Carbonic acid, H₂CO³ is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 × 10-¹¹. What is the pH of a 0.18 M solution of carbonic acid?

Q: What is the pH of a solution with [H3O+]=2.42 x 10-4?

A: pH of any solution is given by  pH = -log[H3O+] where [H3O+]= concentration of H3O+ ions

Q: An aqueous solution of Ca(OH)2with a concentration of 0.146 M was used to titrate 25.00 mL of…

A:

Q: hydronium ion concentration?

A: [H3O+] = 10-pH M

Q: calculate the equilibrium constant for the reaction

A: We are given  concentrations of H+ and Al(H2O)5OH2+ are found to be (2.74x10^-3) M  (1.3x10^-1) M in…

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 6.3 x 10-4 M? pH =

A: pH is equal to negative logarithmic of hydrogen ion concentration

Q: What is the pH of a solution containing 3.2 x 10-6 M hydronium ions

A: The pH of a solution determines the acidity and basicity of a solution, which is calculated using…

Q: The pH of a 0.225 M weak acid solution, HA, is 4.05, what is the K, of the acid?

A: pH = 4.05 pH = -log[H+] = 4.05 [H+] = 10-4.05          = 8.91 * 10-5 M

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 9.0 × 10-6 M? pH =

A:

Q: What is the hydronium concentration [H3O+] of a solution with a pH of 7.84?

A: We have given that pH is a measure of the hydrogen ion activity usually in aqueous solution.  pH =…

Q: Which of the following is not identified as a strong base? о Bа(ОН)2 o NH4OH o NAOH o LIOH

A: The strong base is

Q: Naturally occurring rainwater is acidic due to the presence of carbonic acid, H2CO3, produced when…

A: The problem is asking us to calculate the pH of rainwater given the concentration of carbonic acid…

Q: calculate the pH of the following solution; (a)2.8 × 10–⁴M Ba (OH)2 (b) 5.2 × 10–⁴M HNO3·

A: The given data : a) The concentration of Ba(OH)2 = 2.8×10-4 M b) The concentration of HNO3 =…

Q: Which of these is NOT an example of a strong base? O All of these are strong bases Ba(OH)2 ONH4OH O…

A:

Q: What is the pH of a 2.4 M solution of HCIO4?

A: Concentration of HClO4 = 2.4MpH =?

Q: Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

A:

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

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

Q: Calculate the pH of a solution that has a hydrogen concentration of 2.5 x 10-4 mol/L.   (2A)

A:

Q: A solution of hydrobromic acid has [HBr] = 1.3×10-2 M. What is the pH of this solution

A: As per guidelines if multiple questions, first question is allowed to answer, please post  questions…

Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: In HClO2 the ions present are H+ and ClO2 -. Similarly in Ba(OH)2 the ions present are Ba2+ and OH-.…

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.0 × 10-7 M? pH =

A: The concentration of hydrogen ion in the solution is too low thus, the pH of the solution is the…

Q: A sample of vinegar has a hydronium ion concentration of 5.7 x 10¬ 3 M. What is the pH of this…

A:

Q: A diprotic acid, H₂A, has Ka, = 3.5 x 105 and Ka₂ = 9.2 × 10-1⁰. What is the concentration of the…

A:

Q: CALCULATE PH IF [H3O+] = 4.02 X 10 -3 AND [H3O+] = 8.99 X 10 -7

A: Given[H3O+] = 4.02 X 10-3 [H3O+] = 8.99 X 10-7pH = To be determined

Q: What is the pH of a 0.0338 M nitric acid, HNO3, solution?

A:

Q: needs from the soil if its pH is above 6.5. (a) The hydrogen ion concentration of a soil sample is…

A: A) [H+] =1.58×10-7 pH = -log([H+])  = -log(1.58×10-7) = 6.8 So, pH = 6.8

Q: Phthalic acid (H₂CH₂O₂) is a diprotic acid with Kal = 1.12 x 10-3 and K₁2 = 3.90 x 10-6. Determine…

A: Given : acid is diprotic

Q: A solution of sodium cyanide, NaCN, has a pH of 11.40. How many grams of NaCN are in 245 mL of a…

A: Molarity is defined as moles of solute present per liter of solution.

Q: What is the pH of a 0.138 M solution of H2SO4 (sulfuric acid)?

A: We will use formula of pH

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H] = 8.5 x 10-7 M? pH =

A:

Q: The Ka value for acetic acid, CH,COOH(aq), is 1.8 × 10-5. Calculate the pH of a 1.20 M acetic acid…

A: Acetic acid dissociates as: CH3COOH→CH3COO-+H+

Q: Complete the balanced chemical reaction for the following weak base with a strong acid. In this…

A: Since, NH3 is a weak base and HCl is an acid, so reaction between acid and base forms salt (ammonium…

Q: A diprotic acid (H₂A) has Kal = 4.54 x 10-7 and K₁2 = 5.59 x 10-11. What is the pH of a 0.396 M H₂A…

A: we have to calculate the pH of 0 .396 M diprotic weak acid

Q: What is the pH of a 0.950 M solution of Na2HPO4?

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: It is found that 41.27 ml of 0.2017 M NaOH is required to neutralize 25.00 ml of HNO3 solution in a…

A: Given : Molarity of NaOH = 0.2017 M Volume of NaOH solution required = 41.27 mL And volume of HNO3…

Q: What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH?

A: Given information: Concentration of benzoic acid = 0.40 M

Q: A solution of sodium cyanide, NaCN, has a pH of 11.90. How many grams of NaCN are in 615 mL of a…

A: Given, The pH of the solution = 11.90 The volume of  NaCN = 615 mL = 0.615 L The molar mass of NaCN…

Q: What is the pH of a 0.1 M solution of HF? (Hydrofluoric acid K₂ = 7.1 x 10-4)

A: Concentration of HF solution (C) = 0.1 MKa of HF = 7.1 × 10-4pH of the solution = ?Note:…

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.