The concentration of hydroxide ion in an aqueous solution at 25°C is 5.4 x 10-4 M. What is the rotion of the bydrenium

Q: What is the pH of rainwater saturated with carbon dioxide at 25 deg C is the CO2 concentration is…

A: 1- First determine the concentration of CO2 in M unit :  Concentration of CO2 = ( 300 mg / L)…

Q: The pH of a solution that contains 0.010 M H3O+ is

A: The concentration of [H3O+] = [H+] = 0.01 M.

Q: A solution of 1.789 M HCl (20.00 mL) is titrated with standardized 1.102 M KOH. After 32.0 mL KOH is…

A: Introduction: Molarity is used to express the concentration of the solution. It is defined as the…

Q: An aqueous solution containing only hydroiodic acid has a [HI] of 0.008002 M. What is the pH of the…

A:

Q: What is the hydronium ion concentration in an aqueous hydroiodic acid solution with a pH of 2.750?…

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

Q: If you dilute 1.00 mL of a 1.00 M HCl solution to a final volume of 100.0 mL, what is [OH-] in this…

A: Initial volume=1.00mL Initial consultation=1.00M Final volume=100.0mL Final concentration=?

Q: 17) What is the pH of a 0.020 M Ca(OH)2 solution?

A: Ans is 12.6

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: Barium format is formed from the strong base barium hydroxide and weak acid formic acid. The…

Q: When ____ is dissolved in water, the solution will be acidic. (A) Ca(OH)2 (B) NH4Cl (C) NaCl (D)…

A: Acidic, basic and neutral salt a) Strong acid + strong base ➝ neutral salt + H2O  So, when salt of…

Q: The hydronium ion concentration of an aqueous solution of 0.428 M aniline (a weak base with the…

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: A 7.87⋅10−27.87⋅10-2 M solution of HBr is made.  What is the [OH-] in the solution?  Record this…

A: Concentration of HBr = 7.87 x 10-2

Q: Which of the following are strong bases in solution? Provide explanation on answer chosen: Mg(OH)2…

A: To identify the strong base in solution

Q: Certain metal cations can act as Lewis acids in water to produce an acidic solution even though the…

A: Here Co2+ will react with water to release H+ ions. Thus it remains as, Co2+ + 2 H2O --->…

Q: The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (a)…

A: In quantitative analysis,acid-base titrations are carried out to find the concentration of unknown…

Q: Calculate the [H3O+]

A:

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

A:

Q: How can we answer this question: 1) Equal volumes of 1 M solutions of citric acid, sodium citrate,…

A: A weak acid shows that doesn't ionize promptly in an aqueous solution. The weak acids contain low…

Q: Assuming complete dissociation, what is the pH of a 3.39 mg/L 2Ba(OH)2 solution?

A: Given, Mass of Ba(OH)2= 3.39 mg/L= 3.39 × 10-3 g/L We know , pH = -log[H+] Kw = [OH-] × [H+]

Q: None

A: The three ions that can affect the pH of a solution are: Fluoride ions (F-): Fluoride ions can…

Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

Q: what is the pH?

A: Given :-  Concentration of weak base = 0.120 M  Concentration of conjugate acid = 0.590 M  Kb = 5.9…

Q: What is the pH and pOH of a solution made by adding 10.0mL of 0.034 M HNO3 to 10.0 mL of 0.028 M…

A: Given,molarity of HNO3 = 0.034 MVolume of HNO3 = 10.0 mLMolarity of KOH = 0.028 MVolume of KOH =…

Q: A solution contains 0.0796 M potassium acetate and 0.180 M acetic acid (Ka The pH of this solution…

A:

Q: Calculate the pOH of an aqueous solution at 25°C that is (a) 0.011 M in HNO3 , (b) 3.5 × 10-3 M in…

A: pOH of solution can be can be calculated as, pH=-log[H+]pH+pOH=14pOH=14-pH

Q: The concentration of [H3O+] in an aqueous sample is found to be 1x 10-6 M, what is the pOH of this…

A: We know that:

Q: An aqueous solution containing only hydroiodic acid has a [HI] of 0.006767 M. What is the pH of the…

A:

Q: 16.5 mL of 0.1000M HCI are required to titrate a 10.00 mL aliquot of a saturated strontium hydroxide…

A: The productof the ionic concetrations of a electrolyte that at one temperature can continue in…

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.