If the pH of a 0.15 M acid is 3.6, what is the Ka? 10:3

Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: Which of the following is the weakest acid? OH A OH OMe B OH NO₂ C OH D OMe

A: The objective is to determine the weakest acoid.

Q: vingegar is 5.0% (w/v) solution of acetic (CH3COOH) in water, Acetic Acid's molar mass is 60.032g/…

A: We must convert the specified weight/volume percentage concentration to molarity in order to obtain…

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: What weak acid has a pKa of 5.02 and a molar mass of 201.0 g/mol?

A: Pka value is given by the formula  Pka=-logka. When the pka value is low it is more acidic in Nature…

Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–?  Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: An unknown weak acid with a concentration of 0.077 M has a pH of 1.80. What is the Ka of the weak…

A: The Ka of weak acid

Q: A solution that has a hydrogen ion concentration equal to 9.61 x 10-7 has a pH =

A:

Q: Calculate the pH of a 0.15 M acid solution; Ka=2.95 x10-8 Group of answer choices 4.18 6.36 2.09…

A:

Q: What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. VD…

A:

Q: Cyanic acid (HOCN) is an extremely acrid, unstable substance. What are the[H3O+] and the pH of 0.10…

A: Given  Concentration of HOCN (c) = 0.10 M Ka = 3.5×10-4 [H3O+] = ?  pH=?

Q: What

A:

Q: An unknown weak acid with a concentration of 0.320 M has a pH of 5.600. What is the Ka of the weak…

A: HA  ↔ H+ + A-Writing equilibrium expression for the above weak acid,Ka = [H+] [A-][HA]  But at…

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: What is the OH‾ ion concentration in a solution with pH = 4.75?

A: Given: pH = 4.75   Calculation for pOH:

Q: What is the concentration of barium hydroxide in an aqueous barium hydroxide solution with a pH of…

A: Given information: pH = 10.20

Q: concentration

A: [H+] = 10^-pH  [H+] = 10^-1.80  [H+] = 0.0158 M

Q: The pH of a 0.30 M solution of a weak base B is 10.22. What is the K, of the base? Be sure your…

A: From the given pH, we will get concentration of [H+] and from that concentration of [OH-]. And…

Q: An unknown weak acid with a concentration of 0.091 M has a pH of 1.80. What is the Ka of the weak…

A: Weak Acid - These are the acids that dissociate partially in water.  Given:- pH = 1.80 concentration…

Q: What is the pH of a 75.0 mL solution that is 0.049 M in weak base and 0.055 M in the conjugate weak…

A: The pH can be calculated by using Henderson equation  poH =pkb +log10 [ conjugate acid]/ [weak base]

Q: What is the pH of a 0.730 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: Interpretation: The pH of a 0.730 M solution of NaCN is to be determined. Ka of HCN = 4.9 × 10-10

Q: What is the concentration of [OH] if the solution with a pH=6.9?

A: Given : pH = 6.9

Q: What is the pH of 0.18 M sodium acetate solution? (Ka = 1, 8x10-5)

A:

Q: What is the pH of a solution which is 0.023M in weak base and 0.039 M in the conjugate weak acid (Ka…

A: This question can be solved using Henderson-Hasselblach equation. The equation is, pH=pKa+…

Q: What is the pH of a peach with a [¯OH] = 3.2 × 10-11 M? 3.51 (with margin: 0.1)

A: In the Question, we want to determine the pH of the Solution.  it is defined as a negative logarithm…

Q: A diprotic acid (H2AH2A) has ?a1=4.73×10−7Ka1=4.73×10−7 and ?a2=6.09×10−11.Ka2=6.09×10−11. What is…

A: pH is defined as the negative logarithm of hydrogen ion concentration. It can be given as  pH=-log…

Q: What is the pH of a 0.129 M monoprotic acid whose K is 2.738 × 10-³? pH =

A: pH is the negative logarithm of the hydronium ion concentration. The formula is pH = -log [H3O+]…

Q: What is the H+ concentration of a solution with a pH = 12.09?

A:

Q: What is the percent ionization of a 0.15 M solution of weak acid that has a pH of 1.86?

A:

Q: pH of a 0.30 M solution of a weak base B is 9.02. What is the K, of the base? Be sure your answer…

A:

Q: What is the pH of a 0.115 M weak base solution? The K of the weak base is 0.000096.

A:

Q: pH of the 2.5*10^3 M HA acid solution? ( Ka HA=1.8*10^-6)

A: Given, ka =1.8*10-6  Concentration of HA = 2.5*103 M

Q: What is the pH of a 0.0380 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH = 3.73

Q: Which of the following 1.0 M solutions would have the highest pH? Weak Acid Ka Weak Base Kb HCN 4.9…

A: Option - C is correct

Q: What is the pH of a solution that is 0.041 M in NH4Cl?

A: NH4Cl salt can be formed from weak base NH4OH and strong acid HCl. So it is a salt of strong acid…

Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

A:

Q: An unknown weak acid with a concentration of 0.070 M has a pH of 1.80. What is the Ka of the weak…

A: Weak acid dissociated feably in aqueous solutionpH is equal to negative logarithmic value of…

Q: An unknown weak acid with a concentration of 0.080 M has a pH of 1.80. What is the Ka of the weak…

A:

Q: A 0.036 M solution of a weak base is 0.019% ionized. What is the pH of the solution? pH= i What is…

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.