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 =

Q: If the hydronium ion concentration of a weak acid is 6.32 x 10 M what is the pH?

A: Given :- concentration of hydronium ion = 6.32 x 10-4 M  To calculate :- pH of the solution

Q: The K, of a certain base is 4.4x107. What is the pH of a 0.30-M solution of this base?

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Q: The pH of an aqueous solution of 0.354 M hydrofluoric acid is

A: Hydrogen fluoride is a weak acid and its pKa value is = 3.17 The concentration of HF solution is =…

Q: What are Weak Bases ?

A: Weak base doesnot dissociate completely in their aqueous solution . They dissociate partially

Q: An aqueous HCl solution has a proton concentration equal to 6.00 mol/L. The HCl concentration in…

A: Molarity is defined as the number of moles per liter of the solution. It is expressed as mol/L.

Q: If the K, of a weak base is 7.2 × 10-6, what is the pH of a 0.33 M solution of this base? pH =

A: in this question given data is  α=KaC   ka×kb=10-14C=0.33MPH=-logH+ Apply the value given formula,…

Q: What are the pOH and the pH of a 0.0125-M solution of potassium hydroxide, KOH?

A: KOH is a strong mono basic base in nature which dissociates completely. Here the given concentration…

Q: The pH of a basic solution is 9.03. What is [H*]?

A:

Q: Which one of the following 1.0 M solutions would have the lowest pH?

A: D option is right. HF Ka provides a way to gauge the strength of an acid. Larger values signify…

Q: The pH of a basic solution is 9.93. What is [OH ]?

A:

Q: An aqueous solution has a hydronium ion concentration of 4.0 x 10/ M. What is the pH of this…

A: Answer: pH of a solution is the negative of logarithm of hydronium ion concentration.

Q: What is the pH of a solution with a hydrogen concentration of 8.6x10-2M?|

A:

Q: Calculate the pH of an aqueous solution of 0.0448 M potassium sulfite.

A: PH is defined as negative logarithms of hydrogen ion concentration.

Q: Determine the pH of a solution that contains 6.5x10-3 mol/L of OH- ions

A: pH :- It is defined as the negative logarithm to the base 10 of hydronium ion concentration…

Q: Determine the pH and pOH of a solution at 30 degree Celsius that has 0.32 mols of hydroxyl ions in…

A: Acidity of solution can be calculated from the value of pH.  Now, pH of solution can be calculate…

Q: The pH of a Solution is 1.411. what is the p OH? what is the [H30 ]? what is the TOM]?

A:

Q: if the concentration of OH- in an aqueous solution is 1.4 x10^-7 M, the concentration of H3O+ is…

A: Given;

Q: If a 5.6 L solution has a pH of 3.6, what will the pH be if the volume is increased to 7.2 L?

A: Given:PH of solution-1 = 3.6V1 = 5.6 L.V2 = 7.2 L

Q: A solution of sodium cyanide, NaCN, has a pH of 11.20. How many grams of NaCN are in 835 mL of a…

A:

Q: The hydrogen concentration of a solution is 1 x 10-4 M. What is the pH? pH = ____________ Is…

A: The hydrogen concentration of a solution is 1 x 10-4 M. pH = 4 This is an acid solution.

Q: The pH of an acidic solution is 3.07. What is [OH⁻]?

A: Given data is as follows:  The pH of the solution = 3.07 OH- = ? As we Know that; pH+pOH=14

Q: If the K, of a weak base is 2.7 x 10, what is the pH of a 0.30 M solution of this base?

A: Solution Ph may be a live of however acidic or basic is AN solution.It is measured in terms of…

Q: The pH of a basic solution is 9.03. What is [H1?

A: formula used:-  pH = -log[H+]

Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH  POH= -log[OH-]

Q: Indicate the pH of the following

A: pH = -log[H+]  pH + OH = 14

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: What is the pH of the following solutions? [OH-] = 9.1 × 10-3 M

A: We can only Calculate the pH of solution if we know the Hydrogen ion concentration of solution. To…

Q: If the K, of a weak base is 1.7 × 10-6, what is the pH of a 0.18 M solution of this base? pH =

A: pH of a substance represents the strength of an acid or base. If the pH is small, it is a strong…

Q: If the K, of a weak base is 2.4 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A: Given,  Base dissociation constant of base (say B) = Kb= 2.4 x 10-6  Molarity of base (B) = 0.27 M…

Q: The hydronium-ion concentration of a solution is 8.6 × 10-6 M. What is the solution pH?

A:

Q: From the list of the given compounds, choose the strong acid in an aqueous solution. Ο ΚΝO O NH,OH…

A: From Bronsted lowry concept of acid we know any substance which gives a proton in aqueous solution…

Q: Calculate the pH of an aqueous solution of 0.141 M potassium sulfite. pH = .

A:

Q: what is the pH of a solution that has the following H+ concentraion? 1.75 x 10^-5 mol/L

A:

Q: A solution of sodium acetate 1NaCH3COO2 has a pH of 9.70. What is the molarity of the solution?

A: pH scale is used to measure the acidity or basicity of the solution. If the solution is acidic in…

Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

A:

Q: The pH of a solution is 8.7. What are the pOH, [H3O+] and [OH−] of the solution?

A: Given data contains, pH of a solution is 8.7.

Q: The pH of an acidic solution is 6.75. What is pOH?

A:

Q: The pH of a basic solution is 9.77. What is [OH⁻]?

A: we know, pH + pOH = 14 pOH =  -log[OH-]

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: Determine the pH of a 0.13 M acetic acid solution. The K, of acetic acid is 1.8 X 10 5.

A:

Q: . The [H3O*] of a solution is 1.7 x 10°M. What is the [OH]? What is the pH? What is the pOH?

A: pH is used to determine the concentration of hydronium ion. pOH is used to determine the…

Q: What is the pH of an aqueous solution of 1.56x10² M perchloric acid? pH =

A:

Q: Which of the following are strong acids? HI HNO 3 HE HBr

A:

Q: The hydroxide ion concentration of an aqueous solution of 0.354 M hydrocyanic acid is

A:

Q: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

Q: The pH of a basic Solution is 10.27 what is [H+]?

A: At, 25°C, ionic product of water, Kw is given by: Kw = H+OH- = 10-14 Now, pH and pOH is given by: pH…

Q: The concentration of a strong monoprotic acid is 0.0010 M.  What is the [OH-]? What is the pH?

A: We calculate the pH of an acid or base using the Sorenson pH scale.…

Q: If the hydronium ion concentration is 2.5 x 10^-4, what is the pH ? __ Is this am acid or base ?

A: The concentration of hydronium ion (H3O+] = 2.5 × 10-4  pH = ?  This is an acid or base ?

Q: In a solution, [H+ ] = 3.25 x 10-10 M. What is its pH and is it considered an acid or a base?

A: A solution can be classified as acidic or basic or neutral depending on the pH value. For a solution…

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.