If the ?b of a weak base is 4.6×10−6, what is the pH of a 0.17 M solution of this base?

Q: pH of an aqueous solution of 7.05×10-2 M sodium nitrite, NaNO2 (aq), is . This solution is

A: Given- Concentration of sodium nitrite= 7.05×10^-2M

Q: Calculate the pH of each of the following solutions. (a) 7.5 x 10-4 M Ba(OH)2: 11.1765 x 10l d…

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Q: A certain solution was found to have a pH of 5.50. Which of following statements is true about this…

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Q: what is the pH of a 0.00761 molar solution of HNO3?

A: Nitric acid is a strong acid that dissociates completely in aqueous solution.

Q: What is the pH of a solution that has an OH- ion concentration of 3.20 M?

A:

Q: If the pH is 13.2 what is the molarity?

A: The pH of a solution is mathematically expressed as: pH=-log[H+] where [H+] is the molarity of H+…

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: The pH of an acidic solution is 5.79. What is [OH⁻]?

A: Given: pH = 5.79 [ OH- ] =?

Q: If the pH of a solution of aluminum hydroxide is 9.85, what is the concentration of the aluminum…

A: Since the aluminium hydroxide completely dissociates. Hence the dissociation reaction will be…

Q: Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3

A: pH is the measure of the acidity or basicity of the solutions. pH ranges from 0 to 14. If the pH…

Q: The pH of an acidic solution is 2.83. What is [H⁺]?

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

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: The pH of an acidic solution is 4.47. What is [H⁺]?

A: pH is a quantitative measure of the acidity or basicity of aqueous or other liquid solutions. the…

Q: Methylamine is a weak base with a ?b of 4.4×10−4. Calculate the initial molar concentration of a…

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Q: If the pOH of a solution is 4.21, what is its pH?

A: pOH:- It is generally defined as the measure of hydroxide ion concentration in a solution. It is…

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.