What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=4.6×10−9 M?

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is

A: pOH = - log[OH-] pH + pOH = 14

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H3O+],[H3⁢O+], of 4.18×10−6…

A: The pH of the solution is = 5.38

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A:

Q: what is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^-3 M?

A: [OH-] = 1.0×10-3 M pH = ?

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 2.6 × 10⁻⁴ M. What is the…

A:

Q: What are the conjugate base and conjugate acid for HSO4−? What is the term used to describe species…

A: The term conjugate acid can be defined as the compound which gets formed when and acid reacts with…

Q: What concentration of sodium hydroxide is needed to give an aqueous solution with a pH of 10.210?…

A: NaOH   →  Sodium Hydroxide NaOH  → It is strong BaseSo it will completely dissociate NaOH   ⇌ Na++…

Q: * pH of a Strong Acid, a Weak Acid The pH of a solution is the negative logarithm of the molar…

A: Ph of given solution= 1.

Q: What is the pH of 425.0 mL of an aqueous solution containing 0.559 g of HCI? Round your answer to 3…

A: Volume= 425 ml  1 L = 1000 ml so  425 ml =0.425 L  Volume= 0.425 L  Weight of HCl = 0.559 gram.…

Q: Ethanolamine, HOC₂H4NH₂, is a viscous liquid with an ammonia-like odor; it is used to remove…

A: Answer is given below in two part

Q: The pH of a basic solution is 10.41. What is [OH⁻]?

A: pH of a solution is the parameter which is used to define the acidity or basicity of a solution.…

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

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.5 × 10⁻⁴ M. What is the…

A: Given, Concentration of hydroxide ion = [OH-] = 3.5 × 10-4 M Concentration of hydronium ion = [H3O+]…

Q: Enter your answer in the provided box. Calculate the pH of a 0.083 M Ba(OH)2 solution. pH =

A: The given base is strong base that dissociates completely into ions as,

Q: The normal pH range for human blood is 7.35 – 7.45. The patient’s blood has a concentration of…

A: Normal pH range for human blood =  7.35 – 7.45 [H3O+] = 8.91 x 10-8 M.

Q: The pH of an acidic solution is 5.75. What is [OH⁻]?

A:

Q: What is the pOH of an aqueous solution of 0.272 M hydroiodic acid? pOH =____

A: PH is the power of Hydrogen  PH= -log[H+] Ph+poh= 14 HI is a strong  acid so we can Calculate it's…

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 2.5 × 10⁻⁴ M. What is the…

A:

Q: What is the pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M

A: The pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M is to be calculated

Q: Find the concentration of hydroxide, OH-, ions in a 0.100 M solution of HOAc, acetic acid

A:

Q: An aqueous solution has a hydroxide ion concentration of 5.0 x 10 8 M. What is the pH of this…

A: Given [OH-] = 5 × 10-8 M

Q: Calculate the pH of the resulting solution if 27.0 mL of 0.270 M HCl(aq) is added to 37.0 mL of…

A: we need to calculate the pH of the given solutions

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: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

A: pH of solution is defined as negative logarithm of hydrogen ions  present in solution.

Q: •2calculate the pH value of 0.01M KOH solution.

A: Q. Given KOH solution [ KOH stands for Potassium Hydroxide]C = 0.01 M ( Concentration of KOH )Here…

Q: The pH of a solution at 25°C in which [OH–] = 4.0 × 10–5 M is: 4.40 9.60 4.80 4.00 None of these…

A: Using pOH = -log[OH-] And pH = 14 - pOH

Q: The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the…

A: " Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

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.