A week diprotic acid H2A has Ka1 = 4.2 × 10–7 and Ka2 = 4.8 × 10–11. Determine the pH of a 0.17 M solution of the salt NaHA. A. 9.6 B. 9.8 C. 10.2 D. 4.2 E. 10.4

Q: Which of the following statements is TRUE for an aqueous solution at 20 ºC? Select one: a.A neutral…

A: Solution is said to be neutral if it's pH is 7 or have same [H+] and [OH-] concentration at 25oC .

Q: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: 3. In the reaction below, H2O is a(n): H2SO; +H2O → H;O*+ HSO; a. Base b. acid Su conjugate acid d.…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Question 1 Calculate the pH of the resulting solution when 22.0 mL of 0.12 M KOH are added to 28.0…

A: In this question we have to tell the PH of the resulting solution.

Q: 3. Solution A has a hydronium ion concentration of 3.8 X 10-8 M. Solution B has a hydro- nium ion…

A:

Q: Which one of the following 0.1 M aqueous solutions has pH = 7?   A.  NH4NO3   B.  NaClO4   C.…

A: pH of 7 will only be given by a neutral solution.

Q: which of the following acid solutions has the highest pH? A. 30.0 mL of 1.00 x 10-2 mol/L H2S (aq)…

A:

Q: 4. Calculate the pH and pOH of each of the following solutions. a. [H*] = 1.0x10-M ph= 4,poh=10 =14…

A:

Q: The molar concentration of H+ ions in a solution is 5.8 x 10-9. The pH is a. 9.00 b. 5.80 c.…

A: pH can be calculated as pH = -log [H+]

Q: Part 1 of 2 sodium hypochlorite is the active ingredient in laundry bleach. The Ka is 2.9E-8.…

A: Answer: When salt of weak acid and strong has been dissolved in water then anion coming from weak…

Q: What is the pH of 0.0124 g Mg(OH)2 dissolved in 0.50 L pure water? a. 11 b. 10.93 c. 10.9 d. 10

A: Given that :  Mass of Mg(OH)2 = 0.0124g  Volume of solution = 0.50L Using Molar mass of Mg(OH)2 =…

Q: Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2b. 0.265 M NH4NO3…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: What are the answers to these questions?

A: 1.

Q: each mixture of acids. in HBr and 0.125 mol L in CH3COOH in HNO₂ and 0.085 mol L in HNO3 in HCHO₂…

A: We have to calculate the pH of the mixture. For this first we have to find out the H+ ion…

Q: In an analysis carried out with water (H2O) at 90 °C, a chemist found an amount of hydroniums (H3O+)…

A: Given :-  Concentration of hydronium ion at 90°C = 5×10-7 mol/L  Concentration of hydroxide ion at…

Q: Calculate the H3O+ and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

A:

Q: Question 7 Find the pH of a 0.183 M aqueous solution of hypobromous acid (HOBR), for which Ka = 2.06…

A: pH  calculation of weak acid :

Q: The pain reliever codeine is a weak base with a Kb equal to 1.6×10–6. What is the pH of a 0.250 M…

A:

Q: 9. Calculate the pH of a 0.10 M aqueous solution of acetic acid. (CH3COOH, 60.02 g/mol, K₂ = 1.8 x…

A: à

Q: Carbonic acid, H 2CO 3, is a diprotic acid whose Ka1 = 4.3 x 10 -/ and K a2 = 5.6 x 10 -11.…

A: The dissociation reaction for H2CO3 is as follows : H2CO3-------------> H+ + HCO3^- calculate Ka1…

Q: What is the concentration of H* ions in HCI whose pH is 8.3?

A: pH of the solution is equal to the negative logarithm of H+ ion concentration. Write the expression…

Q: he conjugate base of

A:

Q: What is the pH of a 0.379 M solutiôn of roxyla a. 0.42 b. 5.96 с. 3.19 O d. 6.38 O e. 4.2 x 10-7

A: Given, Molarity = 0.379 M Ka = 1.1 x 10-6  PH= ?

Q: 8. Dimethylamine (CH;),NH is a weak base with a pKa of 11.0 a. Calculate the pH of a solution of…

A:

Q: A solution containing 2.60 x 103 moles of HCl and 3.32 x 10-3 moles of NaOH into a container and…

A: So we’ve given the moles of HCl and the moles of NaOH. We will calculate the pH for the above…

Q: An acid mixture contains 0.60 M HClO (Ka = 2.9 × 10−8) and 0.50 M H2O2 (Ka = 2.4 × 10−12).  What is…

A:

Q: 4.Calculate the pH of a solution that is 0.311 M in nitrous acid (HNO2) and 0.189 M in potassium…

A: Te o predict the pH

Q: °C. What is the concentration of LIOH?

A: Given : pH = 13.14

Q: Calculate the pH of a solution that is 0.111 M in sodium formate (NaHCO2) and 0.253 M in formic acid…

A: The solution contains formic acid which is a weak monoprotic acid and salt of its conjugate base i.e…

Q: Calculate the pH of a solution containing 0.010 M HCOOH (Ka = 1.90 × 10-4) and 0.061 M HCI. A. 0.39…

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.