What is the pH of a 0.136 M aqueous solution of potassium fluoride, KF? (Ka for HF = 7.2×10-4) pH

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: The K, for dihydrogen borate anion (H,Bro,) is 1.72x105. What is the pH of a 0.188 mol L solution of…

A: For salt of weak acid & strong basepH = 12pKw + 12pK + 12logcc = concentrationKa = acid…

Q: The pH of a 0.173 M solution of a weak acid, HB, is 2.53. What is Ka for the weak acid?

A:

Q: For sulfuric acid, K >> 1 and K is 0.012. Calculate the pH of a 1.2 M solution of HSO.

A: Assuming the solution is H2SO4

Q: What is the pH of an aqueous solution of 4.96x102 M hydrobromic acid? pH

A:

Q: A.) What is the pH of a 5.3×10-3 M solution of calcium hydroxide? pH =  B.) What is the pH of a…

A:

Q: 2. Phenol, CH;OH can act as an acid in an aqueous solution. The Ka of phenolis around 2.1 x 10°, and…

A: pH = -log[H+] pOH = -log[OH]  Also, pH + pOH = 14 Also Ka and Kb has a relationship  Ka × Kb = Kw

Q: What is the H3O+ ion concentration in a 5.7 x 10^-4 M Ba(OH)2 solution? What is the pH?

A: Concentration of Ba(OH)2 = 5.7 x 10-4 M To determine : pH = ?

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: For the diprotic weak acid H2A, Kal = 3.9 x 10-6 and K22 = 7.7 x 109 What is the pH of a 0.0400 M…

A: The hydronium ion concentration can be calculated using ICE table as,

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

A:

Q: What is the pH of a 4.96×10-2 M aqueous solution of potassium fluoride, KF? (Ka for HF = 7.2×10-4)…

A:

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

A:

Q: 3. What is the pH of an aqueous solution when the concentration of hydrogen ion is 6.5 x 10-5 M?…

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: The weak acid, chloroacetic acid, is a useful reagent in organic synthesis owing to a reactive C-CI…

A: Given: Concentration of chloroacetic acid i.e. CH2ClCOOH = 5.68 X 10-2 M = 0.0568 M And Ka of…

Q: The [OH] in a 0.20M solution of NH4OH is: (Kb for NH4OH = 1.8 x 10-5) 3.6 x 10-6 M O 1.8 x 10-5 M…

A: Given: Initial concentration of NH4OH=0.20 M Kb of NH4OH = 1.8×10-5 Let x be the dissociated amount…

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: 12) What is the [H,O'] and pH of a 0.350 M HF solution? The K of HF is 3.5 X 104. HF (aq) + H2O (1)…

A:

Q: The pH of a 2.642M solution of a weak acid, HB is 2.34, What is the Ka for the acid?

A: Given: The conc. of the weak acid solution = 2.642 M HB is a weak acid with a pH = 2.34 A weak acid…

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.66. What is Ka for the weak acid?

A:

Q: What is the pH of a 0.150 M solution of acetic acid (pKa=4.75) at 25 degree celsius?

A: Given, the concentration of acetic acid =0.150 Mand pKa of acetic acid =4.75 at 25 °Cwe are asked to…

Q: 2. What is the pH, the pOH and the [OH] of a solution in which the [H*] = 2.43 x 10-6 M? %3!

A: pH is defined as  the negative log of hydrogen ion concentration  pOH is defined as the negative log…

Q: What is the pH of a solution that is O.245 MH2S and 0.160 M sodium hydrogen sulfide (NaHS)? The Ka…

A: The reaction between Hydrogen sulfide and sodium hydroxide is

Q: Lactic acid is produced in the tissues by anaerobic metabolism of glucose. Lactic acidosis occurs at…

A:

Q: 4. Sodium hypochlorite (NaCIO) is often found in household bleach. What is the pH of a 0.740 M…

A: We have to predict the pH of solution .

Q: Ammonia is a weak base that is a household cleaner and has a Kb =1.8 x 10-5. What is the pH of a 3.0…

A: Given: Kb =1.8 x 10-5Concentration = 3.0 M pH = ?

Q: What is the pH of a 3.1 x 10-4 M CsOH solution?

A: Given : concentration of CsOH = 3.1 × 10-4 M  To calculate :- pH of solution

Q: 5.) A typical aspirin contains 324 mg of aspirin (HC,H,O4) with Ka = 2.8 x 104. If you dissolve two…

A: pH = -log[H+] Aspirin is a weak acid. For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10–4.

A: Weak acids :-  Acids which do not undergo complete dissociation and produce very less number of H+…

Q: What is the pH of an aqueous solution of 2.37×10-2 M nitric acid? pH =

A: The important thing to keep in mind here is that nitric acid is a strong acid, which means that it…

Q: What is the pH of a 0.258 M aqueous solution of sodium nitrite, NaNO2 at 25 °C? (Ka for HNO2 =…

A:

Q: What is the pH of a 1.5 x 10² M H;SO, solution? Kai = large Ka2 = 1.2 x 102

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: What is the pH of an aqueous solution of 8.92x102 M potassium hydroxide? pH %3D

A:

Q: What is the pH of an aqueous solution of 6.78x102 M barium hydroxide? pH =

A:

Q: Calculate the pH of a 0.37 M solution of sodium hydrogen sulfite,  (6.0x10^-8). pH =

A: The pH of a 0.37 M solution of sodium hydrogen sulfite is to be determined. (Ka = 6.0x10-8).

Q: Calculate the pH of an aqueous solution of 6.45×10-2 M sodium sulfite.   pH = ?

A: Sodium sulfite is salt of mixture of strong base sodium hydroxide(NaOH) and weak acid sulfurous…

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 a 0.010 M solution of HF? The Ka for HF is 6.8 x 10^-4.

A: Given,   Concentration of HF = 0.010 M  Ka for HF is = 6.8x10-4

Q: What is the pH of a solution with a [H] of 3.5 x 10³? (K)

A:

Q: Calculate the pH of a 1.60 M KBRO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10º. 4.25 2.55…

A: ph is the gives the hydrogen ion concentration in the aqueous solution.

Q: 10. Acetylsalicylic acid (aspirin), HC»H;O4, is the most widely used pain reliever and fever…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: (6)  Is the salt C2H5NH3Cl acidic, basic, or neutral?                            What is the pH of…

A:

Q: Determine the pOH of a 0.461 M C,H5 COOH solution if the Ka of the acid is 6.5 X 10-5 5.48 O 11.74…

A: We will first write dissociation equation of acid, then calculate H+ concentration to find pH and…

Q: pOH

A:

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.63. What is Ka for the weak acid?

A:

Q: What is the pH of a 0.150 M aqueous solution of Magnesium hydroxide (Mg(OH)₂)?

A: Concentration of magnesium hydroxide = 0.150 M  pH of the solution = ?

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the value…

A:

Q: For the diprotic weak acid H₂A, Kal = 2.8 x 10-6 M and K₁2 = 8.9 x 109 M. What is the pH of a 0.0450…

A: Introduction :  Diprotic acid are those acids which produces two moles of hydrogen when they are…

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.