From the list of the given compounds, choose the strong acid in an aqueous solution. H, SO, CH;CO,H KNO, LIOH

Q: Is sodium bicarbonate an acid or a base? how do you know?

A: Answer:- This question is answered by using the simple concept of nature of salts. The salt formed…

Q: The pH of an acidic solution is 5.67. What is [H⁺]?

A: Given that - pH of the Solution is = 5.67    Now, pH is the negative logarithm of Hydrogen ion or…

Q: What is the correct net ion equation for the following reaction between acetic acid and sodium…

A: Answer - A net ionic equation shows only the chemical species that are involved in a reaction, while…

Q: Calculate the pH corresponding to each of the pOH values listed, and indicate whether each solution…

A: The relationship between pH and pOH is given by  pH = 14 - pOH  If the solution is having pH > 7…

Q: Calculate the pH of the resulting solution if 22.0 mL of 0.220 M HCl(aq) is added to 27.0 mL of…

A:

Q: Which equation shows a weak acid in water? O LIOH(s) –-> Li* (aq) + OH(aq) O HF(aq) + H,0(1) CI…

A: Weak acid is an acid that dissociates weakly i. e. it forms very low concentration of H+ in the…

Q: The formula for the pH of a solution of hydronium ions is given by the logarithmic equation pH=−log​…

A: pH is equal to negative logarithmic of hydrogen ion concentration

Q: The pH of a solution is 5.2, what is the [OH] concentration?

A: Given pH of the solution = 5.2 In order to find [OH-] concentration, we have to calculate pOH from…

Q: How do I calculate the [OH] with the given data? Do you start by calculating moles of HCL and then…

A:

Q: What is the concentration of HCN(aq) in the solution?

A: pH is given by the negative logarithm of [H+].

Q: is the Arrhenius definition of an acid and a base? O a An acid contains hydrogen; a base contains a…

A: The concept of Arrhenius acid base is applicable for only aqueous solution.

Q: An aq solution has a hydronium ion concentration 2.0 x 10^ -7. What is the pH?

A: The concentration of hydronium ion, [H3O+] = 2.0×10−7 M

Q: Classify the acidity of perchloric acid, HClO4, based on its reactivity in aqueous solution. Choose…

A: Perchloric acid is strong acid in aqueous solution. It dissociates in the form of H+ and ClO4-.

Q: 7. What are the conjugate base and conjugate acid for HSO, ? What is the term used to describe…

A: Conjugate acid is formed when we add protons to a base and conjugate base is formed when proton is…

Q: A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?

A:

Q: A 0.261 g sample of NaHC2O4 (one acidic proton) required 17.5 mL of sodium hydroxide solution for…

A: The complete balanced Chemical Reaction is - NaHC2O4 + NaOH ----> Na3C2O4 + H2O Thus, one mole of…

Q: In the Brønsted–Lowry concept of acids and bases, acid–base reactions are viewed as proton-transfer…

A: In the Brønsted–Lowry concept of acids and bases, acid–base reactions are viewed as proton-transfer…

Q: In 200 words or less, give an example of an acid or base found or used in the real-world aside from…

A: Ammonia (NH3) is an example of a base found and used in the real-world. Ammonia is a colorless gas…

Q: acidic

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Q: The pOH of an acidic solution is 12.17. What is [OH⁻]?

A: Given that, pOH= 12.17 then, [OH-] = ?

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: When we write and balance the chemical reaction, then there is a rule is applicable behind this…

Q: Calculate the pH of an aqueous solution of 0.0644 M potassium sulfite. pH =

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: The pOH of a solution is 3.21. What is the OH⁻ concentration in the solution?

A:

Q: The pOH of an acidic solution is 11.55. What is [OH 1?

A: The pOH of the solution is = 11.55 The hydroxide ion concentration of the solution is =?

Q: Complete the balanced chemical reaction for the following weak base with a strong acid. In this…

A: According to Bronsted-lowry concept : An acid is defined as a substance which has a tendency to…

Q: When solid sodium hydroxide, a strong base, is dissolved in water which of the following species is…

A: A multiple choice question based on dissociation concept, which is to be accomplished.

Q: Write the equation that describes the equilibrium that exists when nitric acid dissolves in water.…

A: Acids on dissolving in water dissociates into ions. Hence Nitric acid will ionise into ions when…

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: Complete the balanced molecular reaction for the following weak acid with a strong base:…

A: We have to balance a given molecular reaction between a weak acid and a strong base.

Q: Complete the balanced molecular reaction for the following weak acid with a strong base: HC2H;O2(aq)…

A:

Q: the pH of a mysterious solution has an H+ concent that the solution is most likely a

A: The acidic or basic nature of a solution is determined by its pH value. pH measures the…

Q: The normal pH of blood is 7.4. What is the [H+] of normal blood? Is it acidic, basic, or neutral?

A: Answer :-  a) The [H+] of normal blood = 4.0 × 10-8 (M)  b) The nature of Normal Blood = Basic…

Q: The pH of an acidic solution is 5.43. What is [H⁺

A:

Q: The pH scale for acidity is defined by pH =- log1o[H] where [H ]is the concentration of hydrog ions…

A: Given  PH   =  8.45 [H+] =   ?

Q: Complete the balanced chemical reaction for the following weak base with a strong acid. In this…

A: Since, NH3 is a weak base and HCl is an acid, so reaction between acid and base forms salt (ammonium…

Q: 83. Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 =…

A: We know that PH = 14 - POH

Q: The pH reading of a sample of each substance is given. Calculate the hydrogen ion concentration of…

A: pH of any substance is defined as the, pH = -log[H+] = -log[hydrogen ion concentration] a)…

Q: Complete the following neutralization reaction between an acid and a base. Do not incluc not write…

A: Balance chemical equation is defined as which has equal number of atoms or ions in both sides…

Q: The pH scale for acidity is defined by pH = - log10 H+] where H is the concentration of hydrogen…

A:

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: In the given reaction Weak acid is CH3NH3Cl Strong base is NaOH

Q: A solution has a hydrogen ion concentration of 1 x 10^6 M. What is the pH?

A: The negative logarithm of concentration of hydrogen ion is known as pH. pH = – log [H+]

Q: The pOH of an acidic solution is 10.15. What is [OH⁻]?

A: pOH of any solution is given by  pOH = -log[OH- ] where [OH- ] = concentration of OH- ions in the…

Q: Use the References to access impo Classify each of the following as a strong acid or a weak acid.…

A: Strong Acid: An acid which completely dissociates in aqueous solution is called strong acid. e.g.…

Q: true or false: The anion of a strong acid can act as a base.

A: Strong acid is the one which dissociates completely in water. According to Arrhenius concept strong…

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.