alculate the pH of a solution of 0.100 M Na2SO3. Ka1 = 1.23 x10-2 ; Ka2= 6.6 x 10-8 A. 4.55 B. None of the given choices C. 1.54 D. 12.56 E. 10.08

Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

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

Q: Ka = 1.8 x 10-5 Ka1 = 4.3 x 10-7 HOAC H2CO3 %3D Ka2 = 5.6 x 10-11 Which of the following 0.01 M…

A:

Q: acia SOluti Select one: -5 а. 1.33 х 10 М -4 b. 3.76 x 10 'M -5 C. 2.66 x 10 M -5 M d. 5.32 x 10

A: Answer - The correct option is (d) 5.32*10^-5

Q: Calculate the pH of 2.99×10^−5 M NH4Cl. NH3 has a Ka = 5.68 x 10^-10 NH4^+1(aq) + H2O(l) NH3(aq)…

A: NOTE: In question its given incorrect as the specie NH3 is a base so its conjugate acid NH4+ will be…

Q: Which best describes the pH value of a solution with a H3O+concentration of 1.68 * 10 -5M? a. pH =…

A:

Q: 28. Which acid has the lowest pH? 0.040 M HCI A. B. 0.020 M HCIO4 C. 0.050 M HNO, D. 0.030 M HBr

A: pH : pH can be defined as the negative logarithm of hydrogen ion (H+) concentration. The formula is,…

Q: Calculate the pH of a 0.30 M solution of NH 4Cl (Kb for NH 3 = 1.8 x 10 -5). a. 11.67 b.…

A: NH4Cl is the salt weak base NH4OH and a strong acid HCl therefore hydrolysis constant Kh will be…

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: Formic acid, HCOOH, is a weak acid with a Ka equal to 1.8×10 –4.  What is the pH of a 0.115 M…

A: Given: Ka is 1.8×10 –4 Molarity of formic acid is 0.115 M. Introduction: A weak acid dissociates…

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2?   a. 10.2   b. 2.0   c. 9.0   d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: Determine the pH of a 0.288 M NH 3 solution at 25°C. The K b of NH 3 is 1.76 × 10 5. A. 5.48 B.…

A: The reaction taking place will be  NH3 (aq) + H2O (l) ----> NH4+ (aq) + OH- (aq) Hence Kb = [NH4+…

Q: Question 6 Saved Sulfurous acid (H,SO3, K, = 1.30 x 102, K2 = 6.30 x 10-8) ) is a diprotic acid.…

A: Given :  Ka1 of H2SO3 = 1.30 x 10-2  Ka2 of H2SO3 = 6.30 x 10-8  Concentration of NaHSO3 = 0.050 M…

Q: Calculate ao ai and a21. for a. picric acid in a solution with a pH of 1.250. b. oxalic acid in a…

A: a.

Q: Arrange the following solution from lowest pH to highest pH:

A: Acid and base are the chemical compounds which upon adding in water change the pH value accordingly.…

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

A: Given:- For a solution in a container,  No of moles of HCl = 2.60 x 10-3 No of moles of NaOH = 3.32…

Q: Calculate the pH for a 0.0183 M pyrophosphoric acid solution (H4P2O7).  Pyrophosphoric acid has…

A: pH is the hydrogen ion concentration present in the solution. It is calculated by taking the…

Q: A week diprotic acid H2A has Ka1 = 2.6 × 10–8 and Ka2 = 5.1 × 10–10. Determine the pH of a 0.067 M…

A: Answer is explained below. Since, given diprotic acid H2A is a weak acid thus, the salt NaHA is a…

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10.  What is the pH…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: A solution is prepared by diluting 10.1 g HNO 3 (MW=63 g/mol) with water to a volume of 1.5 L. What…

A: Hence the pH =0.97

Q: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

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:

Q: Which of the following is true about a 0.10 M solution of the weak acid HX, which has a Ka of 1.0 x…

A: we have given that Concentration of [HX] = C = 0.1M = 10-1 Ka = 10-5 we have given [HX] is weak acid…

Q: What is the pH of a 0.44 M solution of the weak base C6H5NH₂ (aniline)? Kb 4.2 x 10-10 3 4.87 b.…

A: Since you have posted multiple questions with multiple sub parts,we will provide the solution only…

Q: 4. A 500 ml solution of KOH was found to have a pH of 12.55. Calculate the concentration of [OH] in…

A: The pH value of a solution can be used as a measure of the concentration of hydronium ion (H3O+)…

Q: 1. Calculate pH of the following solutions: a. (H'] = 0.00001M b. (H'] = 2.30 x 10°M c. 0.05M NaOH,…

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: 4. What is the pH of 0.10 M Ba(OH)2 solution? A. 0.70 В. 1.00 С. 13.00 D. 13.30

A: The pH of a solution is given by, pH=-log[H+] The pOH of a solution is given by, pOH=-log[OH-] The…

Q: Which solution has the smaller hydrogen ion concentration? A. Solution A which has a hydrogen ion,…

A: Two multiple choice questions, which are to be accomplished.

Q: What is the pH of a solution that is 0.03M in picric acid and 0.1M in sodium picrate. pka=0.38 O a.…

A: The solution is mixed by adding picric acid to sodium picrate. Sodium picrate is made by adding…

Q: 3. The [OH] of a solution is 5x10(-6) M. What is the pH? O 6.7 8.3 8.7 6.3

A: First of all, we will calculate the concentration of [H+] from ionic product of water and from there…

Q: What is the pH of 1.0M solution of NaCN? [Ka HCN=4.9×10^-10] A. 2.3 B. 11.7 C. 7.0 D. 4.7 E. 9.3

A: pH of a solution is used to measure acidity or basicity of solution.Acidic solution have pH less…

Q: 2. A solution of NaOH has a pH of 13.87. Calculate the pOH of this solution.

A:

Q: You have a 0.0100 M solution of a weak base, B. True or False. a. [OH-] = 0.0100 M b. [B] = 0.000…

A: Given : Weak base, B with concentration = 0.0100 M

Q: Solutions of sodium salts of the acids in the following table are prepared with an initial…

A: Dissociation of a weak acid is given by: HA  ⇌  H+  +  A- The acid dissociation constant of this…

Q: 7. In the equation HCO3 + H2O → H30* + CO3 , Water is acting as c. a Bronsted Lowry acid a Bronsted…

A: This questions are solved using  conjugate acid base concept.

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: The pain killer morphine is a weak base when added to water. The Kb is 1.6 x 10-6. What is the pOH…

A: Here we have to determine the pH of 3.97×10-3M aqueous solution of morphine. Kb of morphine=…

Q: Which one of the following 0.1 M aqueous solutions has pH = 7? OA. NaF O B. NHẠNO3 O C. NaHSO, D.…

A: pH is defined as the negative logarithm of the H+ion concentration.                       pH =…

Q: 7. Determine the [H:O"1 concentration and whether the solution is acidic, basic, or neutral for: a.…

A: • We know,   • PH = 7 means Neutral.   • PH > 7 means Basic.   • PH < 7 Acidic.• H3O+ OH = Kw…

Q: Calculate the pH of a 1000 mL solution prepared by dissolving in water 0.600 mol of a weak acid HA…

A: The volume of the solution is = 1000 mL The mole of a weak acid, HA is = 0.600 mol The moles of…

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: It is an example of Henderson equation.  Here we are required to find the pH of the solution when…

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.