Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a solution that is 0.00789 M ethylamine.

Q: The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3 × 10". Calculate the pH of a 1.2…

A: Given data set: Acid dissociation constant (Ka) for hypobromous acid (HBrO) = 2.3*10-9…

Q: The acid dissociation constant Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a 1.2M…

A: Acetic acid is weak acid and it dissociates partially into [CH3COO-] and [H3O+].

Q: Calculate the pH of 0.085 0 M pyridinium bromide, C5H5NH1Br2. Find the concentrations of pyridine…

A: Given information: Concentration of pyridinium bromide = 0.0850 M

Q: Look up the appropriate Ka1 and Ka2 values for oxalic acid andascorbic acid, and repeat these…

A: The first and second dissociation constants of oxalic acid have been mentioned as follows-

Q: If a sample of a certain solution is determined to have a [H30+] concentration of 7.74×10-3…

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: Determine the pH of a 0.16M NH3 where kb = 2.4 x 10-6 %3D Your answer should follow the format: a)…

A: a) The concentration of NH3 = 0.16 M  Kb = 2.4 × 10–6                                            NH3…

Q: Determine the pH level of a solution that has 0.05385 M of Pyridine, given that the Kb of pyridine…

A: Given, Concentration of the Pyridine solution (C) = 0.05385 M  Kb for pyridine = 1.620 x 10-6 Note:…

Q: Determine the Kb of a weak base if a 0.19-M aqueous solution of the base at 25⁰C has a pH of 10.88

A: The question is based on the concept of equilibrium. we have been given a weak base  whose PH and…

Q: Calculate the pH of a 0.36M methylamine (CH3NH2) solution, if Kb = 4.4x10-4

A: Solution- methylamine (CH3NH2)  is weak base which ionisation is as follow; CH3NH2+H2O→CH3NH3++OH-…

Q: Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric…

A: • The values provided in the question are:-      i) pH of a carbonated cola solution = 3.120    • We…

Q: the laboratory, a general chemistry student measured the pH of a 0.428 M aqueous solution of…

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: What is the pH of a solution of 5.94 M of HASO, which has K,= 5.1 x 10- Round and report your answer…

A: Concentration of H3AsO3 is 5.94 M. The value of acid dissociation constant is 5.1×10-10.

Q: The pH for 0.0715 M solution of CCl,CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based…

A: pH of Solution = 1.40 [CCl3COO2H] = 0.0715 M Ka for CCl3COO2H =?

Q: Calculate the ph of a solution that is made by dissolving 6.45g of NH4Cl(53.49g/mol) in enough water…

A: First calculate molarity by mole/volume. Then use weak base concept to get pH

Q: Calculate [OH–] , [H+] , and the pH of 0.20 M solutions of each of the following  amines. a.…

A: Aniline and pyridine both are weak bases. From the equilibrium table we have to determine its…

Q: The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.29. What is the Kb of this base

A: Given , Concentration of pyridine (C) = 0.10 M pH of pyridine solution = 9.29 Dissociation constant…

Q: The pH of an aqueous solution of 0.530 M methylamine (a weak base with the formula CH3NH2) is…

A:

Q: The acid dissociation constant K, of boric acid (H,BO3) is 5.8 × 10 Calculate the pH of a 2.5M…

A: Give, the dissociation constant (Ka) of boric acid = 5.8×10-10 We have to calculate the pH of a 2.5…

Q: Find the pH of a solution that is 0.25 M in formic acid, and 0.33 M in sodium formate. K, for formic…

A: Given  Ka = 1.7 × 10-4 Concentration of HCOOH = 0.25 M  Concentrate of HCOONa  = 0.33M PH = ? PKa =…

Q: Calculate the pH of the following solutions. 0.20 M pyridine-3-carboxylic acid hydrochloride

A: pH of weak acid

Q: In the laboratory, a general chemistry student measured the pH of a 0.552 M aqueous solution of…

A:

Q: Use information on the table below to determine which of the following bases would have the weakest…

A: Lowest Ka value indicates lowering the acid strength.

