2 H₂O (l) ⇒ H3O*(aq) + OH(aq) Kw = 2.92 x 10-14 at 40 °C. Calculate the pH of 0.10 M NaOH at this temperature. 13.00 14.54 12.04 12.53 O 14.04

Q: Acetic acid (CH, COOH, K, = 1.80 x 10-) is a weak acid, so the salt sodium acetate (CH, COONA) acts…

A: Given, Ka = 1.8 × 10-5 , [CH3COONa] = 0.566 M The reaction : CH3COONa + H2O ⇔  OH- + CH3COOH

Q: What is the pH of a 0.1777 M NH(aq) solution at room temperature?  The base ionization constant of…

A: Interpretation -  To determine the pH of 0.1777 M NH3(aq) solution at room temperature when base…

Q: the ionization constant for HCN is 4.5 x 10^-10. what is the pH of a 0.43 molar solution of sodium…

A: PH = -log [H+]

Q: The acid dissociation constant Ka of hypobromous acid HBrO is 2.3 x 10^−9. Calculate the pH of a…

A:

Q: b)Determine if the following solutions are acidic, neutral, or basic at 35 °C. Explain your answer.…

A: NOTE : In case of neutral water, H+ ions concentration is given has to be assumed as nothing is…

Q: Calculate the pH of a 0.56 M HF solution at 25 °C. HF (aq) = H* (aq) + F¯ (aq), K₂ = 6.9 × 10-4 at…

A: Given: [HF]=0.56M;Ka​=6.9x10−4;pH=???Step 1: Write the dissociation…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.23 M solution…

A: The PH of diprotic acid can be calculated as follows

Q: Consider the following data on some weak acids and weak bases: acid base Ka name formula name…

A: The salt is an ionic compound formed when an acid reacts with a base. The salt solution can be…

Q: What is the concentration of H+ ions

A: Given :- pH = 4.2  To calculate :- concentration of H+ ions   pH = -log[H+]

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: An aqueous solution has hydronium concentration [H3O+] = 9.8 x 10-5 mol L-1. What is the pH of the…

A:

Q: An aqueous solution at 25 °C has a pOH of 13.7. Calculate the pH. Be sure your answer has the…

A:

Q: aq 6. (i) Define pH in words. The strong acid HCl has a pH value of 1, use the following equation…

A: 6)  HCl(aq) ➝ H+(aq) + Cl-(aq) HCl is strong acid. i) Define pH pH = 1 Hydrogen ion concentration =…

Q: Calculate the pH at 25 °C of a 0.36M solution of sodium hypochlorite (NaClO) . Note that…

A: Given: Concentration of NaClO = 0.36M pKa of HClO = 7.50

Q: |Calculate the pH of a 18 M NH,Cl(aq) (ammonium chloride salt of ammonia) at 25°C. The base…

A: The given chemical reaction is: NH4+aq + H2Ol ⇔ NH3aq + H3O+aq The given information is: Conc. of…

Q: Calculate the pH of the following acid in water knowing that its concentration is 0.73 M and its Ka…

A: Step 1: To answer this question, we must use the ICE table. Initial, [HA] = 0.73 M ICE table:…

Q: The base protonation constant K₁ of lidocaine (C14H21 NONH) is 1.15 × 10 Calculate the pH of a 0.88…

A: Step 1: The base lidocaine (C14H21NONH) is a weak base, which is obvious from its small value of the…

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

A:

Q: What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is…

A: Concentration of KOH solution as 0.0125 M at 100 °C

Q: 7. Identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate…

A:

Q: Determine the pH of a 0.20 M solution of CH3NH3Cl at 25 °C. K₁ for CH3NH₂ = 3.7 x 10-4 K₂ for HCI =…

A:

Q: The ionization constant, Ka, for weak acid, HA, is 3.96 × 10-10, What is the pH of a 0.5213 M…

A: Ka = 3.96 x 10 —10

Q: Calculate the pH of an aqueous solution that is ( Ka(HCN) = 6.20 × 10 10-10) a. 0.870 M in HCN. pH =…

A: We know that  HCN is a weak acid it doesn't dissociate completely. The dissociation reaction will be…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.20 M solution…

A: Reactions- H₂A + H2O ↔HA-  + H3O+  Ka1 = 3.4 × 10⁻⁴ HA- + H2O ↔ A2- + H3O+  Ka2 = 6.7 × 10⁻⁹ Ka1…

Q: The base protonation constant X of ammonia (NH Calculate the pH of a 0.16 M solution of ammonia at…

A:

Q: The base protonation constant K of allantoin (C4H4NO3NH2) is 9.12 × 106. Calculate the pH of a 0.44…

A: Step 1: Step 2: Step 3: Step 4:

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: A solution is made by dissolving 28.1 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Weight of Ba(NO₂)₂  = 28.1gMolar mass of Ba(NO₂)₂ = 261.337g/molVolume of Ba(NO₂)₂  solution = 500…

Q: A solution is made by dissolving 25.1 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A:

Q: Phthalic acid is a diprotic acid with ionization constants K₁1 = 1.12 x 10 and K = 3.90 x 10.…

A: Given,Molarity of potassium hydrogen phthalate ( KHP ) = 0.284 MKa1 of phthalic acid = 1.12 x…

Q: stimate the pH of 0.175 M HCOOH(aq) at 25°C.  Ka(HCOOH) = 1.7 × 10−4. Write your answer with two…

A: The acid dissociation constant of HCOOH is .The concentration of HCOOH is .To find the pH of the…

Q: pH

A:

Q: Calculate the pH of a 1.565Mascorbic acid, H2CgHgO6(aq) solution at 25°C. Round your answer to 2…

A:

Q: The base protonation constant K, of allantoin (C,H,N;03NH,) is 9.12 × 10 °. Calculate the pH of a…

A: Given:

Q: The ionization constant, Ka, for weak acid, HA, is 4.55 x 10-9. What is the pH of a 0.3995 M…

A: The equation for the ionization of weak acid HA as follows.HA (aq) + H2O(l) <=>  H3O+(aq) + A-…

Q: Determine the pH of a 0.10 M solution of sodium acetate (CH3COONa) at 25°C. (Ka of acetic acid = 1.8…

A:

Q: The base protonation constant K of ammonia (NH3) is 1.8 × 10¯5. Calculate the pH of a 0.54 M…

A:

Q: Phosphoric acid, H₂PO4 (aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: Molarity of H3PO4 = 0.500 M PKa1=2.16PKa2=7.21PKa3=12.32 ---------------------------------

Q: Phenol, C6H5OH, is used as a disinfectant. The pH of an aqueous phenol solution was measured at…

A: pH is measure of acidity or basiciity of a solution.We have been given value of pH and we have been…

Q: An aqueous solution at 25 °C has a pOH of 3.78. Calculate the pH. Be sure your answer has the…

A: Given pOH = 3.78

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.