An unknown weak base with a concentration of 0.0910 M has a pH of 11.20. What is the Kb of this base?

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: How many moles of NH3 must be dissolved in water to give 622.4 mL of solution with a pH of 11.08? Ko…

A: Given -> Volume of solution= 622.4 ml = 0.6224 L (1L = 1000ml ) pH = 11.08  Kb = 1.8 × 10-5

Q: True or false? The pH of a popular soft drink is 2.3; thus the soft drink is basic.

A:

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

A:

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

Q: A solution of a weak acid has a concentration of 0.64 M and is found to have a pH of 3.77. What is…

A: The dissociation of a weak acid can be depicted as follows.           HA   +H2O ⇔    A-  +  H3O+I…

Q: An unknown weak acid with a concentration of 0.320 M has a pH of 5.600. What is the Ka of the weak…

A: HA  ↔ H+ + A-Writing equilibrium expression for the above weak acid,Ka = [H+] [A-][HA]  But at…

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: Would this likely be a pH be a pH of 1 or 5

A: pH will depend on how much lemon juice you squeeze into the water. If you add small amount of lemon…

Q: An unknown weak acid with a concentration of 0.071 M has a pH of 1.80. What is the Ka of the weak…

A: [acid]=[HA]=0.071MpH=1.80Ka=?

Q: What is the pH of a solution with molar concentration of Ht, [H*] = 1.0 x 10-9 M?

A:

Q: 7.30×10−7. What concentration of this base will produce a pH of 10.14?

A:

Q: when aspirin (C9H8O4) is taken by the mouth, the medicine enters the stomach, which has a ph of ~2.…

A: Aspirin, also known as acetylsalicylic acid, is a medication used to reduce pain, fever or…

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.