Arsenic acid H3AsO4 is a moderately weak triprotic acid. Write equations  showing its stepwise dissociation. Which of the three anions formed in these reactions will be the strongest Brønsted base? Which will be the weakest Brønsted base? Explain your answers

Q: A substance that ionizes completely in aqueous solutions and produces H3O+ is a     weak acid.…

A: A substance that ionizes completely in aqueous solutions and produces H3O+ is a Strong acid. H2SO4 +…

Q: What is the pH of a 0.0023 mol/L solution of nitric acid? The answer should be to the proper number…

A: pH of the solution is calculated as  pH = – log[H+] Given that [HNO3] = 0.0023 mol/L

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.26 M solution…

A:

Q: Calculate the pH of a 0.170 M solution of potassium nitrite, KNO₂. pH =

A: Given that, [KNO2] = 0.170 M =C (LET)  pH = ?

Q: Add curved arrows to the reactants in this reaction. A double-barbed curved arrow is used to…

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.60 M solution…

A: Answer:Value of pH is equal to:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.23 M solution…

A: The PH of diprotic acid can be calculated as follows

Q: Calculate the pH of water at 60 °C. The pKa of water is 13.017 at this temperature.

A: Since pKa = -log(Ka) => Ka = 10-pKa  = 10-13.017 = 9.62 X 10-14 approx H2O (l) -----> H+(aq) +…

Q: Determine the pH of a 0.13 M solution of pyridinium nitrate (C5H5NHNO3) at 25°C. [Pyridinium nitrate…

A: Determine the pH of a 0.13 M solution of pyridinium nitrate

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

A:

Q: An aqueous solution has hydronium concentration [H3O+] = 9.8 x 10-5 mol L-1. What is the pH of the…

A:

Q: An aqueous solution at 25 °C has a pOH of 7.5. Calculate the pH. Be sure your answer has the correct…

A: Given,  At 25 °C, pOH = 7.5

Q: Which is the stronger base, HOC2H4NH2 (ethanolamine) or HCO3− (hydrogen carbonate ion)? (See the…

A: Basicity is defined as the electron donation ability of a molecule.  If it is able to donate…

Q: Write the formula of the conjugate base of C₆H₅SH.

A: According to Bronsted and Lowry theory, when an acid releases a proton, the remaining part must be a…

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A:

Q: As the temperature of water is increased above 25 ℃ the pH decreases.  Which of the statements below…

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.45 M solution…

A: The question is based on the concept of equilibrium. we have determine the pH of the given diprotic…

Q: Calculate the pH of each of the following solutions of strong acids.

A:

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: Carbonic acid (H2CO3) is a polyprotic acid. Write balanced chemical equations for the sequence of…

A: Thank you.

Q: How many moles are there in 20.0 mL of a 0.125 M solution?

A: Molarity = moles of Solute ÷ Volume of solution(L)

Q: Identify which statements regarding acid strength are true and which are false. HCl is a stronger…

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution…

A: Reactions- H₂A + H2O ↔HA-  + H3O+  Ka1 = 3.4 × 10⁻⁴ HA- + H2O ↔ A2- + H3O+  Ka2 = 6.7 × 10⁻⁹ Ka1…

Q: Explain how ammonia can function both as a Brønsted base and as a Lewis base.

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: Exercise 4 Write a Ka (hydrolysis) reaction for the following acids. Use the appropriate type of…

A: Note: As per guidelines solution of question-4 has been made. For the expert solution of other…

Q: The substance morphine is a weak nitrogenous base like ammonia. Write a net ionic equation to show…

A: The compound which accept H+ is known as base.  Here morphine is base.

Q: is HC2H3O2 an acidic ionic or a covalent bond?

A: HC2H3O2 this is a chemical formula of acetic acid (CH3COOH).It has one double bond between Carbon…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: Oxoacids can be formed that involve several central atoms of the same chemical element. An example…

A: The acidity of each oxoacid can be measured by calculating the ratio of the number of double bonded…

Q: Calculate the pH of a 1.00 × 10-5 M solution of HCN(aq). The Ka of HCN(aq) is6.17 × 10-10.

A:

Q: stimate the pH of 0.175 M HCOOH(aq) at 25°C.  Ka(HCOOH) = 1.7 × 10−4. Write your answer with two…

A: The acid dissociation constant of HCOOH is .The concentration of HCOOH is .To find the pH of the…

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: Weak acids dissociate partially in an aqueous solution to furnish the hydrogen ions. The…

Q: Consider the following data on some weak acids and weak bases: name nitrous acid acid hypochlorous…

A: The question is based on the concept of salt hydrolysis. we need to arrange the given salts…

Q: Write the equations for the dissociation of the following weak acids and identify their conjugate…

A:

Q: What is the pH of wine that has an H 3O + concentration of 3.2 × 10 −4 M?

A: The pH scale is used to measure the acidity and basicity of aqueous solutions. pH is the negative…

Q: For each of the following entities • Identify it as a strong or weak acid. Select the correct arrow…

A:

Q: n aqueous solution at 25 °C has a pOH of 9.8. Calculate the pH. Be sure your answer has the correct…

A: This is the question of ionic calculation

Q: Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH.…

A: Concentration of each given acid = 0.1 M (c) We know that -> [H+] = √(Ka ×c)

Q: Which of the following characteristics of perchlorate (CIO4) best explains why perchloric acid…

A:

Q: Indicate whether the chemical species HC6H5O72- acts as an acid or base when added to water.

A: Acid : when acid is added to water , it gives hydrogen ion (H+) in aqueous solution.  Eg. :  HCl…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.46 M solution…

A: For first ionization, [H+] = (Ka1 * C)^1/2 where C = initial concentration of acid = 0.46 M [H+] =…

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.