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

Q: The pHpH scale for acidity is defined by pH=−log[H+]pH=-log[H+] where [H+][H+] is the concentration…

A: pH scale for acidity is defined by pH= −log [H+], where [H+] is the concentration of hydrogen ions…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00640 M HIO4 pH =   (b)…

A: We will find H+ concentration and then calculate pH.

Q: Carbon dioxide in the atmosphere dissolves in raindrops toproduce carbonic acid (H2CO3), causing the…

A: To find the range of [H+] and [OH-] in the raindrops can be given by- Since, Product of the both…

Q: Consider the aqueous solutions of two weak acids depicted in diagrams A and B. (a) What is the…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: LIOH(aq) is classified as a base. The reaction equation with water utilizes which of the following…

A: The compounds that on dissociation in aqueous solution give H+ ions or accept electrons are called…

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.34. What is the Ka of the acid?

A:

Q: The pH of a 0.154 M solution of a weak acid, HB, is 2.72. What is K, for the weak acid?

A:

Q: what is the pH of a 0.15 mol/L solution of hypochlorous acid? the answer should be written to two…

A:

Q: determine the lewis acid and lewis base OH- (aq) + CO2 (aq) → HCO3- (aq) OH- is the:

A: Solution- CO2 accepts a pair of electrons from the O2− ion in OH- to form the bicarbonate ion. ,…

Q: The pH of an aqueous solution of 0.494 M morphine (a weak base with the formula C17H1903N) is

A: We have to calculate the pH of solution

Q: 6.)Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.

A:

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.292 M CH3NH3* and 0.335…

A:

Q: Calculate the pH of a solution when3.78grams of HCl was placed in 150.25 mL of water. HCl is a…

A: Solution -

Q: Determine the pH of each of the following solutions. Ka and Kb  values are given in the following…

A: a)  Molarity of Hydrazine, H2NNH2 = 0.0084 M  Kb for Hydrazine =1.3×10−6  pH of Hydrazine, H2NNH2 =…

Q: The ka of an unknown acid, HYO₂,  is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1…

A: The objective of this question is to calculate the pH of a 0.1 M solution of an unknown acid HYO₂,…

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.