The hydroxide ion concentration of an aqueous solution of 0.591 M acetic acid is [OH-] = M.

Q: Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

A: Conjugate pairs are acids and bases that differ only by a proton (H+).

Q: If the K, of a weak base is 3.8 x 10–6, what is the pH of a 0.21 M solution of this base? pH =

A: In this question we have to calculate the pH of Solution of base of given concentration, the Kb of…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 2.2×102 M. The hydroxide ion…

A:

Q: The pH of an orange juice is 3.33, calculate its [H+] and [OH-]

A: We can determine the hydronium and hydroxide ion concentration by applying the formula of pH =…

Q: Which of the following is an acid that will dissociate completely in water? × OHF NH3 HCI CH3COOH

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Q: In an aqueous solution at 25°C, if [H₃O⁺] = 5.3 × 10⁻⁴ M, then [OH⁻] is:

A: Given [H3O+] = 5.3*10^-4 M  Kw = [ H3O+][OH-]

Q: What is the pH of a solution that has [OH-] = 6.0 × 10−12 M?

A: pH: pH is  justified  as power of hydrogen. pH=-log[H+] Or in general we can say that it helps us to…

Q: What concentration of barium hydroxide is needed to give an aqueous solution with a pH of 10.330?…

A: We have given that  pH = 10.330  And the salt given is Ba(OH)2

Q: Determine the [H*|- JOH-|, and pOH of a solution with a pH of 7.88 at 25 °C. [r"| = M |OF| = M pOH =

A:

Q: According to the Brønsted-Lowry theory, label each of the following as an acid or a base. (a) HNO;…

A: Bronsted-Lowry theory: This theory basically focuses on proton transfer.. Bronsted-Lowry acid: It is…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.4 × 10⁻⁴ M, then [OH⁻] is:

A: The concentration of OH- can be calculated as:

Q: The hydronium ion concentration in an aqueous solution at 25°C is 2.8x1o-2 M. The hydroxide ion…

A:

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

A: To solve this problem we have to know about the strong and weak acids .

Q: H₂SO4

A: Acids are the substances which releases proton i.e. H+ in the solution. Acids often are electron…

Q: What is the pH of an aqueous solution of 3.18×10-2 M hydrochloric acid? pH =

A: Given that, [HCl] = 3.18×10-2 M pH = ?

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.3 × 10⁻⁴ M, then [OH⁻] is:

A: Here given---- [H3O+] = 2.3 ×10-4 M [OH-] = ? We know, dissociation of water occurs as---- H2O…

Q: 6) What is the pH and pOH of a solution with a [OH] of 7.79 X 10* M? Is the solution acidic, basic…

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Q: How to Identify and write equations foracid–base reactions.

A: How to Identify and write equations for acid-base reactions.

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

A:

Q: Calculate [OH -] and pH for each of the following solutions. (a) 0.0036 M RbOH [OH-] =  M pH =…

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Q: Assuming complete dissociation, what is the pH of a 0.348 M Ba(OH), solution? (Round your answer to…

A: Given  Concentration of Ba(OH)2  =  0.348 M  PH = ?

Q: What is the pH of an aqueous solution of 4.16×10-2 M hydrochloric acid? pH =

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

Q: An aqueous solution has a pOH of 9.48. (1) What is the pH of this solution? (2) What is the…

A: Given,An aqueous solution has a pH of 9.48.

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 7.6 × 10⁻⁴ M, then [OH⁻] is:

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.2 × 10⁻⁴ M, then [OH⁻] is:

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.3 × 10⁻⁴ M, then [OH⁻] is:

A: [OH-] = 7.7 x 10-11 M

Q: Calculate the  [ H3O+ ]  of an aqueous solution that is  3.0  ×  10−9  M in OH−.

A:

Q: What is the pH and concentration of OH- of 0.0200 M CH3COOH?

A: Given,Concentration of acetic acid is 0.0200M.Ka = 1.8×10-5.The equation will be:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.3 × 10⁻⁴ M, then [OH⁻] is:

A: Using ionic product of water, concentration of hydroxyl ion can be determined from the hydronium ion…

Q: alculate [OH -] and pH for each of the following solutions. (a) 0.0027 M NaOH [OH-] =  M pH =…

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 5.8 × 10⁻⁴ M. What is the…

A: Given: The concentration of hydroxide ion is 5.8 x 10-4 M The ionization constant (Kw) of water is…

Q: What is the pH of a solution which is 0.0230.023 M in weak base and 0.0370.037 M in the conjugate…

A: The question is based on the concept of determination of PH. We have been given a weak base solution…

Q: The pOH of a basic solution is 5.13. What is [OH⁻]?

A: pOH of basic solution = 5.13. Calculate concentration of OH- ion.

Q: he pH of a half-neutralized solution is 1.86. What is the value of [H+] and Ka?

A:

Q: What is the hydronium ion concentration in an aqueous hydrochloric acid solution that has a pOH of…

A: HCl is the strong acid.So in aqueous medium it can be easily donate proton easily.

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 7.4×103 M. The hydronium ion…

A: 1. We are having the hydroxide ion concentration as 7.4*10-3 M We have to calculate the hydronium…

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: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

A:

Q: What is the pH of an aqueous solution of 8.57E-2 M barium hydroxide? pH =

A:

Q: What is the pH of an aqueous solution with an OH- concentration of 0.00250 M?

A: Solution:- Given concentration of OH- = 0.00250 M  [OH-] = 0.00250 M  As we know, p(OH) = -…

Q: calculate the ph of the following solution and tellw hether it is acidic, basic, or neutral…

A: Given, [H3O+] = 4.53 ×10-8 M

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 5.2 × 10⁻⁴ M. What is the…

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 2.5 × 10⁻⁴ M. What is the…

A:

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.