It is an acid which do not dissociates completely in water .

Q: Apply the Bronsted theory of acids and bases to the following reaction: H3AsO4(aq) + H2O( l ) ⇆…

A: Answer:- This question is answered by using the simple concept of conjugate acid and base. Conjugate…

Q: Which of the following statements is true about the pH value of a solution? Oa If the pH is exactly…

A: A solution can be divided into 3 types based on the pH of the solution as acidic, basic, and…

Q: O ACIDS AND BASES Understanding the difference between strong and weak acids acid he chemical…

A: Acid can be defined as a species that give hydrogen ions in an aqueous solution.

Q: Determine whether each anion is basic or neutral. For those an- ions that are basic, write an…

A: An anion is a species which have more electrons than the no. of protons. Due to extra electrons, it…

Q: List the following acids in order from weakest to strongest based on the information in the table…

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Q: Which solution below has the highest concentration of hydronium ions (H+)? pH = 8.1 pH = 4.3  pH…

A: The concentration of hydronium ions can be calculated by the reverse of the mathematical operation

Q: Calculate the pH of a 0.0306 M solution of calcium hydroxide. B. Is H3N an acide, basic, neutral or…

A: A.  Concentration of calcium hydroxide = 0.0306M 1 mol Ca(OH) 2 has 2 mol OH- ions Now,…

Q: Calculate the pH corresponding to each of the hydrogen ion concentration given below, and indicate…

A: pH of any solution is given by  pH = -log[H+ ] where [H+ ] = concentration of H+ ions in the…

Q: An aqueous solution has a hydrogen ion concentration of 1.0 × 10-8 M. What is the hydroxide ion…

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: The pH equation is pH = -log [H+] It a log base 10 equation.  How does the concentration of a pH 5…

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Q: Both HCO3^- and HS^- are amphoteric. Write an equation to show how each substance can act as an acid…

A: According to Arrhenius theory, acids are the substances, which when added to water, release H+ ions…

Q: OH(aq) + H₂CO3(aq) HCO3(aq) + H₂O(1) [Select] [Select] [Select] î + [Select] û Considering the…

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Q: What are diprotic and tricrotic acids? List an example of each?

A: According to Arrhenius, Acid which gives H+ ions in the aqueous solution. number of displaceable…

Q: Identify the following species as strong or weak acids or bases. a) HF b) NaOH c) NH3 d) HCIO4 e)…

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Q: concentration of 7.23 x 10^-7 at 100 degrees C. What is the hydrogen ion concentration? Is the…

A: In water,  [H+] = [OH-] [OH-] = 7.23×10-7 M [H+] =  7.23 ×10-7 M Kw =[H+][OH-] =  5.23 × 10-13 pH =…

Q: If the following are dissolved in water, classify the resulting solutions as acidic, basic, or…

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Q: The acids correctly ranked according to decreasing strength is: Provide an explanation Select one:…

A: Option B is correct

Q: An aqueous solution has a hydrogen ion concentration of 1.0 × 10¬8 M. What is the hydroxide ion…

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Q: 2. Define Bronsted and Lawry theory of acid and base with an example. Explain conjugated acid and…

A: Bonsted's vision - Lowry is an acid-base reaction theory to the idea promoted independently by…

Q: Apply the Bronsted theory of acids and bases to the following reaction: H3AsO4(aq) + H2O( l ) ⇆…

A:

Q: Determine the [H+] if [OH-] is 7.10x10-3M and classify the solution as acidic or basic.

A: Answer - Anything below 7.0 is acidic, and anything above 7.0 is alkaline, or basic. pH scale,…

Q: What is the pH of a 0.6 M HNO2 solution? (Enter your answer to the hundredths place, without units.)

A:

Q: Based on the auto-ionization of water, draw a graph showing the relationship of [OH-] and [H+].…

A: Auto ionisation of water means that water self ionises to give H+ and OH- ion.

Q: A. Give the chemical equation that correct describes the ionization of HBr in water B. Give the…

A: We have to predict the chemical reaction in given both questions.

Q: Classify the following as Brønsted acids, bases or both. Write the letter that corresponds to your…

A: According to Bronsted acid base theory, acid are the specie that donate H+ and base are specie that…

Q: Why is there more than one definition of acid–base behavior? Which definition is the right one?

A: Over the time period, different researchers have postulated their own acid and bases definitions.…

Q: A solution is made by dissolving 13.9 g of HONH:CIO3 in 500.0 mL of water. Does HONH3* have any…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: What is meant by strength of a base

A: The meaning of strength of the base is the tendency to finish [OH-] ion in their aqueous medium…

Q: Calculate the [OH-] in each of the following solutions, and indicate whether the solution is acidic…

A: The relationships which we will be needing are 1) pH = -log[H+ ] where [H+ ] = concentration of H+…

Q: OH (aq) + H2CO3(aq) HCO, (aq) + H2O(1) [ Select ] [ Select ] + [ Select ] [ Select ] Considering the…

A: According to Bronsted-Lowry Concept, conjugate acid-base pair only differ by one proton (H+). A…

Q: What kinds of cations act as weak acids? List some examples?

A: When a neutral atom tends to lose an electron then it acquires a positive charge and it is called a…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

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

Q: In an aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak…

A: Here given various type of  compounds .

Q: A: Classify the following as Brønsted acids, bases or both. Write the letter that corresponds to…

A: According to Bronsted acid-base theory, acid is the the proton (i.e. hydrogen ion) donor and base is…

Q: A: Classify the following as Brønsted acids, bases or both. Write the letter that corresponds to…

A: According to Bronsted and Lowry , the compound which donate H+ ( proton ) is called acid and which…

Q: Which ion forms a basic solution when dissolved in water?a) Br- b) NO3- c) HSO4- d) SO32 -

A: An acid donates proton and forms a conjugate base. The strength of an acid depends upon the…

Q: The ph of a solution is 12.65 what is the [H+

A:

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10 M. a. Is this solution an…

A: pH = -log[H+]  [H+] = 10-pH

Q: Explain the process of self-ionisation/autoionisation of water molecules. The points should be…

A: NOTE : Since you've posted multiple sub-parts,we'll solve first three sub-parts for you. To get the…

Q: Question: Explain the process of self-ionisation/autoionisation of water molecules. The points…

A: The self-ionization of pure water is also known as autoionization of water. In this reaction, H2O…

Q: Which of the following are not strong acids? (choose all that apply) HCIO4 HI HNO3 HF HCIO2 HBr HNO2…

A: Strong acid: An strong acid undergoes complete dissociation in water Weak acid: A weak acid…

Q: NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq) In this chemical equation, NH3 and H2O serve as --- and ---,…

A:

Q: Consider the reaction.   CH3CH2O−+HC≡CH↽−−⇀HC≡C:−+CH3CH2OH   Classify each reactant and product…

A: According to the Brønsted theory of acids and bases, 1) Acids are those substances which donate…

Q: Classify the following as strong or weak acids and/or bases: a) HBr b) CIO4 c) HCO3 d) H2SO3

A: The correct option are as follows:

Q: Classify each of the following as a Strong acid (sa) or a Weak acid (wa) and indicate how each…

A: An acid is a compound that donates H+ or forms H3O+ in aqueous solution.

Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution. A. [H3O+][H3O+] = 6.6×10−12 M…

A: In given question Kw = [H+][OH-] formula used

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.