What is the pH of a solution with a hydrogen ion concentration of 1.3 x 10-11?

Q: Calculate the hydrogen ion concentration of a Nitric acid solution with a pH of 2.11.

A:

Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

A:

Q: What is the pH of a hydrogen concentration of 1 x10 -6? pH pH

A: PH = -log[H+ ] Negative logarithm of H+ concentration  PH = power of hydrogens

Q: In a sample of lemon juice, H+ concentration is 3.8 x 10-4 M. What is the pH?

A: we know pH = −log [H+] where   [H+]  = concentration of H+

Q: What is the concentration of an aqueous HI solution that has a pH of 2.74?

A: The question is based on the concept of PH calculations.   pH is defined as negative logarithmic of…

Q: Calculate the pH from the H+ concentration. 5.2 x 10-12 M

A:

Q: What is the pH of a solution with [H3O+]=1x10-9M?

A:

Q: * The hydrogen ion concentration of a fruit juice is 3.3 x 10-2M. What is the pH of the juice ? Is…

A: 1). pH is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being neutral.…

Q: Calculate the pH of solutions with the following hydronium ion concentrations: a) 1.00 x 10^-9 M…

A:

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H, O0*], of 5.24 × 10-³ M.

A: pH is defined as the negative logarithm of the activity of hydronium ion. But in dilute solutions,…

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: 5. What would the pH of a solution that had a hydroxide ion concentration of 1 x 10º M be?

A:

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=1.6×10^−4 M?   pH=

A: The pH of an aqueous solution can be calculated using equation (1). In this equation [H+] represents…

Q: What is the pH of 8.1 x 10-5 M HClO4 solution?

A:

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

A:

Q: The pH of a 0.045 M Ca(OH)2 solution is: +1.3467 O +12.954 O +12.653 O -1.3467

A:

Q: A solution contains [OH-] = 4.88 x 10-6 M. What is the pH of the solution?

A: Given   The concentration of OH- is 4.88×10-6 M.

Q: If a solution has [OH-] = 3.64 x 10^-7, what is the hydronium ion concentration?

A:

Q: Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.     Ka = 7.11*10^-3

A: Given: Concentration of H3PO4 = 0.400 M And Ka of H3PO4 = 7.11 × 10-3  NOTE: Since only the 1st Ka…

Q: What is the pH

A:

Q: What is the pH of a HCI solution with a concentration of 6 x 104 M?

A: pH= -log [H^+]

Q: caculate the pH of a solution in which [OH─] = 3.1 x 10-3 M

A:

Q: What is the pH of a solution with an [H*] = 1 x106 %3D

A: Given that, [H+]=1×10-6M pH=?

Q: What is the pH of the solution if the hydroxide ion concentration is 1.0 x 10-6? 4 8. 10

A:

Q: What is the hydroxide ion concentration [OH-] in a solution that has pH = 3? Assume the solution at…

A:

Q: What is the pH of a solution with [OH] = 6.9 x 10-2 M? %3D

A: pH is negative logarithm of hydrogen ion concentration. pOH is negative logarithm of hydroxide ion…

Q: calculate the pH and pOH of a 4.3 x10-3M solution of NaOH

A: Concentration of NaOH = 4.3 x 10-3M NaOH is a strong base and it can dissociate into its ions…

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H] = 8.5 x 10-7 M? pH =

A:

Q: If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric…

A: Given data, Calculating the concentration of hydrofluoric acid.

Q: What is the pH of an aqueous solution of 2.37×10-2 M nitric acid? pH =

A: The important thing to keep in mind here is that nitric acid is a strong acid, which means that it…

Q: What is the pH of a substance that has an H30+ concentration of 7.6 x 10^-12 M

A: pH = 11.11

Q: What is the pH of a solution with a hydrogen concentration of 2.3x10-SM? pH pH 2 2 2 3 3 3 5 5 6 6 6…

A:

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: What is the pH of a solution if the [H+] = 7.2 x 10^-9?

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: 11. If the [H+] is 1 x 10 ^-3 . What is the pH of the solution?

A: Interpretation -  To determine the pH of the solution when concentration of [ H+ ] is given as 1 ×…

Q: What is the pH of a 7.8×10-5 M Ca(OH)2 solution?

A:

Q: what is the pH of a solution that has the following H+ concentraion? 1.75 x 10^-5 mol/L

A:

Q: What is the pH of a solution if [OH-]=2.4 x 10-6?

A: pH of any solution in terms of [OH-] is given by  pH = 14 + log[OH-] where [OH-] = concentration of…

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

A:

Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: What is the pH of a 5.3 x 10^-6 M HBr solution?

A:

Q: What is the pH of a solution with a [H] of 3.5 x 10³? (K)

A:

Q: A solution has [OH-] = 8.9 x 10^-3, how would you calculate the ph of the solution ?

A: This problem can be solved by knowing that for any solution, pH + pOH = 14. The pH of a solution is…

Q: Calculate the pH of a solution  with [H+]  = 1.8 x 10-5 M

A: [H+] = 1.8 × 10-5 M

Q: What is the pH of a solution with [H3O+] = 4.5 x 10-5M?

A:

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of (H*] = 4.1 x 10-5 M? pH =

A: Given information,      [H+] = 4.1 × 10-5 M

Q: What is the concentration of H3O+ in an aqueous solution with pH of 8.2?

A:

Q: Calculate the pH and pOH of a 4.3 x 10-3M solution of NaOH.

A: Given information: Concentration of NaOH = 4.3 x 10-3M

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.