The pH of a basic solution is 12.39. What is [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 pH of a 0.0039 M solution of Ca(OH), is

A: Provided concentration 0.0039M One Ca(OH)2 gives two OH-  So, 1 M Ca(OH)2 gives= 2M Ca(OH)2 Hence,…

Q: 12.9 g of NaOH was dissolved in water affording a final volume of 250 mL. What is the pH of the…

A: Given :-  mass of NaOH = 12.9 g  volume of solution = 250 mL  To calculate :-  pH of solution

Q: If an acid, HA, dissociates to 0.1% when added at a final concentration of 0.05M in water, that is:…

A: 1- First calculate the H3O+ ion concentration :  [H3O+] = ( Concentration ) × ( Degree of…

Q: The pH of an aqueous solution of 4.45x102 M ammonium bromide, NH,Br (aq), is This solution is

A: NH4Br is a salt of weak base and strong acid. We have to determine pH of an aqueous solution of…

Q: The pH of a 0.0030 M solution of Ca(OH), is

A:

Q: Calculate the pH of the solution, where the acetic acid is x10 stronger than acetate.

A: In chemistry, pH is defined as the potential of hydrogen ion. It is the negative logarithm of…

Q: The pH of an acidic solution is 4.03. What is [H⁺]?

A: Given : pH of acidic solution = 4.03 pH of the solution is the negative logarithm of concentration…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 6.3×10-2 M. The hydroxide ion…

A: EXPLANATION: At 25oC ,It is always true. GIVEN: To Solve: Hydroxide ion concentration(M)=?pH of…

Q: The pOH of a basic solution is 2.65. What is PH?

A: Given, the pOH of a basic solution, pOH =2.65we are asked to calculate the pH of the solution.

Q: The pH of 0.01 m Potassium hydrogen phthalate is

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.3×10-2 M. The hydronium ion…

A: Given : Hydroxide ion concentration [OH-] = 9.3 × 10-2 M.  a)  Hydronium ion concentration [H3O+] =…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 2.4×10-2 M. The hydronium ion…

A: By using hydronium ion and hydroxide ion concentration we can find pH and pOH of solution.

Q: How do I calculate pH of a salt? for example in 0.10 M NaClO4(aq)?

A: Salt are produced by the reaction of an acid and a base. For example, The pH of salt is given as :

Q: The pOH of a basic solution is 2.87. What is pH?

A: We have given that  pOH = 2.87  We know that  pH + pOH =14  pH = 14 - pOH        = 14 - 2.87   pH =…

Q: Calculate the pH for an aqueous solution having a hydrogen ion concentration of 2.15 × 10-3 M.

A: pH = -log[H+] where [H+] = hydrogen ion concentration  Hence substituting the values we get  pH =…

Q: The pH and pOH of 0.05 M of NaOH is ..

A:

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: If the hydroxide concentration of a solution is [OH-] = 4.67 X 10-8 what would the pH of that…

A: Given:The concentration of OH, [OH-] = 4.67 X 10-8To find:pH = ?

Q: The pH of an aqueous solution of 0.236 M sodium cyanide, NaCN (aq), is This solution is acidic,…

A: NaCN is salt of strong base and and weak acid. The chemical nature of the solution depends on the…

Q: The pH of an aqueous solution of 0.530 M methylamine (a weak base with the formula CH3NH2) is…

A:

Q: What is the pH of a solution that is 2.8×10−9 M in NaOH?

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.2×10-2 M. The hydronium ion…

A: Concentration of OH- in aqueous solution is 3.2*10-2M.

Q: The pH of an aqueous solution is 5, what would be the pOH of this solutions

A: pH + pOH = 14

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

Q: If a sample of a certain solution is determined to have a [H3O+] concentration of 5.6×10^−12…

A:

Q: Calculate the pH of the following solutions of strong acids: HNO3 0.0575 M

A: Here, we have to calculate the pH of 0.0575 M HNO3 solution.

Q: The pH of an aqueous solution of 0.124 M ammonium nitrate, NH4NO3 (aq), is ___________. This…

A:

Q: The pH of an acidic solution is 2.11. What is [H*]?

A:

Q: The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.

A: Since pKa for phenol is 9.98 and concentration of phenol is 0.508 M (given)

Q: What is the pH of a solution with a pOH of 2.4? Is the solution acidic or basic?

A: We have pOH as 2.4 , we have to calculate pH as well as nature of solution.

Q: The pH of a solution with a [OH–] concentration of 1.20 x10–6 M are___, respectively.

A:

Q: The pH of an acidic solution is 2.11. What is [H⁺]?

A: PH is defined as negative logarithm of concentration of [H+] ion. Given PH = 2.11

Q: The pH of an acidic solution is 4.17. What is pOH?

A: pH and POH is defined for acid and base. We have relation between them so we will use the same

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 5.1×10-² M. The hydronium ion…

A: Given:  [OH-] = 5.1 x 10-2 M  At 25°C :Kw = 10-14  Also, Kw = [H3O+][OH-]

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.4×10-2 M. The hydronium ion…

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 12.51. What is pOH?

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 4.6×10-² M. The hydronium ion…

A:

Q: The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated…

A: [CH4N2O] = 1.00 M pH = 7.050 Calculating the [H3O+] from the given pH value, pH = -log[H3O+] [H3O+]…

Q: The pH of a O.0086 M solution of Ca(OH)2 is

A: The negative logarithmic concentration of hydrogen ion concentration in as solution is called pH. It…

Q: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

A:

Q: The hydronium ion concentration in an aqueous solution at 25°C is 7.7×10-² M. The hydroxide ion…

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 2.1×10-3 M. The hydronium ion…

A: Given, The concentration of the hydroxide ion, [OH-] = 2.1×10-3 M Concentration of the hydronium…

Q: If the pOH for a solution is 3.00, what is the pH? Is the solution acidic or basic?

A: The acidity or basicity of an aqueous solution is specified by the scale is called pH scale. Its…

Q: The pH of a solution that has measured (H+) of 6.8*10^-9 M is

A: We have given that   [H+] = 6.8×10-9M  pH is measure the acidity and basicity of aqueous…

Q: What is the pH of a 0.200 M NaHCO, solution? The K, for HCO, is 5.6 x 1011

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.