Write the equation which has       Keq = [AB2]2/[A2][B2]2

Q: Calculate the pH of 0.10 M solution of hypochlorous acid, HOCl, Ka = 2.9 x 10-8 (Weak acid) HOCl ⇌…

A: In multiple questions we solve only first question according to the Bartleby guideline. First find…

Q: Calculate the pH of a 0.0488 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka =…

A:

Q: Calculate pH of a solution of a 0.10 M CH3COOH solution? Ka = 1.8 x 10^-5 a. How many grams of…

A: Given: 0.10 M CH3COOH solution To find:  pH of the solution and the mass of CH3COOH used

Q: Determine the ka for each of the different concentrations for Acetic Acid              1.00 M…

A: Given that, (i) Concentration of acetic acid = 1.00 M    pH of the acetic acid solution = 2.65 We…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Ka = 4.5*10^-4 (given) pKa = – log [ Ka ] = – log(4.5*10^-4) = 3.347 Now, By using Henderson…

Q: What is the pH of a 0.025 M aqueous solution of Sr(OH) 2?   a. 12.40   b. 1.60   c. 1.30   d.…

A: The concentration of Sr(OH)2 = 0.025 M Strontium hydroxide is a strong base dissociates completely…

Q: Carbonic Acid Buffers and the case of the child that drinks 1L of Cherry Coke® 10 Reasons to NEVER…

A: Buffer:A buffer is a solution of equimolar concentration of weak acid and its conjugate base or weak…

Q: Amphetamine (C,H13N) is a weak base with a pKp of 4.2. Part A Calculate the pH of a solution…

A: 1-Phenylpropan-2-amine is amphetamine. Its molecular mass (M) is 135.23 g/mol Concentration of…

Q: Calculate the pH of a 0.0058 M solution of ascorbic acid. Ka = 7.9x10-5 Express your answer to two…

A:

Q: What is the pH of a 0.0830 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: Determine the pH of each solution. 0.23 M KCHO2 (Ka(HCHO2)=1.8×10−4) 0.18 M CH3NH3I…

A: We need to determine the pH of the each solutions below :1.  0.23 M KCHO2      Ka of HCHO2=1.8×10-4…

Q: 0.3 M solution of weak acid HX its dissociation rate is 27%. a) What is the dissociation constant of…

A: We will calculate ionisation constant and pH.

Q: What is [H30+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2? CH3CO,H(aq) + H20(1) = H30*(aq)…

A: Acetic acid and sodium acetate form buffer solution

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   pKb=-[logkb]pKb=-[log 1.7 ×…

Q: Calculate the pH of a 0.0058 M solution of ascorbic acid (a weak acid).  Ka = 7.9×10-5 Express your…

A: Ascorbic acid is an weak monoprotic acid.

Q: Calculate the [H+] and pOH of a 0.0005 M solution of Boric acid. Ka=5.90x0^-10​

A:

Q: What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 x 10-9?  The equation for the…

A: The relation between pH and pOH is given by, pH + pOH =14 Kb is the base dissociation constant. The…

Q: Calculate the pH of a 0.355 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.

A: Given : concentration = 0.355 M               Ka = 1.30 × 10-5

Q: What is the hydronium ion concentration in 0.275 M nitrous acid? Ka= 7.1x10^-4

A: We have to predict the hydronium ion concentration.

Q: Calculate the pH of a 0.315 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.

A:

Q: Calculate the pH of a 1.0L solution of 0.100M acetic acid 0.100M sodium acetate after the addition…

A: The given buffer solution is a mixture of weak acid acetic acid CH3COOH and conjugate base CH3COONa.…

Q: What is the equilibrium concentration of [H3O+] in a 0.20 M aqueous solution of HNO3? 10-7 M 0.4 M…

A: Given: Concentration of  HNO3 solution = 0.20M

Q: What is the pH of a 0.0013 M solution of niacin? Ka = 1.5x10^-5

A:

Q: What is the pH of a solution containing 0.30 M CH₃COONa and 0.10 M CH₃COOH? The Ka of CH₃COOH is 1.8…

A:

Q: how many liters of 0.54 monoprotic acid should be added to 685000 L of water with ph 7 to reach ph…

A: Given the desired pH of the acid solution with water = 5.2 Frist we have to find the [H+(aq)] from…

Q: Write down the reaction between [Cr(C2O4)2(H2O)2] and dilute potassium hydroxide.

