Which of the following are weak acids? Mark all that apply.

Q: Write all the species (except water) that are present in a phosphoric acid solution. Indicate which…

A:

Q: How can we identify Conjugate Acids and Bases?

A: A number of theories have been proposed to explain what an acid or base is. Bronsted-Lowry's concept…

Q: Illustrate using an equation, the meaning of the terms: conjugate acid and conjugate base. Give…

A: The question is based on the concept of conjugate acid & base .

Q: If you know the [OH−], how can you determine the pH of a solution? Essay answers are limited to…

A: pOH can be calculated from the [OH−] as follows, pOH = - log [OH−]

Q: Does

A: Strong acid which break completely into ions while weak acid which do not break into ions

Q: Which of the following bases exhibit negligible behavior as a base?

A: Acid is a species that gives H+ ions in a solution. The base is a substance that gives the OH- ions…

Q: State the process to determine which conjugate base is more stable ?

A: Those acids which donate a proton (H+) are called the conjugate base. Those bases which can accept…

Q: Give examples of species which donot behave as Lewis acid or Lewid base?

A: Electron pair acceptors are known as Lewis acid. They are electrophilic in nature that means they…

Q: each of the following as a strong acid or a weak acid and indicate how each should be written in…

A: The main difference between a strong acid and weak acid is that strong acids are 100 % ionizable in…

Q: Which of the following is the strongest base?

A:

Q: Arrange the following in increasing order of acid strength. Rationalize your answer.

A: - I and - R effect increase acid strength. + I and + R effect decreases acid strength.

Q: Make a journal entry about the idea below.  "An acid cannot exist in the absence of a base." Is…

A: This statement is false.

Q: Justify the statement that water behaves like an acid and also like a base on the basis of protonic…

A: In aqueous solution, water looks like: H2O + H2O     ⇌   H3O+ +  OH-

Q: In most solutions containing a strong or weak acid, the autoionization of water can be neglected…

A: Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

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

A:

Q: Without doing any calculations, which of the following acids, if in solutions of equal…

A: 11.  Ka is the ratio of  product of concentration of products raised to their stoichiometric…

Q: Which one of the following is a stronger base? Explain why in the space provided.

A: In Structure I, lone pairs on the nitrogen atom are localized whereas in Structure II, lone pairs…

Q: Determine which polyprotic acid from the list is the unknown acid.

A:

Q: Fill in the missing chemical formulae in the tables below. conjugate acid conjugate base HCO, "oa'H…

A:

Q: a) Give an example of a substance that is a base in two ofthe three acid-base definitions, but not…

A: The substances which generates H+ ions in the solution are termed as acid whereas the species which…

Q: e preparations of two aqueous solutions are described in the table below. For each solution, write…

A: Acids are defined as which give H + in the solution and base is defined as which gives OH- in the…

Q: Determine whether each of the following is true or false for a weak base.

A: According to BRONSTED and Lowery, relationship between the strength of an base and the strength of…

Q: The relationship between [OH] and basicity is?

A:

Q: Choose one of the solutions represented. Identify the solution as a weak acid, a strong acid, or a…

A: We know that *Strong acids or Strong bases dissociate completly into ions when dissolved in water…

Q: A Hydrochloric acid is an example of a strong acid. Determine its [OH-], pH and pOH if the…

A: Higher concentrations of strong acids ( equal or more than 1M) should be expressed in Molarity…

Q: A weak monoprotic acid is 4.3% ionized in solution at equilibrium. Find the pH of the solution and…

A: The pH of a solution is the negative logarithmic of hydronium ion concentration in the solution.

Q: pH of this at 0.033

A: In this question we have to calculate the pH of at 0.033 M. pH for a salt is calculated by:…

Q: Which of the following is a correct conjugate acid-base pair?

A: Given,                HF  +  NH3  <------>  NH4+  +  F-   Required,                    Correct…

Q: Write ionization equations for a weak acid and its coniugate base. Show that adding these two…

A: Acids and bases can generally be classified under two categories, namely strong acids and bases and…

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: n acid or base in

A:

Q: HF a strong acid, justify your answer.

A: HF is a weak acid, because its ability to dissociate to donate proton is low. It is not strong…

Q: Which of the following statements is correct concerning the strength of acids:

A: In case of oxyacids with a similar number of O atoms, the acidic nature depends on the…

Q: How can I determine whether an acid is a strong acid or a weak acid?

A:

Q: Compute the pOH, [H3O+], and [OH-] of soda drink if its pH value is 2.

A: Given  PH = 2  POH , [ H3O+] , [ OH- ] = ?

Q: Which of the following pairs of species is nota conjugate acid-base pair?

A:

Q: Which of the following weak acid solutions is the strongest acid?

A:

Q: Define about weak acid ?

A: Define about weak acid

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: Calculate the [OH-] of a solution with 10.0 M H3O+ and classify as acidic, basic, or neutral.

A: Given : Concentration of H3O+ in the solution = 10.0 M

Q: Criteria of conjugate acid base pair.please explain?

A: Given: Conjugate acid base pair.

Q: What is the definition of acids and bases according to Arrhenius, Lewis and Bronsted and Lowry and…

A: Arrhenius theory of acid and base : It was proposed in 1887. According to this theory, an acid is a…

Q: IDENTIFY THE CONJUGATE ACID-BASE PAIRS. Show complete solution.

A: The solution is given below -

Q: Arrange the following acids according to their strength starting from the weakest to the strongest…

A: Strong acid is substance which release hydrogen ions when dissolved in water and weak acid is…

Q: A strong acid has a weak bond to its acidic proton, where as a weak acid has a strong bond to its…

A: Strong acids can provide hydronium ion easily but weak acids can not provide hydronium ion easily.

Q: In H₂O, HF is weak and the other hydrohalic acids areequally strong. In NH₃, however, all the…

A: Solution-When we say that an acid is a strong acid we mean that, that specific aciddissociates…

Q: Define and give an example of (a) A weak acid, (b) A weak base

A: Definition of weak acid and weak base with example is given below

Q: he chemical formulas of the species that will act as of the species that will act as neither acids…

A: (1) We have: 0.7 mol of HCl is added to 1.0 L of 0.7 M NH3 solution.  The chemical equation for 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.