In an aqueous solution at 25°C, if [H,O*] = 2.9 × 10 M, then [OH] is:

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: Assuming complete dissociation, what is the pH of a 4.15 mg/L Ba(OH)₂ solution? pH =

A: Upon dissociation the base will give the hydroxide ions which will make the solution basic and from…

Q: Calculate either [H,O] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.59 x 107…

A:

Q: Before you begin a day trip, you inflate the tires on your automobile to a recommended pressure of…

A:

Q: Calculate the pOH of a solution in which [H=] = (0.5)[OH‐].

A:

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶. What is [OH⁻]?

A: The product of [H+] and [OH-] is 1.0×10-14 at 25°C. [H+] = 5.5×10-6.

Q: At equilibrium, a 0.45 M [NH3] solution produced an [OH-] of 2.90*10^-3 M. What is the Ka of this…

A: Given, equilibrium concentration of NH3 = 0.45 M, and equilibrium concentration of OH– = 2.90 ×…

Q: Macmillan Learning Calculate either [H₂O+] or [OH-] for each of the solutions at 25 °C. Solution A:…

A:

Q: For given aqueous solution if [OH]=1.0x10^-5 M, what is [H+]

A: At a specific temperature, the concentration of ion of hydrogen and concentration of ion of…

Q: Calculate either [H,O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.59 × 10-7…

A:

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.49 × 10−7…

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Q: Calculate [OH¯] for a solution where [H,O*] = 0.00379 M. %3D [OH¯] = M

A: For an aqueous solution, we know that the production of the concentration of the hydrogen ions and…

Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.546 M hydroxylamine (a weak base…

A: Concentration of hydroxylamine = 0.546 MKb of hydroxylamine

Q: The H⁺ concentration in an aqueous solution at 25 °C is 9.3 × 10⁻⁶. What is [OH⁻]?

A: • The values provided in the question are:-      i) Hydrogen ion concentration of a solution, H+ =…

Q: Calculate [OH -] and pH for each of the following solutions. (a) 0.0036 M RbOH [OH-] =  M pH =…

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Q: In an aqueous solution at 25°C, if [H,O+] = 2.6 × 10-4 M, then [OH] is:

A: Find the solution below

Q: Give the major elimination product of the following reaction. Br CH,CO,H heat ?

A: Given is organic reaction.this is elimination reaction.In which reactant is alkyl bromide.

Q: 2) Calculate [OH-] at 25 °C for each solution and determine if the solution is acidic, basic, or…

A: Ph=-log[H+] Ph+poh=14 POh= -log[OH-] A) Acidic solution  B) basic solution

Q: You have an aqueous solution with [OH-] = (9.859x10^-5) M at 25°C. What is [H3O+]?

A: [OH-]=9.859x10-5M[H3O+]=?Now we will calculate the concentration of the hydronium ions.

Q: alculate [OH -] and pH for each of the following solutions. (a) 0.0027 M NaOH [OH-] =  M pH =…

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Q: In an aqueous solution the  [OH-] is 1.0 x 10- 6 M. What is the [H+]

A: At 25oC, the mathematical relation between molarities of H+ and OH- is given as: [H+][OH-]=1.0×10-14…

Q: The OH- concentration in an aqueous solution at 25 celcius  is 7.1 x 10^-5. what is [H+]?

A: Given,  Concentration of OH-ion = [OH-] = 7.1 x 10-5 M  What is [H+] = ?

Q: Why is [ H3O] = [OH]  =1×10^-2M not feasible in water? What would happen if we tried to make such a…

A: The dissociation of ionisation reaction of water is  2 H2O (l) --------> H3O+ (aq) + OH- (aq)…

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: When we write and balance the chemical reaction, then there is a rule is applicable behind this…

Q: The H⁺ concentration in an aqueous solution at 25 °C is 7.5 × 10⁻⁶. What is [OH⁻]?

A: Autoionization of water takes place as follows:In pure water, the concentration of the hydronium ion…

Q: Assuming complete dissociation, what is the pH of a 3.67 mg/L Ba(OH)₂ solution? pH =

A: The mass of barium hydroxide = 3.67 mg =         ( 1.0 mg = 10-3 g)Molar mass of Ba (OH)2, = 171.34…

Q: At 25 °C, what is the hydroxide ion concentration, [OH¯], in an aqueous solution with a hydrogen ion…

A: The ionic product of water is the product of the concentration of H+ and OH-. So that with the help…

Q: Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That…

A: Given that, the table is:Solution[H3O+]pHA4.1B8.33CFill up the missing entities in the given table.

Q: The pH of an acidic solution is 3.59. What is [H⁺]?

A: pH  is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions  are…

Q: Calculate either [H3O+] o or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.63 x…

A: A solution is acidic if it's pH is less than 7 and it is basic when it's pH is more than 7 , at 7 it…

Q: Calculate the pOH of a solution that has [OH-] = 3.6 x 10 -5 M

A: pOH of any solution is given by  pOH = -log[OH- ]  where [OH- ] = concentration of OH- ions in M

Q: What is the solution that the concentration of [OH-]= 2.5 c 10^-9M?

A: Given:: [OH-] = 2.5×10-9 M Nature of solution = ?

Q: icmillan Learning Calculate either [H,O*] or [OH-] for each of the solutions at 25 °C. Solution A:…

A: At 25°C , H3O+×OH- =1×10-14 PH=-logH3O+ When PH of the solution is >7, then it is a basic…

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.15 x 10-7…

A: • [H3O+] × [OH-] = 1 × 10-14 • pH = -log[H3O+]

Q: Assuming complete dissociation, what is the pH of a 4.04 mg/L Ba(OH)2 solution? pH=

A: Given :  We have to calculate pH.

Q: The pOH of a 0.07 M NgOH solution at 25 °C is:

A: Given :- concentration of NaOH = 0.07 M  To calculate :- pOH of the solution

Q: Calculate [H], [CIO], and [OH] in an aqueous solution that is 0.175 M in HCIO, (aq) at 25 °C. [H*] =…

A:

Q: -8 An aqueous solution at 25 °C has a OH concentration of 1.7x 10 °M. Calculate the H,0' concentrati…

A: [OH-] = 1.7 × 10-8 M Temperature = 25 °C [H3O+] =?

Q: The H⁺ concentration in an aqueous solution at 25 °C is 4.5 × 10⁻⁴. What is [OH⁻]?

A: We know that pH is negative log of Concentration of H+  ions. pH = -log [H+] Similarly pOH = -log…

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.