18.)  What is the pH of a solution with [OH-] = 1.8x10-5? a. 4.75 b. 9.25 c. 7.00 d. 4.76 e. 8.25

Q: 10. What is the hydrogen ion concentration of a solution with a pH of 10.33? 2.14 X 10-³ 4.68 X 10-4…

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

Q: 105. Determine the pH of each solution. a. 0.10 M NH,CI c. 0.10 M NaCl b. 0.10 M NaC,H;Oz

A:

Q: 13. What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb=1.7x10-9) A. 8.77 B.…

A: Given that,Concentration of pyridine,Kb value for pH of the solution = ?

Q: 535 mL of HCl(g) at 26.5 °C and 747 torr was dissolved in enough water to make a 625 mL solution.…

A: Given,  535 mL of HCl(g) at 26.5°C and 747 torr was dissolved in water make a 625 mL solution the pH…

Q: 5.12

A: PH

Q: Arrange the following in increasing PH: a. II, III, I, IV b. IV, I, II, III c. II, III, IV, I d. I,…

A:

Q: 27. If exactly equal mole amounts of KOH and HCl are reacted in a pure water solution, what will be…

A: The balanced chemical equation for the chemical reaction between KOH and HCl can be written as…

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: 1. IfH ions in the solution increases, a The more basic is the solution. b. The solution becomes…

A: Acidity and basicity of a solution can be measured by using pH scale. pH less than 7 means solution…

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: Which of these could be the pH of a very concentrated solution of a strong acid? a. 6 b. 0  c. 9…

A: CORRECT ANS- B)0

Q: If a solution of aspirin has a [OH-] = 4.4 x 10–12 M, what is the pH of the solution?

A: Given, [OH-] = 4.4 ×10-12 pH is the negative logarithm in hydrogen ion concentration.

Q: What is the pH of a solution that contains [OH-] = 0.0010 M? a. 3.00 b. 5.00 c. 11.00 d.

A: The question is based on the concept of PH. pH is defined as negative logarithmic of hydronium ion…

Q: 10. What is the hydrogen ion concentration of a solution with a pH of 10.33? d. 4.68 X 10-4 e. 2.14…

A: The objective of this question is to calculate the hydrogen ion concentration of a solution given…

Q: What is the pH of IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: 25. In a solution containing 10-8 M HCI and 10-8 M acetic acid, H* is supplied mostly by A. The…

A: In a solution containing 10 M HCl and 10 M acetic acid, H+ is supplied mostly by:A. The strong…

Q: The poison strychnine is a weakly basic compound with Kb = 1.8 x 10 What is the pH of a 0.058 M…

A: Given that, 0.058 M solution of a weak base, i.e. C = 0.058 M. The Kb is 1.8×10-6. We have to…

Q: 22. Hydrochloric acid (HCI) is a strong acid, and Hydroiodic acid (HI) is a weak acid. Which of the…

A: Introduction: As per Bronsted-Lowry concept, an acid is a substance that can donate H+ ions and base…

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: What is the pH of a solution made by mixing 40.0 mL of 0.20 M HCl with 40.0 mL of 0.10 M KOH?…

A: HCl and KOH will react as per the following reaction HCl + KOH --> KCl + H2O

Q: One aqueous solution of a strong acid has pH = 1.20, another pH = 1.80. If equal volumes of these…

A: First find the H+ concentration of both the solutions and find H+ concentration after mixing the…

Q: The pH of a 0.0040 M solution of Ca(OH), is A) 13.02 B) 11.90 C) 11.60 D) 2.097 MacВook Air

A: Given Concentration of Ca(OH) 2 = 0.0040 M Concentration of OH- = 2 x 0.040 = 0.0080 M

Q: 14. A solution contains 3.25 x 10 moles of hydroxide ions per litre. What is the pH of the solution?…

A: We know , hydroxide ion = [OH-]             and,   pH+pOH = 14                 So, pH = 14-pOH and…

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: Calculate the pH of a solution prepared by mixing 30 ml of 0.1 N NaOH and 25 ml of 0.1N HAc. A. 2.46…

A: Acid-base titration is an analytical technique utilized to determine the unknown concentration of an…

Q: Calculate the pH of a solution if the concentration of OH- is 2.67 x10^(-5) M A. 14 B. 4.57 C.…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: What is the pH of a solution that is 1.67x10-5M H+?a. 4.8b. 5.2c. 0.22d. 10.2

A: According to question,  Concentration of H+ ion is = 1.67* 10-5

Q: What is the pH of a solution that is 0.40 M in HCN? The Ka for HCN is 4.0x10-10. a. 0.40 b. 9.40 c.…

A:

Q: 3. Identify the following as strong acids, weak acids, strong bases, or weak bases. a. HBr. b. HCN…

A: We have to identify given chemicals, as strong acid/base and weak acid/base

Q: If the OH- ion concentration in an aqueous solution at 25.0 C is measured as 3.4 x 10-3M what is the…

A: 1.Given, Concentration of OH- ion = 3.4*10-3M. Ionization constant of water, Kw = 1.0*10-14.…

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

A:

Q: A solution with (OH- )of 5 x 10^3 has a pH of? A.-2.3.   B. 11.7.   C 7.0. D. 2.3

A: (b) 11.7 Concentration of OH- ions = 5×10-3 Now, pOH = -log[OH-]                    = -log (5×10-3)…

Q: What is the pH of a 3.1 x 10-3 M LiOH solution? a. 11.5  b. 2.51 c. 11.2 d. 2.64

A: To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion…

Q: What is the pH of an aqueous solution at 25.0 °C in which [H+] is 0.0030 M? A. -5.81 B. 2.52 C.…

A: pH is the measure of acidic or basic nature of the aqueous solution of a substance. The pH of the…

Q: Calculate the pH of a solution that is 0.0060 M in HClO4 and 0.0060 M in HCN. Ka of HCN is…

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.