What is the pH of a 0.050 M triethylamine, (C2HS)3N, solution? Kb for triethylamine is 5.3 x 10-4

Q: What is the pH of a 0.250 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Given data,Molarity of aniline=0.250MKb=4.3×10-10

Q: In the laboratory, a general chemistry student measured the pH of a 0.345 M aqueous solution of…

A: The ionization reaction for caffeine is as follows, C8H10N4O2+H2O→HC8H10N4O2++OH- For above…

Q: What is the concentration of hydroxide ion in a 0.060 mol dm-3  aqueous solution of methylamine,…

A:

Q: Calculate the pH at 25°C of a 0.45 M aqueous solution of oxalic acid (H2C2O4). (Ka1 and Ka2 for…

A: We have to calculate the pH value.

Q: In the laboratory, a general chemistry student measured the pH of a 0.317 M aqueous solution of…

A: In an aqueous solution of benzoic acid, C6H5COOH (aq)⇔C6H5COO- (aq) + H+ (aq)

Q: What is the pH of a 0.0270 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: HCN is a weak acid , it ionizes  as follows  HCN <----> H+ + CN- Given , Concentration of HCN…

Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given :- concentration of methylamine solution  = 0.0730 M  Kb for methylamine = 4.4 × 10-4  To…

Q: What is the pH of a 0.220 M solution of sodium cyanide (NaCN)? Ka for HCN is 4.9 x 10-9.

A: NaCN has one less hydrogen and corresponds to a conjugate base (a weak base). The credentials…

Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,l? (Kb of CH;NH, is 4.4 x…

A: This is a basic buffer solution. A buffer resist the change in PH of the solution.

Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution?             Kb for triethylamine is…

A: Given, 0.350 M triethylamine  Kb for triethylamine is 5.3 *10-4

Q: Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and…

A: We will calculate pH

Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: 10. Calculate the pH of a 0.150M solution of sodium acetate (NaC,H,O;) at 25°C. (K, for acetic acid…

A: Given-> Concentration of sodium acetate = 0.150 M Ka (CH3COOH) = 1.8 × 10-5

Q: Calculate the pH of the following solutions: a. 2.0 M morphine hydrochloride, C,„H,„NO,•HCI (pK, =…

A: In order to solve this question, we will be using simple concepts of chemical and ionic equilibrium.…

Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…

A: pH = 12.155 Therefore, pOH = 14 – 12.155 pOH  = 1.845 So,as we know that ;  [OH¯] = 10¯pOH =…

Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?

A: Given concentration of CH3COOH = 1.75 × 10-5

Q: What is the pH of a 0.0280 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A:

Q: 6.5 g of sodium acetate was dissolved in 100 mL of water to give a final volume of 106 mL. If the Ka…

A: Sodium acetate dissociates in water into sodium and acetate ions. Sodium ions react very little with…

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

A: The question is based on the concept of PH calculations. we have been given a weak acid and its…

Q: Dimethylamine, (CH3)2NH, a key intermediate in detergent manufacture, has a Kb of 5.9 x 10-4. What…

A: Ionic equilibrium is the equilibrium which is established between the unionized molecules and the…

Q: what is the ph of a 0.85 M solution of pyridine (C5H5N, Kb = 1.70 x 10 ^-9)

A: Pyridine is a weak base. pOH of a weak base. pOH = -log [OH-] pH = 14 - pOH For a weak base like…

Q: Calculate the pH of the solution that contains 0.145 M NH3 and 0.192 M NH4Cl.  The Ka of NH4+ is…

A: The solution will be the buffer solution if the weak acid and its corresponding conjugate base are…

Q: A solution is made by dissolving 26.5 g of LIC3H5O2 in 500.0 mL of water. Using Kb(C3H5O2) = 7.7 x…

A: Given: The mass of LiC3H5O2 = 26.5 g The volume of the solution = 500.0 mL The Kb of C3H5O2- = 7.7 ×…

Q: A weak base is dissolved in water with a concentration of 0.200 mol/L. The Kb value of the base is…

A: Given :- initial concentration of base = 0.200 mol/L                Kb of base = 9.75 × 10-4  To…

Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,1? (Kb of CH,NH, is 4.4 x…

A:

Q: What is the pH of a 0.0650 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A:

Q: What the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 10*)?

A: A numerical problem based on pH of the weak base, which is to be accomplished.

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

A:

Q: The acid constants of the polyprotic acid НЗASO4 are К_a1 %3D 5х10 ^-3, К_а2 - 8х10^-8, К_а3 %3D…

A:

Q: 1 out of Calculate the pH of a 0.40M solution of sodium acetate (NaCH,COO) given that the K, of…

A: NaCH3COO solution means salt hydrolysis. NaCH3COO is made up of weak acid acetic acid and strong…

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: What is the pH of a 0.560 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.560 M And Ka of HNO2 = 4.5 X 10-4  Since Ca(NO2)2 is a…

Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?

A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…

Q: What is the pH of a 0.0370 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A:

Q: Calculate the pH of a buffered solution that is 0.100 M in C6H5COOH (Ka = 6.4 x 10–5) and 0.100 M in…

A: Given: C6H5COOH=0.100 M Ka=6.4×10-5 C6H5COONa=0.100 M To find: pH of buffered solution Solution: pH…

Q: 6. What is the pH of a 0.25 M solution of methylamine hydrochloride (CH3NH3CI)? Kb for methyl amine…

A: This ia a salt of weak base and strong acid. So apply formula for salt of weak base and strong acid.

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4.  What is the pH of a 0.290 M  solution of methylamine?

A:

Q: The Kp of dimethylamine [(CH3)2NH] is 5.90×104 at 25°C. Calculate the pH of a 1.55x103 M solution of…

A: Given :  Concentration of (CH3)2NH = 1.55 × 10-3 M  Kb = 5.90 × 10-4  To calculate :-  pH of…

Q: What is the pH of a 0.300 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: CH3NH2 is a weak base that partially dissociates in water. C6H5NH2(aq) ↔ OH-(aq) + C6H5NH3+(aq)…

Q: What is the pH of 0.31 M diethylammonium chloride, (C2H5)2NH2Cl.  The Kb of diethylamine, (C2H5)2NH,…

A: The pH of the 0.31M diethylammonium chloride is given below

Q: What is the pH of 0.273 M trimethylammonium iodide, (CH3)3NHI? The Kb of trimethylamine, (CH3)3N, is…

A: Kb = 6.3 x 10-5

Q: In the laboratory, a general chemistry student measured the pH of a 0.441 M aqueous solution of…

A:

Q: 6. What is the pH of a 0.250M solution of methyl amine (CH3NH2, Kb = 4.4 x 104)?

A:

Q: What is the pH of 0.278 M diethylammonium iodide, (C2H5)2NH2I.  The Kb of diethylamine, (C2H5)2NH,…

A:

Q: What is the pH of a 0.0500 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: Given -> Molarity of HCN = 0.0500 M Ka = 4.9 × 10-10

Q: What is the pH of a 0.0680 M solution of hydrocyanic acid, HCN (Ка %3D 4.9 х 10-10)?

A:

Q: In the laboratory, a general chemistry student measured the pH of a 0.470 M aqueous solution of…

A:

Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…

A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…

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.