A 0.0500 M solution of a base is 7.5% ionized. Calculate the base ionization constant Kb.

Q: The pH of a basic solution is 12.03. What is [H⁺]?

A: Given: pH of solution = 12.03

Q: The weak acid HZ has a Ka of 2.55×10−4. Calculate the pH of 0.040 M HZ.

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.9x10? M. The hydronium ion…

A: Hydrogen (Hydronium) ion concentration and hydroxide ion concentration has Following relationship -…

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10^-6 M.

A: Given that, in a solution, the hydrogen ion concentration is [H+] = 4.5×10-6 M. We have to calculate…

Q: The pH of a basic solution is 10.61. What is [H⁺]?

A:

Q: The pH of rainwater in a polluted area was found to be 3.50. What is the hydrogen-ion concentration…

A: The given data : The pH of rainwater = 3.50 To determine = The concentration of hydrogen ions.

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: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

A:

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

A:

Q: -69 The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3x 10. Calculate the pH of a…

A: Consider the dissociation of hypobromous acid is as follows:                       HBrO   →     H+…

Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

A:

Q: Determine the pH of a solution that is 0.00482 M HCl0.00482 M HCl and 0.0304 M HClO2. The Ka of…

A: Given -> Molarity of HCl = 0.00482 M Molarity of HClO2 = 0.0304 M Ka = 1.1 × 10-2

Q: Calculate the pH of a solution that is 1.9 x 10^-2 M Ba(OH)2.

A: pH of a solution is equal to the negative logarithm of hydronium ion concentration while pOH is…

Q: pH of a 0.30 M solution of a weak base B is 9.02. What is the K, of the base? Be sure your answer…

A:

Q: The hydrogen ion concentration of a basic solution is 9.70 × 10-10 M. What is the pH of the…

A:

Q: The ionization constant for water (Kw) is 2.9 × 10−14 at 40 °C. Calculate the pH of pure water at 40…

A: Autoionization of water takes place as follows: The product of the concentration of the hydronium…

Q: Explain the principle, STRONG ACID + STRONG BASE & WEAK ACID + WEAK BASE in terms of the tendencies…

A: The substance which donates a proton acts as an acid and the substance which accepts a proton acts…

Q: Write the structures and names for two classes of weak acids and two classes of weak bases.

A: Conjugate acids of weak bases are always  weak acids and conjugate bases of weak acids are always…

Q: Classify the basicity of magnesium hydroxide, Mg(OH)2, based on its reactivity in aqueous solution.…

A: Weak base and strong base: Weak base: (partial dissociation) week base is a compound that is…

Q: The pH of a 0.30M solution of a weak base is 10.66 . What is the Kb of the base?

A:

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,…

Q: Define the conjugate and describe how you would identify the conjugate of a weak acid.

A:

Q: The pH of a basic solution is 12.19. What is [OH⁻]?

A: pH of the basic solution = 12.19 [OH-] = ?

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.