Describe amphoteric behavior and give an example.

Q: The pH scale is used to measure the acidity or alkalinity of a solution. The scale ranges from 0 to…

A: Formula to calculate the pH…

Q: For ClO−, write an equation that shows how the anion acts as a base.

A: Arrhenius Acids and Bases:Acid release hydrogen ion in water, base release hydroxide ions in…

Q: How many of these species are amphiprotic? HCO3 HNO2 OH NH3 PO32- Select one: 1 O 2 O 3 4 O 5

A: Amphioprotic : amphioprotic species are the species that can act as acid and as well base ie the…

Q: Why is ammonia described as a Brønsted-Lowry base andnot an Arrhenius base?

A: According to  Arrhenius base theory bases are hydroxide ion donors.

Q: Determine the pH of the following: a single solution prepared to final concentrations of 0.01469 M…

A: pH is the negative logarithm of hydrogen ion concentration. When an acid is mixed with a base, both…

Q: What is normal physiological pH range?

A: To write: The normal physiological pH range?

Q: The molar concentration of OH in a water solution is 1.0 ´ 10 -9. The pH of the solution is

A:

Q: Complete and balance the equations according to acid and base behavior in water. Phases are…

A: According to Arrhenius theory, acid gives H+ ions and base gives OH- ions when dissolved in water.

Q: Which refers to a measure of how acidic or basic a solution is? O pH O solubility O reactiveness O…

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Q: Write an equation for the ionization of the following acids in water: a. HCl, a strong acid…

A: The pair of acid and base differing from each other by just one proton is called conjugate acid-base…

Q: g) H3P h) КОН

A: H3P=  pka value of PH3 is 27. It means that, pka value is more, so this is weak acid.

Q: Explain, in terms of ions, why the colorless vinegar is classified as an Arrhenius acid.

A: question 5.  Given :- HC2H3O2 + H2O <=> H3O+ + C2H3O2-   To explain :- why vinegar is…

Q: List the factors that affect acid strength?

A: Acid is the one which accepts the electrons according to Lewis theory. According to Bronsted theory…

Q: Classify the following aqueous solutions as strongly acidic, weakly acidic, neutral, weakly basic,…

A: (a) battery acid, pH 0  ----> strongly acidic. (b) lime juice, pH 2.7  -----> strongly acidic.…

Q: Determine the [H3O+] concentration and whether the solution is acidic, basic, or neutral : a) [OH-]…

A:

Q: . 60.0 mg of codeine sulfate (C18H21NO3H)2SO4 is dissolved in 10.0 mL of water. Calculate the…

A: The given solution contains 60mg of codeine sulphate in 10m1 of water. Also given the molecular…

Q: Use the table to calculate the pH of pure water at a. 0°С b. 25 °C с. 100°C

A: The data given is,

Q: Calculate the percent ionization of a 0.355 M solution of nitrous acid. % Ionization =

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Q: What are the Four factors affect the acidity of HA ?

A:

Q: Define amphoteric compounds, and give example with chemical equations?

A: An amphoteric substance is a substance that has the ability to act either as an acid or a base.…

Q: Write formulas for the Lewis acid and the Lewis base that react to form H3NAlBr3.

A: According to the Lewis Concept of acid-base:-  Acids are electron acceptor  bases are electron donor

Q: с) HF d) HNO2

A: C) HF is a weak acid D) HNO2  is a weak acid Ka of HF and HNO2 are 6.6×10-4 and 7.2×10-4

Q: HSO4– is amphoteric. Write the equation that takes place between HSO4– and OH–.

A: Given : HSO4- is amphoteric, which means that it can act both as an acid or a base.

Q: Everything I need to know about hydrolysis,acid-base properties of salt.

A: I have to tell about the hydrolysis and acid-base properties of salt.

Q: classify the solution as acidic, basic, or neutral. [H3O*] [OH] pH РОН Classification 6.3x 104 2.5x…

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Q: What are the amphiprotic species?

A: A chemical substance which can release or accepts a proton or hydronium ion in aqueous solution to…

Q: Calculate the percent ionization of a 0.489 M solution of hypochlorous acid. % Ionization =

A:

Q: What is an amphiprotic species? Name one and write bal-anced equations that show why it is…

A: A chemical species is a substance that can undergo many reactions. The type of reaction they can…

Q: Calculate the pH of each of the following solutions: (a) 0.0010 M HCl (b) 0.76 M KOH

A: The pH and pOH of the solution can be determine by using the formula is as follows;

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

A:

Q: The pH scale is used to measure the acidity or alkalinity of a solution. The scale ranges from 0 to…

A: pH is a measure of acidity of solution. Lesser the pH,more acidic the substance will be. It is…

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: Calculate [H3O+] and [OH-] for each solution at 25 °C.a. pH = 8.55 b. pH = 11.23 c. pH = 2.87

A: The pH is the measurement used to identify the compound as acidic or basic. The pH of a compound can…

Q: The pH scale is used to measure the acidity or alkalinity of a solution. The scale ranges from 0 to…

A: Since pH = -log[H+], Convert this logarithmic expression to an exponential expression in order to…

Q: What mass of HClO4 must be present in 0.500 L of solution to obtain a solution with each pH value?a.…

A: The answer for part (a) is given below. Kindly repost the other parts as separate one.

Q: Define the term amphoteric?

A: Compounds that have a pH lower than 7, are sour in taste, donate a proton, and can turn blue litmus…

Q: How can a substance, like water, show its amphiprotic nature?  What information can be derived from…

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Q: how does a basic anion interact with water? provide a net ionic equation for a basic anion

A: Answer: Basic anions are the conjugate base of weak acids. For example: CH3COO-, HCOO-, F- etc.

Q: Write the structures and names for two classes of weak acids and two classes of weak bases.

A: Conjugate acids of weak bases are always  weak acids and conjugate bases of weak acids are always…

Q: What causes heartburn? What are some possible ways to alleviate heartburn?

A: Heartburn is your chest or throat's painful burning sensation. Heartburn happens when stomach acid…

Q: 1. Define and give an example of a monoprotic acid. 2. Define and give an example of a diprotic…

A: There are four questions are given but I am solving first three questions according to the…

Q: Commercial ammonia generally has a mass percent concentration of 25% NH3, which translates to 14.7 M…

A: 25 % NH3 solution has a concentration of 14.7 M . We have to calculate the pH and pOH of a quarter…

Q: 12. Define the term 'pH'. What does water ionize into? What is an acid? What is a base? If something…

A: This question is related to acid-base chemistry. Acid convert blue litmus in to red.

Q: Given the amphiprotic nature of water, why is water neutral? Provide 5 sentences to justify your…

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Q: Complete and balance the equations according to acid and base behavior in water. Phases are…

A: There will be a complete reaction with water, when the solute is a strong acid (e.g., HClO4, H2SO4,…

Q: What word is used to describe a chemical that can behave like an acid OR a base?

A: amphoteric is used to describe a chemical that can behave like an acid or base some of the oxides…

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.