What is the concentration of hydroxide ion in a 0.77 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 10-14.) what is M

Q: Calculate the concentrations of all species in a 1.63 M NaCH,COO (sodium acetate) solution. The…

A: From given  Initial concentration CH3COO-  = 1.63M  Ka CH3COOH = 1.8 × 10-5  Na+ is spectator ion…

Q: What is the concentration(M) of nitric acid if it takes 42.7mL of 0.250M barium hydroxide to…

A:

Q: For a solution of 0.020 M lactic acid, HC3H5O2 (Ka = 8.4 × 10-4), calculate: [H+]= _______ M pH=…

A: For a weak acid ,HClO                     HC3 H5O2       ⇌      C3 H5O2 -       +      H+…

Q: The value of K, at normal body temperature (37°C) is 2.8 × 10-14. Calculate the concentration of…

A: Given values : Kw = 2.8 x 10-14 [ H3O+ ] = 0.01 M

Q: What is the concentration of hydroxide ion in a 0.54 M aqueous solution of hydroxylamine, NH2OH?…

A: Hydroxyl amine is a weak base and it partially dissociates into NH2+ ion and OH- ions. The ICE table…

Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.630 M? (Kb = 1.3…

A:

Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.560 M? (Kb = 1.3…

A: Given information,  H2NNH2 in a solution with a concentration of a 0.560 M  Kb = 1.3 x 10-6

Q: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous…

A: Given that,  Ionisation constant of lactic acid Ka = 1.36×10-4 Amount of lactic acid dissolved in…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.7 × 10⁻³. What is [H⁺]?

A:

Q: What is the concentration of OH− at 25o C in 0.25 M nitric acid solution?

A:

Q: [OH⁻

A:

Q: Propanoic acid HC3H5O2, has a Ka of 1.3 x 10-5. What is the [H3O+] in a (1.51 x 10-1) M solution of…

A: The ionization of Propanoic acid HC3H5O2 takes place as,                             HC3H5O2 (aq)  +…

Q: The concentration of SO42- ion in a 0.25M Al2(SO4)3 solution is:

A: Given information: Concentration of aluminum sulfate = 0.25 M

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

A:

Q: How many grams of KHP is required to completely neutralize 25.00mL of a 0.100-M sodium hydroxide…

A: Molarity = moles of solute/volume of solution (in L)  so, moles = molarity × volume (in L)     When…

Q: If it takes 10.0 mL of 2.0 M H2SO4 to neutralize 30.0 mL of KOH, what is the molar concentration of…

A: When an acid reacts with a base it produces salt and water. Such reactions are known as acid-base…

Q: A solution is 0.20 M Ba(OH)2. How many moles of H+ must be added to neutralize 100.0 ml of the…

A:

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

A:

Q: iv) What name is given to the solution formed when all the NaOH has reacted? Calculate the p" of the…

A: The question is based on the concept of titrations. we are adding acetic Acid to the sodium…

Q: What is the percent ionization of a 0.100 M solution of benzoic acid? C6H5COOH K₂ = 6.46 x 10-5 a…

A: Given, Concentration of benzoic acid solution (C) = 0.100 M Ka for benzoic acid (C6H5COOH) = 6.46 ×…

Q: What is the pOH of an aqueous solution of 4.90×10-2 M potassium hydroxide? pOH = ______

A: KOH is Strong base so it's pOh can be easily Calculated by Poh= -log[OH-] POH is the power of OH-…

Q: Calculate the concentrations of all species in a 0.990 M NaCH,COO (sodium acetate) solution. The…

A: NaCH3COO is salt and hence dissociates completely. The concentration of CH3COONa is 0.990 M. So the…

Q: 4. What are the pOH and the pH of a 0.0125M solution of potassium hydroxide, KOH? 5. The hydronium…

A:

Q: percent ionization

A:

Q: 1. Calculate the hydronium ion concentration of a solution with a pH of-1.07. 2. What are the pOH…

A: pH = -log[H3O+]  pOH = -log[OH-]  pH + pOH = 14.0   Note :- In question no. 3 concentration of…

Q: What is the pH of an aqueous solution of 9.10×10-3 M nitric acid? pH =

A: Given concentration of nitric acid is 9.10×10-3 M. Relation between pH and concentration of…

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: The hydronium ion concentration of an aqueous solution of 0.465 M acetic acid (K, = 1.80×10-5) is…

A:

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

A:

Q: if the concentration of hydrogen ionsis 6.33 x10''-3 what is the concentration of hydroxide ions?

A: concentration of hydrogen ion = H+ = 6.33 x 10-3 concentration of hydroxide ion = OH- = ?

Q: What is the percent ionization of a 0.0075 M solution of ammonia? K₂(NH3) = 1.8 x 10-5 [?] % %…

A: In a solution of ammonia, ammonia is present as NH4OH due to presence of water. NH4OH acts like a…

Q: What is the percent ionization of H¿NNH2 in a solution with a concentration of a 0.530 M? (Kb = 1.3…

A: Weak base dissociate partially in solution. The degree of ionization is not complete in such…

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

A: The formula for ionic product of water  is given.

Q: In a 2.31 M HCOOH aqueous solution, determine the percentage of ionised HCOOH molecules. Ka 1.8 x…

A: Given,  Molar concentration of HCOOH = [HCOOH] = 2.31 M  Acid dissociation constant of HCOOH = Ka =…

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…

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁴. What is [OH⁻]?   What is the…

A: 1) [H+] =5.5×10-4 M [OH-] = ?

Q: A 0.80 M solution of Carbonic acid is prepared and is in equilibrium with its ions. The chemical…

A: Given data Initial concentration : 0.8 M Ionization constant : Ka=4.3×10-7 Equilibrium reaction…

Q: What is the pOH of a solution that contains 5.6 x 10° M HCI at 25°C? Express your answer in two…

A:

Q: At 40 °C the value of Kw is 2.92 x 10-14. Calculate the [H+] and [OH-] in pure water at 40 °C. What…

A: H2O ⇋ H+ + OH- Kw=[H+][OH-] [H+]=[OH-]=x 2.92×10-14=x2 x=1.7×10-7=[H+]=[OH-]

Q: Determin the pOH for a 1650 mL solution of 3.00 g of Mg(OH)2

A: Given that:                        Volume of the solution = 1650 ml = 1.65 L           Mass of…

Q: At 25 °C, what is the hydroxide ion concentration, [OH 1, in an aqueous solution with a hydrogen ion…

A:

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.9 × 10⁻⁴. What is [OH⁻]?

A: Given- The H⁺ concentration in an aqueous solution at 25 °C is 6.7 × 10⁻⁶.

Q: Which of the following 0.5M aqueous salt solutions will have a pH of 7.0 at 25.0oC? LiF LiBr…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: he OH⁻ concentration in an aqueous solution at 25 °C is 5.9 × 10⁻³. What is [H⁺]?

A:

Q: The h+ concentration in an aqueous solution at 25C is 9. X 10-6. What is [oh-]?

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: (a) Calculate the OH concentration in an aqueous solution at 25°C with an H,O" concentration of 7.15…

A: We will calculate value of hydroxide concentration using formula- [H3O+] [OH-] = Kw

Q: The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous…

A: Given: The ionization constant of the lactic acid = 1.36×10-4 Mass of lactic acid= 20.0g Volume of…

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.