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 x 10-4 C. 7.2 x 10-10 d. 2.2 x 10 10 a O b

Q: Calculate the H3O+ ion concentration of a solution with a pH of 8.34 A. 2.88 x 10^-9 M B. 3.85 x…

A: Concept: We know that pH = -log [H3O+] So, Concentration of H3O+ can be expressed as [H3O+] = 10-pH

Q: What is the pH of a 1.8 x10^-2 M Ba(OH)2 solution?        A. 12.56 B. 2.85 C. 4.44 D. 6.38

A: Ba(OH)2 is a strog base. It dissociates completely to gibe Ba2+ and OH- ions Ba(OH)2  --------->…

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: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…

A:

Q: What is the pH of a solution with [H3O+] = 3.9 x 10-6M?

A: Given :-  [H3O+] = 3.9 x 10-6M  To be calculated :- pH of the solution

Q: The pH of a 0.50 M solution of the weak acid HA is 4.76. The value of Ka is O a. 6.0 x 10-10 O…

A: Given data :- Concentration of weak acid = 0.50 M pH of weak acid (HA) = 4.76

Q: At a certain temperature the Ka for the hydrogen sulfite ion, HSO," is 6.2 × 10⁹. Which of the…

A: Given,the molarity of NaHSO3 = 0.100 mol.L-1Ka = 6.2 x 10-8

Q: 22. A solution for which [OH-] = 3.0 x 10-10 is classified as a. acidic b. basic c. neutral

A: Given, [OH-] = 3.0 x 10-10 pOH = -log [OH-] pOH = -log[3.0 x 10-10] pOH = 9.52

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: For each strong base solution, determine [OH-], [H3O+], pH, and pOH.a. 0.15 M NaOH b. 1.5 * 10-3 M…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

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: Kb

A:

Q: 24. When any acidic substance enters the bloodstream, the bicarbonate ions neutralize the hydronium…

A:

Q: A solution has a pH of 8.0 at 25°C. What is the hydroxide-ion concentration at 25°C? O a. 8 M O b.…

A: pH is the negative logarithm of H+ concentration to the base 10 represented by: pH = -log H+ For 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: Calculate the pH of the following solutions and indicate whether they are acidic, basic, or neutral.…

A: Answer:

Q: 58/ Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HCIO4 c. a solution that is 0.045 M…

A:

Q: A solution which contains 0.10 M KOH has a pH which is ___________ that the pH of a solution which…

A: pH = -log H+pOH = -loh OHpH +pOH = 14Given , KOH = 0.10 mCA(OH)2 = 0.10 mpH = ?

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: 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: A week diprotic acid H2A has Ka1 = 4.2 x 10-7 and K2 = 4.8 x 10-11. Determine the pH of a 0.17 M…

A: Whenever a weak diprotic acid and strong base reacts with each other than it form a salt which…

Q: Calculate the pH of a solution if the concentration of H+ is 2.67 x10^(-5)M A. 11 B. 4.57 C. 7M…

A:

Q: Calculate the pH of a 1 x 10-5 M HNO, solution. a. 9 10 b.14 C. 5

A:

Q: What is the pH of a solution with [OH¯] = 1 x 10-5M ? A. 1 x 10-9 %3D B.9 C.5 D.5 E. 9

A:

Q: A 0.050 M solution of a weak acid, HA, has pH = 2.74. Determine the value of K₂.

A:

Q: 4. Calculate the [H*] or [OH] as required for each of the following solutions at 25 C, and state…

A: The question is based on the concept of PH and pOH calculations.   pH is defined as negative…

Q: + What is the pH of an aqueous solution composed of 0.64 M NH4 and 0.20 M NH3? (K₂ of NH4* = 5.6 ×…

A: The concept behind this answer is based on acid-base equilibria and the Henderson-Hasselbalch…

Q: Which of the following does NOT describe an acidic solution????? a. the pH is less than 7 b. the…

A: We need to find out the, which is not an acidic solution out of these 4:

Q: 10. Which solution would be expected to have the highest pH? (No calculation needed.) A. 0.50 M NaOH…

A:

Q: Calculate the pH and pOH of each solution at 25 °C.a. [H3O+] = 1.7 * 10-8 M b. [H3O+] = 1.0 * 10-7 M…

A: a. [H3O+] = 1.7 x 10-8 M pH = -log[H3O+] = -log (1.7 x 10-8 ) = 8 - log1.7 = 8 - 0.23 = 7.77 pOH =…

Q: Calculate [H+] in a solution that has a pH of 9.77. a. 5.9*10^9 b. 1.7*10^-10 c. 5.9*10^-9 d.…

A:

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

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.