Determine the pH of a 0.10 M solution of sodium acetate (CH3COONa) at 25°C. (Ka of acetic acid = 1.8 ×10−5.) pH =

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 6.3 x 10-4 M? pH =

A: pH is equal to negative logarithmic of hydrogen ion concentration

Q: A chemist dissolves 539. mg of pure potassium hydroxide in enough water to make up 90. mL of…

A:

Q: Naturally occurring rainwater is acidic due to the presence of carbonic acid, H2CO3, produced when…

A: The problem is asking us to calculate the pH of rainwater given the concentration of carbonic acid…

Q: The pH scale ranges from 0-14. Why do we choose to use this scale to represent hydrogen ion…

A: The hydrogen ion concentration would lies from 1 M to very low value upto 10-14 . So, this is very…

Q: What is the pH of a 0.250 M  solution of H2SO4? Ka2 = 1.20×10–2

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: Using standard heats of formation, calculate the standard enthalpy change for the following…

A: We have given that HCl(g) + NH3(g) → NH4Cl(s) ∆Hrxn = ∆Hp - ∆HR…

Q: Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.

A:

Q: Calculate the pH of each solution and indicate whether the solution is acidic or basic.(a) [H3O+] =…

A: pH of the solution is calculated as, pH =-logH+

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: Kw of water at 100°C is 5.62 x 10-13. What is the pH of water at this temperature

A: Given- Kw = 5.62 × 10-13 T= 100°C = 100 + 273 = 373 K

Q: 1) The pH of coffee is 4.9. What is the concentration of OH in coffee?

A: As per the company guidelines, we are authorised to solve only one question at a time. Please post…

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: do write the chemical formula for the conjugate base of selenic acid, H₂SeO04. e Write the chemical…

A: According to Bronsted and Lowry concept an Acid is a substance that has the tendency to donate a…

Q: 6.7

A: Here : O.35 M = C ( original concentration )  [H+] = √( Ka1 • C )  Using this formula, Calculate…

Q: What is the pH of 0.65 M ethanolamine, HOCH2CH2NH2, (Kb = 3.2 x 10−5)? pH =

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

Q: Enter your answer in the provided box. What is the pH of 0.105 M methylammonium bromide, CH3NH3Br?…

A: Step 1:As we know,pKb​=−log(Kb​)pKb​=−log(4.4×10−4)pKb​=3.36 Step 2:CH3NH3Br is the salt of strong…

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.