The concentration of H* (or H3O*) from part A should be 1.02×10¬2 mol L-1. What is the pH of the solution?

Q: Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3…

A: The pH of a solution can be calculated as follows: pH= 14-pOH where pOH = -logOH- To calculate…

Q: A chemist takes 8.579 mL of liquid acetic acid, CH,COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

A:

Q: What is the pH of rainwater saturated with carbon dioxide at 25 deg C is the CO2 concentration is…

A: 1- First determine the concentration of CO2 in M unit :  Concentration of CO2 = ( 300 mg / L)…

Q: 1) Calculate the pH of a solution prepared by dissolving 2.20 g of sodium acetate, CHCOONA, in 78.0…

A: Given: mass of sodium acetate=2.20 gvolume of acetic acid=78.0 mLmolarity=0.10 MKa=1.75×10-5 To…

Q: A. Calculate the pOH of each of the following solutions: 1) 0.5 M of Ca(OH), 2) 0.0235 Mof HCI 3)…

A:

Q: What is the pH of a 0.0810 M solution of HONH;CI (Kb of HONH2 is 1.1 x 108)?

A: Given,                HONH3Cl -----> HONH3+ + Cl-  Hydrolysis of the weak conjugate acid, HONH3+…

Q: The autoionization constant of water (K„) is 1.139 × 10-15 at 0°C and 9.614 × 10-14 at 60°C. (a)…

A: a) calculate the standard enthalpy of autoionization of water. Given: (Kw)1 at 0oC = 1.139×10-15…

Q: an aqueous solution containing 3 grams of CH3COOH in 500 ml of it and having a pH = 3 solution of…

A: Given that,  pH of 500 mL solution containing 3 g CH3COOH = 3 Molarity of CH3COOH solution = (3…

Q: What is the pH of a 0.0500 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: HONH3Cl is a salt and in solution it gets dissociated as HONH3Cl → HONH3+ + Cl- The hydrolysis…

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: The weak base dimethylamine, NH(CH3)2, has a molar mass of 45.09g/mol and a base-dissociation…

A: pH is used to measures the concentration of hydrogen ion. The expression for calculating the pH is…

Q: Below is the reaction for the formation of acid rain due to high concentration of atmospheric…

A:

Q: Calculate the pH of a solution made by dissolving 1.87g of sodium caproate (NaC6H11O2) in water and…

A: We will calculate pH

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: The concentration of OH- in a solution of householdbleach is 3.6 × 10-2 M. Calculate the pH of the…

A: Given here the Concentration of OH- in a solution [OH-] = 3.6 ×10-2 M . we are asked to calculate…

Q: A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

A:

Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 :will be respectively…

A: Kh=kWkC pH + pOH = 14  From Ostwald's dilution law ,  pOH=-logkbxc Where c is the concentration of…

Q: The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its…

A:

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…

A: Given: Ka value of acetylsalicylic acid = 3.00×10-4

Q: What is the pH of the resulting solution

A:

Q: The value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of Kp, for its conjugate…

A:

Q: The substance benzoic acid (C6H5COOH) is a weak acid (K₂ = 6.3x10-5). What is the pH of a 0.230 M…

A:

Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH  POH= -log[OH-]

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: Calculate the pH of a 1.50 M (CH»),NHB solution (aq., 25 °C). 3) Kb (CH3)N - 6.31 x 105

A: (CH3)3NHBr is a salt of weak base and a strong acid formed by the reaction of  trimethyl amine…

Q: The pH of a solution at 25°C in which [OH]= 2.0 x 10 is: 1 9.52 4.76 4.69 3.30 9.30

A: In this question, we want to determine the pH of the Solution.  You can see details Solution below…

Q: The PH of a Oil M agueas sólutiom of Naz( the sodium salt of 2s 10,70: what is thie ha for Hz?

A: Given: Concentration of NaZ solution = 0.15 M pH of NaZ solution                   = 10.70

Q: Aniline (C6H5NH₂) is an organic base used in the manufacture of dyes. Calculate the pH and the…

A: Given,  The concentration of Aniline ( C6H5NH2 ) = 0.15 M.  The Kb of aniline = 4.3 × 10-10 M.  The…

Q: Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL…

A: Buffer solution is a aqueous solution consisting mixture of  weak acid and its conjugate base or a…

Q: Calculate the pH of a mixture made by adding 54.6 mL of 0.015 M HHNO3(aq) to 142.9 mL of water at…

A: Given,  The pH of a mixture made by adding 54.6 mL of 0.015 M HNO3(aq) to 142.9 mL of water at 26.6…

Q: .623 g of NaC2H3O2 are placed in a solution of 0.105 M HC2H3O2 to make 1.00 L of solution. What is…

A: pH is negative logarithm of Hydrogen ion concentration

Q: Calculate the pH and pOH of a solution resulting from dissolving 0.75 grams of perchloric acid in…

A: Given: Mass of perchloric acid i.e HClO4 = 0.75 g And volume of solution = 1500 mL = 1.500 L…

Q: What is the pH of a 0.248 M aqueous solution of potasslum acetate, KCH,CO0 at 25 °C? (K, for CH,COOH…

A: 1.) Potassium acetate is a salt of conjugate base of acetic acid. So we would draw ICE table and use…

Q: The pH of an aqueous solution of 0.144 M ammonium perchlorate, NH4ClO4 (aq), is . This solution is

A:

Q: The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2.  What is the pH of…

A: The ionisation reaction for the  dichloroacetic acid will be  HC2HO2Cl2 ------> H+ + C2HO2Cl2-…

Q: The pOH of an aqueous solution of 0.590 M phenol (a weak acid), C6H5OH, is _____

A:

Q: Q6) 200 ml , o.0ol M NAOH is udded to 30oml, o.0005 M HCL. what is the PH of the Soluution ? Ans. :…

A: The balanced Chemical Reaction between HCl and NaOH is - HCl + NaOH ----> NaCl + H2O Here, one…

Q: The [H3O+] = 4.7 x 10-5 M for the HC7H5O2 and NaC7H5O2 solution. What is the pH of the solution?

A: Given H3O+ concentration of the solution, [H3O+] = 4.7*10-5 M

Q: A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

A:

Q: What is the pH of an aqueous solution of 0.005 M C6H5O- at 298 K of the Ka for phenol at the given T…

A: Given: Concentration of C6H5O- = 0.005 M And Ka of C6H5OH = 1.0 × 10-10

Q: The first acid ionization constant of the oxoacid H;PO, is 8 x 10-2. What molecular structure do you…

A: H3PO2 is a monoprotic acid in aque.

Q: The pH and Kh of O.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 will be respectively equal…

A: Value of pH is used to measure extent of acidity or basicity of a solution. At room temperature,…

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10¬1º. Calculate the pH of a…

A: Given, initial concentration of HCN = 3.0 M            Ka for HCN = 6.2 x 10-10 The hydrocyanic acid…

Q: Calculate the pH of an aqueous solution of 1.00 M iodic acid at 298K.

A: The equation for the dissociation of Iodic acid is,

Q: prepared

A: Equilibrium Reaction is :  F^-(aq) + H2O(l) <------> HF(aq) + OH-(aq)    Major species are :…

Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

A:

Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…

A: Ans. 3.33*10-11

Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…

A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…

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.