Calculate the pH of a 0.20 M solution of NaC2H302. HC2H3O2 has a Ka-1.8 O a. 8.56 O b. 7.00 Oc. 9.02 Od. 4.98 O e. 5.44

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: 37. A solution has a pH of 10.65. What is the [H3O+] value for this solution?\ a. 2.2 x 10-11 b. 4.5…

A: In Chemistry, pH is a scale which is used to specify the acidity or basicity of an aqueous solution.…

Q: An aqueous solution of a weak acid, HA is prepared by dissolving 0.030 mol of HA in water to yield…

A:

Q: Calculate the pH of a solution of 0.100 M H2SO3. Ka1 = 1.23 x10-2 Ka2= 6.6 x 10-8

A: First dissociation                                                                2nd…

Q: The pk, for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.95 O b. 1.24 O c.…

A:

Q: What is the pH of 0.01 mol.L-¹ KOH solution ? Select one: a. 0 b. 2 c. 7 d. 12 e. 14

A: Given,0.01 mol.L-1 KOH solution .Required,                  The pH of the above solution .

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: T he pH of aqueous 0.050M trimethylamine is 11.24, what is the K b of this base?  Trimethylamine…

A:

Q: Calculate the pH and pOH of an aqueous solution that is 0.75 % HCI, by mass, and has a density of…

A: Given :-  % by mass of HCl = 0.75%  density of solution = 1.04 g/mL  To calculate :-  pH and pOH for…

Q: Calculate the pH of a 2.4 M Ca(OH)2 aqueous solution. a. 14.7 b. 13.3 c. 13.6 d. 14.4

A: Ca(OH)2 is strong base hence it dissociated fully in solution

Q: 1. Calculate the pH of the following: a. A solution whose pOH = 5.73 b. 12.0 M HNO3 c. 0.076 M…

A: Calculate the pH of the following---

Q: 40. The pH of a sample of human blood was measured t be 7.52 at 25°C. Calculate pOH [H+], and [OH-]…

A:

Q: C. A 0.0543 M solution of a weak acid HA has a pH of 4.87. Calculate K, and % ionization of a the…

A: There is more than one question, and all are different. As per answering guidelines I can answer…

Q: Which acid is monoprotic. O a. HSO4 O b. H3PO4 O c. H2SO4 O d. HNO3

A:

Q: The pKa of HOCl is 7.5. Calculate the pH of a 0.41 M solution of HOCl. a. 6.50 b. 3.94 c.…

A: Given ,  pKa = 7.5          so, - log(Ka ) = pKa = 7.5                  => Ka  =  10(-7.5)…

Q: Calculate the pH of each of the following solutions. Is the solution acidic or basic? a. [H+] = 2.6…

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

A:

Q: The following are all STRONG ACIDS. Rank the three solutions from lowest to highest value of pH A.…

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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.