A: Introduction: [Cr(C2O4)2(H2O)2] is a chromium (|||) complex in which C2O4 oxalate ion has a charge…

Q: The Ka of formic acid (HCHO) is 1.8 x 10^-4. Calculate the pH with a solution that is 0.15 M in both…

A: Given information is as follows; Ka = 1.8×10-4 HCHO  and  KCHO = 0.15 M           Determination of…

Q: What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when…

A:

Q: Calculate the pH of a 0.0153 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4)

A:

Q: A.) Calculate the pH of a 0.322 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka =…

A: A:  pH = 2.01   B:  pH = 2.69

Q: What is the pH of 0.025 M aqueous acetate ion? (Kb of CH3CO2– = 5.6 ×× 10–10)

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Acetic acid has a Ka = 1.8 x 10- 2 points 5 Determine the pH of a O.2 M acetic acid solution *…

A:

Q: Calculate the following: a) The pH of an aqueous solution of acetic acid that has a concentration of…

A: a.

Q: Determine the pH of a 0.10 M solution of sodium acetate (CH3COONa) at 25°C. (Ka of acetic acid = 1.8…

A:

Q: What is the pH of 0.15M solution of acetic acid? Ka of acetic acid (CH3COOH) is (Ka = 1.8x10-5 )

A: The PH of a solution is defined as :                                           The negative…

Q: 5. The pH of 0.800 M aqueous benzenesulfonic acid is 0.51. What is the value of Ka for…

A: Benzenesulfonic acid is a monobasic acid which means it has only one removable proton. Given data,…

Q: Determine the Ph of a 0.020 M solution of oxalic acid, H2C2O4. What is the concentration of C2O4 ion…

A: Oxalic acid is diprotic acid and Ka1 = 6.5 * 10-2 and Ka2 = 6.1 * 10-5 [Oxalic acid] = 0.020 M…

Q: What is the pH of a 0.0770 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)? 1 3 4 C 7 8 9 +/-…

A: PH = -log[H+] [H+] = 0.0770M

Q: Calculate the pH of a 1.00L solution containing 10.0mL of 5.0M acetic acid and 29.0mL of 0.3M sodium…

A: Acetic acid and sodium acetate form a buffer solution. The pH can be calculated using the…

Q: A solution is made by dissolving 16.7 g of CH₃NH₃NO₃ in 500.0 mL of water.   a)Write the acidic…

A: The compound given is CH3NH3NO3. Given : Mass of CH3NH3NO3 = 16.7 g And volume of solution = 500.0…

Q: Formic acid has Ka = 1.8 x 10-4. Calculate the pH of a solution that is 1.43 M sodium formate,…

A:

Q: If the pH value of an aqueous solution of trimethylamine [(CH3) 3N] is 10.75, what should be the…

A:

Q: Rank the following aqueous solutions in terms of pH. Why Are they in that order? (a)0.1 M CH3COOH…

A:

Q: A 0.121 M solution of acetic acid has a pOH of 11.20. What is the K3 of acetic acid? Oa. 2.5 x 106…

A: Given: The concentration of acetic acid is 0.121 M The value of pOH is 11.20

Q: A certain organic amine acts as a mono acid base in an aqueous solution. A 0.05M solution has a…

A:

Q: The Kp of ethylamine is 4.30 x 104. What is the pH of a 0.08457M aqueous solution of ethylamine?…

A:

Q: Trichloroacetic acid (CCl3COOH) is a corrosive acid that is used to precipitate proteins. The pH of…

A: Given information: Concentration of trichloroacetic acid (CCl3COOH) =  0.050 M Concentration of…

Q: Calculate [OH⁻] in a solution obtained by adding 1.50 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of…

A: Given: mass of KOH = 1.5 g volume = 1.0 L Molarity = 10.0 M NH3 Kb of NH3 = 1.80×10-5  moles of NH3…

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.