The pH at 25°C of an aqueous solution of hydrofluoric acid, HF, is 2.13. Calculate the concentration of HF in this solution, in moles per liter.

Q: Calculate the pH of an aqueous solution of 0.2070 M potassium carbonate. pH =

A: “Since you have posted multiple questions, we will provide the solution  only to the first question…

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: 0.35 g of hydrogen chloride (HCl) is dissolved in water to make 8.0 L  of solution. What is the pH…

A: Ph = -log (H+)

Q: A solution of acetic acid is prepared in water by adding 11.1 g of sodium acetate to a volumetric…

A: The objective is to determine the concentration of acetic acid and acetate.Given:Mass of sodium…

Q: The ph of an unknown solution is 8.84. Calculate the pOH. Express your answer in standard notation…

A: pH of the solution depends on concentration of H+ ion present. With increase of H+ ion…

Q: 10 mL of 5.0 X 10 M HCl solution is mixed with 150 mL of water to make a new HCl solution. What is…

A: We have to calculate the pH of solution

Q: what is the pH of the diluted solution? The

A: We have to find pH of resulting solution

Q: In a titration experiment, it takes 31.45 mL of 0.018 M NaOH to neutralize a 15.00 mL sample of HCI.…

A: Acid reacts with base to form salt and water. In the given reaction acid is HCl. It reacts with NaOH…

Q: A chemist dissolves 641. mg of pure nitric acid in enough water to make up 60. mL of solution.…

A: Molecular mass of nitric acid = 63 gm / mol => moles of nitric acid = mass in gm / molecular mass…

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: Consider the following data on some weak acids and weak bases: name acid hydrofluoric acid HF…

A: The question is based on the concept of salt hydrolysis. We need to arrange given salts in…

Q: The pH of a basic solution is 10.19. What is [OH⁻]?

A:

Q: A stock solution is made by dissolving X grams of KOH in water and making it up to the mark in a…

A: The solution which resists change in pH of the solution is called a buffer solution. The resistance…

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

A: Weak base are bases which does not dissociate completely to furnish hydroxide ion when dissolved in…

Q: A chemist dissolves 213. mg of pure barium hydroxide in enough water to make up 130. mL of solution.…

A: pH of a solution is defined as the negative log of the hydrogen ion concentration. pOH of a solution…

Q: An aqueous solution has a hydronium ion concentration of 4.0 x 10/ M. What is the pH of this…

A: Answer: pH of a solution is the negative of logarithm of hydronium ion concentration.

Q: solution contains a mixture of hydrogen cyanide (HCN, Ka = 4.9 X 10–10) and sodium cyanide (NaCN).…

A: pH of buffer solution is calculated by using Henderson Hesselbalch equation

Q: The hydrogen ion concentration of a basic solution is 7.70 × 10-9 M. What is the pH of the solution?

A: pH = - log[H+]

Q: Nitric Acid is used in cleaning glassware during very precise analytical chemistry. You obtain a…

A: Given, Concentration of HNO3 = 0.15 M  PH =?

Q: e classification of acid and base

A:

Q: The pH of a basic solution is 10.57. What is [OH⁻]?

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: The hydroxide ion concentration in a solution of NaOH is 9.0 x 10-¹ M ot 25 °C What is the of thic…

A: pH is equal to negative logarithmic value of hydrogen ions concentration

Q: The pH of an aqueous solution of 9.69×10- M ammonium chloride, NHĄC1 (aq), is This solution is

A: NH4Cl is a salt of strong acid (HCl) and weak base (NH3) hence pH this solution  is given by the…

Q: Calculate the pH of pure water

A: Given :- Kw = 2.4 × 10-14  To calculate :- pH of pure water at 37°C

Q: . What is [OH⁻]?

A: The pH of a solution is determined as the negative logarithm of the concentration of hydrogen ions…

Q: The pH of a solution of HBr is 2.88 at 25°C. What is the H⁺ concentration in this solution?

A:

Q: What is the pOH of an aqueous solution of 1.78E-2 M perchloric acid? pOH =

A:

Q: A student is provided with a 1.0 M stock solution of hydrochloric acid (HCl) and asked to mix 5.00…

A: The dilution solution is prepared by reducing the concentration of solute in stock solution by…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: The pH of an aqueous solution of 0.180 M potassium cyanide, KCN, is 8.93 (Assume that K₂ (HCN) =…

A: KCN dissociates in solution as KCN ---> K+ + CN-[ CN- ] = [ KCN ] = 0.180 MCN- hydrolyzed as CN-…

Q: The pH of an aqueous solution at 25°C was found to be 8.50. The pOH of this solution is The…

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

Q: An aqueous solution at 25 °C has a pH of 5.8. Calculate the pOH. Be sure your answer has the correct…

A: given pH = 5.8, we know that pH + pOH = 14

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

Q: concentration of 7.23 x 10^-7 at 100 degrees C. What is the hydrogen ion concentration? Is the…

A: In water,  [H+] = [OH-] [OH-] = 7.23×10-7 M [H+] =  7.23 ×10-7 M Kw =[H+][OH-] =  5.23 × 10-13 pH =…

Q: Observations: Note the pH of each solution you test. Record if the solution is acidic, basic, or…

A:

Q: A chemist dissolves 428. mg of pure sodium hydroxide in enough water to make up 100. mL of solution.…

A:

Q: The pH of 0.01 M hydrochloric acid (HCl) is 2, the pH of 0.01 M sulfuric acid (H2SO4) is 1.7, and…

A:

Q: A chemist dissolves 744. mg of pure hydrochloric acid in enough water to make up 250. mL of…

A: Given data :  Mass of HCl = 744. mg = 0.744 g (1 mg = 0.001 g) Volume of solution = 250 mL = 0.25 L…

Q: an aqueous solution has an OH- concentration of 5.753 x 10^-3 M. calculate the pH of this solution.

A:

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

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.