A basic solution has a pH of 11.8. What is the concentration of hydroxide ion, [OH-]?

Q: The molar concentration of OH- in a water solution is 1.0 x 10-9. The pH of the solution is

A: OH — = 1.0 x 10—9

Q: What is the pH of a solution with a hydroxide ion concentration of 10-2 M?

A: [OH-] = 10-2 M  pOH = - log [OH-] pOH = - log (10-2) = 2 At room temperature; pH + pOH = 14 pH + 2 =…

Q: What is the pH of a 0.025 M solution of NaOH

A: Applying formula POH = - log[OH-]

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.26 M solution…

A:

Q: A sample of grape juice has a pH of 3.92. What is the hydroxide-ion concentration of this solution?…

A:

Q: Calculate the pH of a solution that has [ OH-] = 5.2 x 10-7 M pH=  _?_

A: Given, Concentration of OH-, [OH-] = 5.2*10-7M. The pOH of the solution can be calculated as…

Q: a solution has a concentration of OH- =4.0x10-5 M. what are the concentration of H3O+ and the pH of…

A: pH of a solution can be defined as negative of logarithm of concentration of hydronium ions

Q: water has a hydroxide ion concentration of 2.0 x 10-6 M. What is the pH of seawater?

A:

Q: Solution Y has a pH of 7.5 Solution X has a pH of 9.5   a.) what is the [H3O+] in each solution?…

A: We are given pH and we have to tell H+ and OH- ion concentration

Q: A sample of grape juice has a pH of 3.80. What is the hydroxide-ion concentration of this solution?…

A: The pH of the solution can be mathematically expressed as: According to the given information, the…

Q: If the Hydrogen ion concentration of a solution is 1.00 x 10^-4 M, what is the hydroxide ion…

A: Hydrogen ion concentration = 1.00 × 10-4 M. Hydroxide ion concentration = ?

Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

A:

Q: The hydrogen concentration of a solution is 1 x 10-6 M. What is the pH? pH =  Is this an acid,…

A: [H+] = 1 x 10-6 M  PH = ?

Q: What is the pH of a 2.2 x 10- M solution of RbOH? What is the hydronium ion concentration of the…

A: pH is related to pOH as: pH+pOH=14

Q: What is the pH of a solution that is 3.0 M H2SO4

A: Please find the solution below:

Q: What is the pH of a 2.8 x 10-4 M solution of NaOH? What is the hydronium ion concentration of the…

A:

Q: The pH of a solution is 3.83. What is the OH⁻ concentration in the solution?

A:

Q: What is the pH of a solution that has an [H+]=0.0470 M ? 3.06 12.7 1.33 8.42

A: We have to calculate the pH of Solution.

Q: )What is the hydronium ion concentration in an aqueous hydrobromic acid solution with a pH of 2.530?

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the pH of a 0.0000100 M solution of CsOH?

A: Given :-  Concentration of CsOH = 0.0000100 M   To calculate :-  pH of solution

Q: A sodium hydroxide solution has a pH of 12.40, what is the OH– concentration in this solution?

A:

Q: The [h3O+] of tomato juice is 2.2 x 10^-4 M. What is the pH of the solution

A: Given [H3O+] = 2.2 x 10-4 M

Q: The pH of a basic solution is 11.99. What is [H⁺]

A: pH of the solution  is defined as "the negative logarithm to the base 10 of the value of the…

Q: The hydronium-ion concentration of a solution is 7.0 × 10-6 M. What is the solution pH?

A: pH of the solution is =   -log [H+]

Q: what is the ph of a solution whose hydrogen ion concentration is 0.015?

A: As we know, HCl is a stong acid. It dissociates completely into H+ and Cl—in a chemical equation –

Q: A nitric acid solution has a pH of 1.75 what is the [H+] and [OH-].

A: Given, pH of nitric acid solution =1.75we are asked to calculate the [H+] and [OH-]

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution…

A: Reactions- H₂A + H2O ↔HA-  + H3O+  Ka1 = 3.4 × 10⁻⁴ HA- + H2O ↔ A2- + H3O+  Ka2 = 6.7 × 10⁻⁹ Ka1…

Q: 1. A solution is 0.055 M HBr. What is the pH of this solution? 2. A solution is 0.00025 M HCI. What…

A: Write the expression for pH. pH=-log[H+] Write the relation between pH and pOH. pH + pOH=14 Write…

Q: A solution has a pH of 3.10. What is the OH− concentration of the solution at 25°C

A: The sum of pH and pOH of the solution is equal to 14. Calculate the pOH of the solution.…

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: at 0.125 M aqueous solution of a weak base is 9.2% ionized. what is the pH of the solution?

A: Given  Concentration (c) = 0.125 M Percentage ionization = 9.2 % pH = ?

Q: If the pH of a solution is 8.1, what is [H3O*] in the solution? What is [OH ] in the solution?

A:

Q: what is the ph of a solution that has [OH-]= 6.9x10^-12

A: Given :- concentration of OH- ions = 6.9 × 10-12 M  To calculate :- pH of the solution

Q: The pH of water should be around 7. What does this mean about the concentration of H+ and  OH- ions…

A: Given : pH of water is 7  To find : Relate it to Concentration of H+ and OH- Solution : pH stands…

Q: hat is the concentration of hydronium ions in a solution with a pH of 5?

A: Given- pH of the solution =5  We know formula,  pH = - log [H+]

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: The hydronium ion concentration in a given solution is 1.8 x 104. What is the concentration of the…

A: Hydronium ion concentration H+ and hydroxide ion concentration OH- are related to each other as:…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.46 M solution…

A: For first ionization, [H+] = (Ka1 * C)^1/2 where C = initial concentration of acid = 0.46 M [H+] =…

Q: Ammonia, NH3NH3, is a weak base with a KbKb value of 1.8×10−51.8×10−5. A) What is the pH of a 0.370…

A: Given  concentration of NH3 = 0.370 M Kb = 1.8 x 10-5    To find : a) pH of ammonia solution…

Q: What is the pH of a 3.47 x 10 ^-4 M solution of hydrochloric acid?

A: Given data is as follows: The concentration of hydrochloric acid  = 3.47×10-4 M The pH of the…

Q: What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous…

A: From given pH value pOH is determined. Then, [OH-] concentration is calculated.

Q: The pH of an acidic solution is 7.35. What is pOH?

A: The relation between pH and pOH can be expressed as,                   pH + pOH = 14…

Q: Sodium hydroxide is used to clear clogged drains. A solution of NaOH has a pH of 9.52 at 25C. What…

A: PH  is a negative logarithm of concentration of H+  ions.  PH = -log [H+]  POH = -log[OH-]  PH + POH…

Q: The pH of an aqueous solution of 0.483 M nitrous acid is

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: What is the pH of a 4.9 x 10-4 M solution of HBr?

A:

Q: Calculate the pH of a solution that has [H3O+] = 3.9 × 10−8 M.

A: We are given  [H3O+]  = [H+] = 3.9 × 10−8 M we are to calculate the pH.

Q: pH of a solution is 3.53. What is the OH⁻ concentration

A: [H+] = 10-pH [H+] x [OH-] = 1 x 10-14

Q: The pH of an acidic solution is 5.47. What is [OH⁻]

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the [H3O+] of a solution that has a pH of 4.6? What is the pH of a solution whose [OH-] =…

A: PH = -log H3O+PH = 4.6Calculate H3O+ concentration4.6 = -logH3O+logH3O+ =-4.6H3O+ =Antilog…

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.