NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.036 M in NH4Cl?

Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…

A: H2CO3 ⇌HCO3−  +   H+.........     ka1= 4.3x10-7 HCO3− ⇌CO3-2 ​+   H+..........    Ka2=5.6x10-11ka1…

Q: What is the pH of a 0.360 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹

A: Given data--> C= 0.360 M solution of C5H5NHBr Kb=1.7*10-9   pkb = - log10(1.7*10-9) pkb= 9 -…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.26 M solution…

A:

Q: Calculate the pH of a 0.170 M solution of potassium nitrite, KNO₂. pH =

A: Given that, [KNO2] = 0.170 M =C (LET)  pH = ?

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Given,  Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. The pH…

Q: The acid dissociation constant K of alloxanic acid (HCH₂N₂O5) is 2.24 × 10¯7. a Calculate the pH of…

A: Information of question

Q: For the diprotic weak acid H2A, ?a1=3.7×10−6 and ?a2=6.2×10−9. What is the pH of a 0.0450 M…

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.60 M solution…

A: Answer:Value of pH is equal to:

Q: Determine the pH of a 0.20 M solution of weak base pyridine C5​H5​N.Kb​=1.7×10−9.

A: PH is defined as power of hydrogen,it is calculated as negative logarithmic value of hydrogen ion…

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: At 25°C, calculate the pH of a 0.426 M solution of the salt KNO2. (Ka (HNO2) = 4.50 × 10−4 ).

A:

Q: Household bleach is prepared by dissolving chlorine in water.  Cl2 (g) + H2O  « H+ (aq)  +  Cl-…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A solution is made by dissolving 26.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Given that, Weight of Ba(NO₂)₂  = 26.5 g Weight of Ba(NO₂)₂  = 26.5 g/261.337 g/mol = 0.1014 mol…

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: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

A:

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)

A: Given, Concentration of C₅H₅NHBr = 0.420 M Kb = C₅H₅N is 1.7 × 10⁻⁹

Q: 6a) Write the hydrolysis reaction of hypochlorous acid Clearly identify the acid, base, conjugate…

A: Given data:Concentration of solution of acid =0.050 MDetermine the hydrolysis reaction of…

Q: 0 A chemist dissolves 578. mg of pure perchloric acid in enough water to make up 120. mL of…

A: Given:Mass of perchloric acid (HClO4)= 578. mg                 (3 significant figures)Volume of the…

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

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 x 10 and Ka2 = 6.7 x 10°. What is the pH of a 0.30 M solution of…

A: Given,the molarity of H2A = 0.30 MKa1 = 3.4 x 10-4Ka2 = 6.7 x 10-9

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: To calctulate the pH, we would use Ka or Kb expression.  “Since you have posted multiple questions,…

Q: The acid dissociation constant Kof alloxanic acid (HCH³N₂O²) is 2.24 × 10 Calculate the pH of a 4.0M…

A: The concentration of  = 4.0 MThe dissociation constant for acid =  pH of the solution = ?

Q: pH and pOH of [H+] = 7.23×10-4 M

A: Given : [H+ ] = 7.23 X 10-4 M

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.45 M solution…

A: The question is based on the concept of equilibrium. we have determine the pH of the given diprotic…

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

A:

Q: Which of the following can be classified as a Lewis base? BH3 O I only II, III, and IV O I and II O…

A: Lewis bases are those compounds which has lone pair of electrons to donate.  Lewis acids are those…

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: of a 0.432 M aqueous solution of n pH =

A: pH of solution is defined as negative logarithm of hydrogen ions present in the solution. Here we…

Q: For the diprotic weak acid H2A, ?a1=2.9×10−6 and ?a2=8.2×10−9. What is the pH of a 0.0650 M solution…

A: Diprotic acid is dibasic acid which has two acidic H+. This will dissociate two times.

Q: Household bleach is prepared by dissolving chlorine in water.  Cl2 (g) + H2O  « H+ (aq)  +  Cl-…

A: The hydrogen ion concentration in the solution of a pH of 1.19 is;

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA]…

A: we have to calculate the percent ionization

Q: Calculate the pH of a 0.0307 M aqueous solution of nitrous acid (HNO₂, K₂ = 4.5×10-4). pH =

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: Calculate the pH of the weak acid, lactic acid (HC3H5O3), if the concentration is 0.10 mol/L and the…

A: Given data,Molarity of lactic acid=0.10mol/LKa of lactic acid=1.4×10-4

Q: What is the concentration of hydronium ions in a solution at 25°C with pH = 4.282?

A: pH = - log [H3O+] 4.282 = -log[H3O+] log[H3O+] = -4.282 = -5 + 0.718   log [H3O+]  = log 10-5 + log…

Q: The acid dissociation constant K, of alloxanic acid (HC H₂N₂O) is 2.24 x 10 Calculate the pH of a…

A: Ka of alloxanic acid HC4H3N2O5 = 2.23×10-7Concentration of alloxanic acid = 3.9 MpH of the solution…

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: Calculate the pH of a 0.506 M solution of NaF. The K, for the weak acid HF is 6.8 × 10-4. pH =

A: The PH of NaF can be calculated as follows

Q: What is the pH of a 0.680 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given: concentration = 0.680 M              Kb=1.7×10-9

Q: What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: pH= 1/2(pKb-logc) Here given Kb=1.7×10-9,hence pKb=-logKb=-log(1.7×10-9) given c=0.430 M

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Interpretation: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3×10-7 and Ka2 = 5.6 × 10-11.…

Q: What is the pH of a 0.600 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.46 M solution…

A: For first ionization, [H+] = (Ka1 * C)^1/2 where C = initial concentration of acid = 0.46 M [H+] =…

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.