Using chemical equations, show how the triprotic acid H3PO4H3PO4 ionizes in water. Phases are optional. Ka1:   Ka2:   Ka3:

Q: Determine the pH of a 0.21 M solution of pyridinium nitrate (C5H5NHNO3) at 25°C. [Pyridinium nitrate…

A: To calculate pH , we need to calculate the concentration of hydronium ion given by pyridinium ion on…

Q: If 0.235 g of KHP (potassium hydrogen phthalate) require 15.5 mL of NaOH solution to neutralize it,…

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Q: What are the conjugate base and conjugate acid for HSO4−? What is the term used to describe species…

A: The term conjugate acid can be defined as the compound which gets formed when and acid reacts with…

Q: A solution of sulfuric acid (H2SO4) has a concentration of 0.0075 M. Calculate the pH of this…

A: Given, Concentration of H2SO4 solution = [H2SO4] =  0.0075 M pH of the solution = ? Note:  Sulfuric…

Q: 5.07 g of HCl(g) is dissolved in water to make a 220 mL solution. Calculate the pH of the solution.

A: Since you have posted multiple questions we are answering first question for remaining question to…

Q: Is H2Cr2O2 an acid, base, or neutral? please justify your answer with an equation showing its…

A: The question is based on the concept of chemical substances  we need to identify the nature of the…

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

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Q: Boric acid dissolves in water according to the equation B(OH)3(aq) + H₂O → B(OH)2 (aq) + H+ (aq)…

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Q: Rainwater is found to be slightly acidic compared to pure water. It has a hydrogen concentration of…

A: Given: H+ of rainwater = 10-5.6

Q: How does the hydronium ion concentration, (H3O+) change when the pH of a solution is lowered from…

A: pH = -log[H3O+]  log[H3O+] = -pH  so, [H3O+] = 10-pH

Q: (b) If the pH of water in a lake falls below a value of 5, fish often fail to reproduce. How much…

A: pH is a measure of acidity. pH = – log[H+] [H+]= 10–pH

Q: Morphine has the formula C17H19NO3. It is a base and accepts one proton per molecule. It is isolated…

A: Given information is as follows: Volume of sulfuric acid = 8.92 mL = 0.00892 L Concentration of…

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: Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are…

A: Since the volume and concentration of acid taken is same for all acids  Hence the moles of all acid…

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: 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…

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Q: A 1.800-L sample of hydrogen fluoride gas at 20.0° C and 0.750 atm pressure was dissolved in enough…

A: Given that : Volume of solution(V) = 1.8 L Temperature(T) = 20°C = 293 K Pressure(P) = 0.750 atm

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

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Q: If 0.235 g of KHP (potassium hydrogen phthalate) require 15.51 mL of NaOH solution to neutralize it,…

A: For the neutralization number of mmols of NaOH = number of mmols of KHP Number of mols = Molarity x…

Q: Arsenic acid, H3AsO4, is used industrially to manufacture insecticides. Arsenic acid is a polyprotic…

A: Given, Arsenic acid is a polyprotic acid with Ka1 = 2.5 × 10–4 Arsenic acid is a polyprotic acid…

Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

A: pH of solution is defined as negative logarithm of hydrogen ions  present in solution.

Q: Determine the pH of a solution that is 0.00542 M HCl and 0.0513 M HClO2. The Ka of HClO2 is 1.1 ×…

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Q: A solution is made by dissolving 16.7 g of CH₃NH₃NO₃ in 500.0 mL of water.   a)Write the acidic…

A: The compound given is CH3NH3NO3. Given : Mass of CH3NH3NO3 = 16.7 g And volume of solution = 500.0…

Q: Consider solutions of the following salts: NH4NO3 KNO3 Al(NO3) For each of the above, state whether…

A: A question based on nature of salt, which is to be accomplished.

Q: Determine the OH− in a solution with a pH of 3.7.

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Q: Describe superacid and derive the acidity function(HO) to represent it

A: The objective of this question is to explain the superacid is a very strong acid. It is a compound…

Q: Acidity of a solution is determined by the concentration H of hydrogen ions in the solution…

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Q: The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the…

A: " Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

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.