What is the concentration of H in 0.100 M hydrochloric acid, HCl?

Q: What is the original molarity of a solution of ammonia whose pH is 10.48?

A: The original molarity of solution of ammonia whose pH is the 10.48 is calculated as follows

Q: The H* concentration in an aqueous solution at 25 °C is 8.7 x 10°. What is [OH]?

A: Given: Temperature = 25 oC Concentration of H+ = [H+] = 8.7 x 10-6

Q: What is the original molarity

A:

Q: The hydroxide ion concentration of an aqueous solution of 0.591 M formic acid , HCOOH is [OH*]= М.

A: The concentration of aqueous solution of formic acid, HCOOH = 0.591 M

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

A: Given Concentration of hydroxide ion [ OH- ] = 3.5 x 10-4 M we have to calculate concentration of…

Q: If you dissolved the salt calcium cyanide, Ca(CN)2, in water, what type of solution would you expect…

A: Given dissolution of calcium cyanide in water.

Q: HCl is a strong acid. In 1.0 M HCl, what is the molar concentration of [H+]?

A: Since HCl is a strong acid  hence it will dissociate completely into ions in solution  The…

Q: What is the pOH of an aqueous solution that has a hydroxide ion concentration of 7.0 ✕ 10−4 M?

A: POH  = -log (OH-)

Q: A solution of HCl has a ph of 2.3. If so what is [OH-]?

A:

Q: What is the pH of a solution in which 15 mL of 0.39 M NaOH is added to 25 mL of 0.39 M HCl?

A: Since NaOH and HCl are strong base and acid respectively Hence they will react as per the reaction…

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

A:

Q: Which solution has the higher pH, a 0.001 M solution of NaOH or a 0.001 Msolution of Ba(OH)2?

A: The simplification is as follows:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 7.5 × 10⁻⁴ M. What is the…

A:

Q: The hydroxide ion concentration, (OH'), of an aqueous solution of 0.364 M isoquinoline (a weak base…

A: The dissociation of weak base isoquinoline is, C9H7N  + H2O ↔C9H7NH+ + OH- By definition the value…

Q: What is the pH of a solution if 10 mL of 1.0 M HCl is added to 10 mL of 3.0 M NaOH solution?

A:

Q: The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0063 M. What is the…

A:

Q: What is the concentration of hydronium ions (or H+ ions) in a 0.200 M monoprotic weak acid?

A: Given  Concentration of weak acid = 0.200 M Acid -= Monoprotic weak acid Concentration of H+ ion =…

Q: . What is [OH⁻]?

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

Q: What is the pH of a solution with a concentration of 0.00001 moles/ml (M) of H1?

A: Gvien, concentration of 0.00001 moles/ml (M) of H1

Q: What volume of 0.252 M potassium hydroxide solution is required to completely neutralize 0.0106…

A: An acid base reaction is also called as neutralization reaction. The H+ ions of acid react with OH-…

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 5.8 × 10⁻⁴ M. What is the…

A: Given: The concentration of hydroxide ion is 5.8 x 10-4 M The ionization constant (Kw) of water is…

Q: What is the pH of 8 × 10−8 M HCl?

A: As the concentration of the acid is very low, the ionization of water molecules into hydrogen ions…

Q: What is the concentration of barium hydroxide in an aqueous barium hydroxide solution with a pH of…

A: Given information: pH = 10.20

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.9 × 10⁻⁴ M. What is the…

A: Given :  Temperature = 25 °C  [OH-] = 3.9 x 10-4 M

Q: The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0032 M. What is the…

A:

Q: For a solution with a hydroxide (OH-) concentration of 5.0 x 10-5 M, what is the concentration of…

A:

Q: The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0052 M. What is the…

A: pH: It  is defined by saying that power of hydrogen in any solution. as we know that: kW=H-×OH+

Q: What is the [OH-]  in a solution with a pH of 2.50?

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 1.1 x 10-4 M. What is the…

A: In an aqueous solution, the the concentration of hydroxide ion and the concentration of hydronium…

Q: The hydroxide ion concentration of an aqueous solution of 0.444 M acetic acid is [OH'] = |M.

A:

Q: What is the [OH -] in a solution with a pH of 8.97?

A: Since pH = -log[H+] = 14 + log [OH -]

Q: Calculate the pH value of 0.5 M NaOH

A: As NaOH is very strong electrolyte i.e base so it will dissociate completely  :…

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 3.6 × 10⁻⁴ M. What is the…

A: The concentration of the species gives the amount of that species used in the desired reaction.…

Q: The H* concentration in an aqueous solution at 25 °C is 1.5 x 10°. What is [OH]?

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 5.2 × 10⁻⁴ M. What is the…

A:

Q: What are the concentrations of H+ and OH− in a solution of 150 mM HCl?

A: Conc. of given HCl Soln  = 150 mM  (Since 1 M = 1000mM )  = 0.15 M   H+ + Cl- ---> HCl  As we can…

Q: What is the [OH–] in a 0.0002 M solution of NaOH?

A: Given that, [NaOH] = 0.0002 M Thus,

Q: The hydroxide ion concentration of an aqueous solution of 0.532 M acetylsalicylic acid (aspirin),…

A: Given : Concentration of HC9H7O4 = 0.532 M  Since HC9H7O4 is a weak acid. Hence it will dissociate…

Q: The hydroxide ion concentration of an aqueous solution of 0.558 M formic acid , HCOOH is M. [ОН] 3

A: Given: Concentration of formic acid = 0.558 M Ka of formic acid = 1.8×10-4

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 6.3 × 10⁻⁴ M. What is the…

A:

Q: What is the pH of a solution in which 15 mL of 0.15 M NaOH is added to 25 mL of a 0.10 M HCl ?

A: HCl is a strong acid and NaOH is a strong base. The net ionic equation involved in the titration of…

Q: The concentration of hydrogen ions H+ In a 0.100m solution of hydrochloric acid ,HCL is

A: 1. In physical chemistry,  Molality of solution is defined as total number of moles of solute…

Q: Which of the following solutions is the most basic? 6 M NH3 150 M KOH 100 M Ba(OH)2

A: Given,6 M NH3150 M KOH100 M Ba(OH)2

Q: HCl is a strong acid that dissociates in water:HCl S H+ + Cl-. What is the pH of 0.01 M HCl?

A: Strong acids basically get ionized entirely into its ions and furnish identical amount of…

Q: In a solution of Ba(OH)2, if the concentration of the hydroxide ion is 0.45 M, what is the…

A: Barium hydroxide is a strong base which undergoes complete dissociation in aqueous solution giving…

Q: The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0092 M. What is the…

A:

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 7.2 x 10-4 M. What is the…

A: Concentration of hydroxide ion =7.2×10^-4M Concentration of hydronium ion=?

Q: What is the concentration of H⁺ in 2.0 M acetic acid, HC2H3O2?

A: Given, concentration of acetic acid =2.0 Mwe are asked to find the concentration of H+ in 2.0 M…

Q: What is [H3O+] in a 0.55 M solution of a weak acid, HX, that is 3% ionized?

A: HX + H2O <=> H3O+  +  X- Percent ionisation of an acid ( HX)  = ( [ H3O+ ] / [ HX ] ) × 100

Q: What are the concentrations of H+ and OH− in a solution of 0.02 M NaOH

A: NaOH is a strong base and ionizes completely. We will find concentration of OH- and then…

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.