Q: Construct the expression for Ka for the weak acid, HPO,2". HPO, (aq) + H20(1) = H;O*(aq) + PO, (aq)…

A:

Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

A:

Q: 1.) A 0.46 M solution of an unknown acid has a pH of 1.45. Is this a strong or weak acid? Explain.…

A:

Q: Construct the expression for Ka for the weak acid, CH-COOH. CH.COOH(aq) + H₂O(l) = H₂O (aq) + CH.COO…

A: Ka is the ratio of the equilibrium concentrations of product over equilibrium concentrations of…

Q: 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…

A:

Q: Acidic Basic Neutral HC4H4O6- CO32- Na+ NH4+ НРО2- CI- Zn2+ PO43- NO3- Fe3+ HČO3- Ca2+ H2PO4- K+ In…

A: Solution                               We know that cations - compound having postive charge…

Q: The pH of an aqueous solution of 0.542 M triethylamine (a weak base with the formula (C₂H5)3N) is

A:

Q: What is Kb for the conjugate base of HCN (Ka = 4.9 × 10⁻¹⁰)?

A: We have given that  What is Kb for the conjugate base of HCN (Ka = 4.9 × 10⁻¹⁰)?  Acid : Acid is…

Q: A 0.100 M ethylamine solution (CH3CH2NH2) has a pH of 11.82. Find the value of the Kb of this base.

A: We have to predict the Kb for the base.

Q: The ka of an acid is 7.6 times 10-3 at 25 degrees celsius, what is the kb of the conjugate base?

A: The ionic product of water is equal to the product of dissociation constant of conjugate base and…

Q: The acid dissociation constant Ka of carbonic acid (H2CO3) is 4.5x10^−7. Calculate the pH of a 4.5M…

A: Given :-  Concentration of H2CO3 solution = 4.5 M  Ka for H2CO3 = 4.5 × 10-7  To calculate :-  pH of…

Q: Calculate the ph of a solution that is prepared by dissolving 8.57 NaC2H3O2(82.03g/mol) in enough…

A:

Q: base protonation constant K, of ammonia (NH,) is 1.8 x 10. ulate the pH of a 1.1 M solution of…

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

Q: The Kb for aniline (C6H5NH2) is 4.3 x 10-10. What is the pH of a 0.15 M solution of aniline?

A: From the ICE table, we have

Q: The acid dissociation K, of benzoic acid (C6H5CO,H) is 6.3 × 10 –³. Calculate the pH of a 1.5 ×…

A: Since benzoic acid is monoprotic acid. hence we can write C6H5CO2H as HA  where A = C6H5CO2 group…

Q: Calculating the pH of a weak acid solution The acid dissociation constant K, of hypobromous acid…

A: Given information: Acid dissociation constant for HBrO = 2.3×10-9 Concentration of hypobromous acid…

Q: Construct the expression for Ka for the weak acid, NH,*. NH,*(aq) + H,0(I0) = H,0*(aq) + NH;(aq) 1…

A: The hydrolysis or ionisation reaction of weak acid is given as, => NH4+ (aq) + H2O (l) ------>…

Q: Convert the FF. P-function to molar concentration a. pH=1.020 B. pOH=.0025. C. pBr= 7.77  D. pCa=…

A:

Q: Calculate the pH of an aqueous KOH solution that is made by dissolving 654 mg of solid KOH in enough…

A:

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: Step by step please clearly

A: Given reaction,

Q: What is the pH of a 0.025 M pyridine solution? (Kb value for pyridine = 1.7x 109)

A:

Q: If you have a 0.1650 M solution of a base is 6.1% ionized, then calculate the base ionization…

A: A base is a compound that accepts H+ ion (proton). Bases dissociate in water to release OH- ions…

Q: Calculate the pH of an aqueous solution that is 0.295 mol L-1 in sodium formate (HCOONA) and 0,.205…

A: Given : Concentration of sodium formate = 0.295 M Concentration of formic acid = 0.205M

Q: Sulfuric acid (H2SO4) has two acidic protons with the following ionization constants: Ka1 is…

A: As we know, Strong acid dissociates completely and releases [H+] ion. So, we can calculate directly…

Q: Calculate the pH of the following: 1. 0.10 M 2-aminophenol|

A: Given: Concentration of 2-aminophenol (which is a base like NH3 and hence assuming it B) = 0.10 M

Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

A:

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.