What is the pH of a 0.47 M weak base solution (Kb = 9.55 x10-5)?

Q: What is the pH of a 5.0×10-2 M solution of KOH at 25 °C?

A:

Q: What is the pH of a 0.65M NaClO solution. (Kb=3.448x10^-7)

A: Negative Logarithm of concentration of [H]+present in the solution is known as pH of the solution.

Q: What is the pH of a 0.024 M acetic acid (Ka=1.8×10-5) solution at 25°C?

A: Given that, at 25°C, the concentration of the acetic acid solution is C = 0.024 M. The Ka of it is…

Q: What is the pH of a system that is 0.40 M in NH3 and 0.80 M in NH4Cl? (Kb = 1.8 x10-5 )

A:

Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…

A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…

Q: Would you expect a solution of ammonium chloride (NH4Cl) to be acidic or basic when added to water?…

A: Introduction- For the salts of strong acids and strong bases, the pH of salt will be neutral that is…

Q: Calculate the pH of each of the following solutions at 25°C. a 0.125 M HONH2 (K = 1.1 x 10-8) %3D pH…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is

A:

Q: What is the pH of an aqueous solution that is initially prepared as  0.40 M  Ca(ClO2)2 ?    Note:…

A: To calculate pH , we would use an ICE table for ClO2-.  For this first we would Calculate it's…

Q: If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?

A: From the relation, pOH is calculated as,

Q: Calculate the OH- for a 0.300 M solution of pyridine, Kb = 1.7 x 10^-9

A:

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: If a buffer solution is 0.300 M in a weak acid -5, (K = 2.6 x 10) and 0.470 M in its conjugate base,…

A: The Henderson-Hasselbalch equation is given as,

Q: What is the pH of a 3.6×10-2 M solution of KOH at 25 °C?

A:

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: 10. Fill in the gaps in the following table: pH 4.20 [H*] (mol/L) [OH]] (mol/L) Acid/Base Sol'n? 1.9…

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Q: If Kw is 2.9 x 10-15 at 10 0C, what is the pH of pure water at 10 0C ?

A: Given :- Kw at 10°C = 2.9 × 10-15  To be calculated :- pH of pure water at 10°C

Q: What is the ionization constant at 25 C for the weak acid (CH3)2NH2+, the conjugate acid of the weak…

A: The given solution contains a weak acid and a weak base.

Q: What is the pH of a solution of 0.075M HNO2 and 0.030 NaNO2?

A:

Q: The acid-dissociation constants of phosphoric acid (H3PO4) at 25 degrees Celsius are Ka1 = 7.510-3,…

A: Given data contains, Molarity of aqueous phosphoric acid solution is 2.5M.…

Q: What is the pH of a 0.85 M H2SO4?   Show your ICE table and calculations.  Ka1 for H2SO4 is a very…

A: The sulfuric acid completely disassociates in the solution, hence we can assert that the…

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 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: a value of 7.2 x 10*. What is the pH to 2 decimal -f hydrofluoric acid with a concentration of 0.537…

A: We will calculate pH

Q: What is the pH of a soln which  is 0.5 M NH3 and 0.075M NH4Cl? (kb=1.8x10-5)

A: The solution of NH3 and NH4Cl will form a buffer solution and the pH of a buffer solution is…

Q: A weak base, BOH, has a ph of 9.80 and Ka equal to 1.0 x 10-5. What is the Molarity of BOH?

A: Given data, The pOH of a weak base is calculated as shown below.

Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

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

Q: pH

A:

Q: Calculate the pH of a 0.021 M NaCN solution at 25 degrees Celsius. Ka (HCN) = 4.9 x 10^(-10). You…

A: Given, Concentration of NaCN solution = 0.021M. Ka(HCN) = 4.9*10-10. The hydrolysis reaction of NaCN…

Q: What is the pH of a 0.0100 M  solution of analine (C6H5NH2) , a weak base.     Kb= 4.0 x10-10

A: The chemical equation for aniline can be written as: This equation shows that aniline is a base,…

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

A:

Q: What is the pH of 0.10 bicarbonate (HCO3-) solution? Kb=2.4E-8. x= ? [H3O+] = ? pH = ?

A: The solution for the first part is as follows :

Q: what ph does a 12,7 M NaOH solute have?

A: NaOH ---> Na+ + OH–  [NaOH] = 12.7 M = [OH–]  So, pOH  = – log [OH–] pOH = – log (12.7) = 1.103…

Q: e pH of a 3.6x10-3 M Ba(OH)2 solution.

A:

Q: What is the pH of a 0.75 M solution of sodium cyanide, NaCN? (Kb for CN- = 2.5 x 10^-5)

A: NaCN is a salt of weak acid and a strong base. The pH of a salt of weak acid and strong base can be…

Q: What is the pH of 0.80 M methylamine (CH3NH2). Kb = 4.4x10-4.

A:

Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5

A: Given, Molar concentration of NH4Cl = [NH4Cl] = 0.1 M Base dissociation constant of NH3 = Kb = 1.8…

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: What is the pH of a 3.0 x 10 M solution of CoHsNH2 (Kb= 4.3 x 1010? What is the percent error in…

A: As PhNH2 is an weak base,it can be calculated using a formula.

Q: Calculate the pH for a 0.1 M solution of C6H5COOH (K, = 6.46 x 105) and the pH for a 0.2 M %3D…

A:

Q: Consider a 0.015 M hypochlorous acid solution (Ka = 3.0 x 10-8). pH = a =

A: pH and α is calculated by dissociation of hypochlorous acid and using the value of Ka.

Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?

A:

Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: what is the pH of an aqueous solution with [H3O+] = 2 x 10-14 mol L-1?

A: [H3O+] = 2 × 10-14 mol L-1  pH of the aqueous solution = ?

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 a 1.00 x 10^-9 molar solution of KCl?

A: KCl is a salt of strong acid (HCl) and strong base (KOH).

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

A:

Q: ph of 0.10 M NaNO2 (Ka of HNO2 is 4.5 x 10-4 ?

A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4

Q: What is the pH of a solution of 0.30 M CH:NH:Cl? Kb for CH:NH2 = 4.4 x 104

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.