If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this base?

Q: What is the original molarity of a solution of ammonia whose pH is 10.48?

A: The original molarity of solution of ammonia whose pH is the 10.48 is calculated as follows

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: If the OH of a solution is 2.56 x 10^3 determine the H3O and the pH of the solution. Show formula.…

A: pH + pOH = 14pOH = -log10[OH-]  use this relation to find pH pH = - log10 [H+] = - log10 [H3O+]…

Q: What is the original molarity

A:

Q: The pH of an aqueous solution of 0.415 M aniline (a weak base with the formula C,H&NH,) is

A:

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N?

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9 To solve: pH of 0.65M…

Q: Which of the following solutions would be expected to have a pH of 7.00?

A:

Q: What is the pH of a 0.083 M solution of NaCN?

A: Given :- Concentration NaCN solution = 0.083 M  To calculate :- pH of solution

Q: What is the ph of a 0.214 M weak base solution? The Kb of the weak base is 0.000033.

A: Given :-  Concentration of weak base = 0.214 M  Kb = 0.000033  To calculate :-  pH of solution

Q: Determine the Kb of a weak base if a 0.19-M aqueous solution of the base at 25⁰C has a pH of 10.88

A: The question is based on the concept of equilibrium. we have been given a weak base  whose PH and…

Q: (Q7) If the initial concentration of the weak base ammonia in a solution is 0.401 M and the solution…

A:

Q: Find the pH of a KOH solution made by mixing 123 mg KOH with enough water to make 250 cm3 of…

A: Formula used:- pOH = 14-pH

Q: What is the pH of a 0.627 M weak base solution? The Kb of the weak base is 0.000066.

A: Given :- concentration of weak base solution = 0.627 M  Kb for weak base = 0.000066  To calculate :-…

Q: Rainwater that falls close to a power plant has H3O+ ion concentration of 6.25x10-4. What is the…

A: Formula of pH  pH = -log[H+] or pH = -log [H3O+]

Q: What is the pH of a 0.105 M solution of acetic acid? What is the percent ionization of the acid?

A:

Q: If the OH- ion concentration of a blood sample is 4.7 ×10−7 M, what is the pH of the blood sample?

A: We know that, pOH can be expressed as the negative logarithm of hydroxide ion concentration, i.e.…

Q: Calculate the pH of a 0.73 M sodium benzoate, C6H5COONa, solution. The Ka of Benzoic Acid, C6H5COOH,…

A: Given information: Ka of Benzoic Acid, C6H5COOH = 6.3 × 10−5 M. The concentration of Benzoic Acid,…

Q: What is the pH of 2.9x10 M

A:

Q: What are the names and formulas of the conjugate bases of these acids: (a) HNO2, (b) H2SO4, (c) H2S,…

A: A conjugate base is formed by the deprotonation of the corresponding acid. As H+ ion is released…

Q: What is the pH of a solution ten times as acidic as one of pH 5?

A:

Q: If the pH of a 25 °C NaOH solution is 9.00, what is the molarity of NaOH in that solution?

A:

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

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: An unknown weak base with a concentration of 0.0910 M has a pH of 10.90. What is the Kb of this…

A:

Q: The pH of an aqueous solution of 0.593 M dimethylamine (a weak base with the formula (CH3)2NH) is…

A:

Q: What is the pH of a 0.0138 M solution of pyridine (C5H5N), a weak base?

A:

Q: Calculate the pH of an aqueous solution where the [OH-] is 6.9 × 10^-9 M.

A:

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: What is the pH of a strong, monoprotic acid solution with a concentration of 0.763M?

A:

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

A:

Q: What is the pH of the solution if hydronium ion, H3O*, concentration is 3.0 x 10-9 M? Is the…

A: Given :- concentration of H3O+ i.e. [H3O+] = 3.0 × 10-9  To calculate :-  pH of solution  Nature of…

Q: The pH of a 0.016 M weak acid solution is 2.19. What is the percent ionization for this acid?

A:

Q: The pH for 1.0 × 10⁻³ M solution of cocaine, a weak base, is 9.70. Determine the value of Kb for…

A: Cocaine can be denoted as B. Concentration of OH- ions in cocaine can be determined as follows,

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: Sodium hydroxide is a strong base. What is pH of a 0.02M sodium hydroxide solution?

A:

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: Give the formula of the conjugate base of HSO^−4HSO4^−.   Give the formula for the conjugate acid…

A: Bronsted -Lowry Acid: A substance that donates proton (H+).   Bronsted -Lowry Base: A substance that…

Q: The pH of an aqueous solution of 0.470 M methylamine (a weak base with the formula CH3NH2) is

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: What is the pH of a 6.9 × 10⁻⁶ M KOH solution?

A: Use formula POH= -log(OH-) PH+POH=14 PH= 8.84

Q: The pH of an aqueous solution of 0.390 M methylamine (a weak base with the formula CH;NH2) is

A: 12.09

Q: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial…

A: Weak acid or base are those substance which does not dissociate 100%. The value of degree of…

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

A:

Q: The pH of 0.55 M aqueous solution ammonia HN3 at 25.0 degree C is 11.50. What is the value of Kb for…

A: NOTE : You have given HN3 instead of NH3. Since the pH is in basic zone, hence the specie will be…

Q: a 0.365g sample of HCl is dissolved in enough water to give 2.00 x 10 ^2 mL of solution. what is the…

A: pH = -log[H+] [H+] = [HCl] = Number of moles of HCl/Volume of solution (L) Number of moles of HCl =…

Q: What is the pH of a 0.25 M solution of methylamine hydrochloride, CH3NH3Cl?

A: The question is related to finding out the pH of a salt solution which is composed of weak base and…

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 ?

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.