Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 x 10 M Select one: O a. 2.05 O b. 5.5 O c. 3.47 O d. 1.2

Q: The following question refers to the following system: A 1.0 liter solution contains 0.25 M HF and…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Convert the following pOH to [H+] concentration. pOH = 11.1, [H+] = _____________

A: pH is used to define the acidity or the alkalinity of a solution. pH is the negative logarithm of…

Q: following

A: When pH value less than 7 then Solution is acidic and if pH is greater than 7 then Solution is basic…

Q: 8. On a separate sheet of paper, draw a chemical model at the atom/molecule level illustrating what…

A: Acid Dissociation: When an acid dissolves in water, it releases one or more hydrogen ions (H+). This…

Q: 36. Determine the pH of 0.25 M HBr solution.* A. 0.30 O B. 0.52 C. 0.60 O D. 13.0

A: 1 mol of HBr contains one mole of each H+ and Br- ions each.

Q: The

A: Cl have more electronegative element than other so that it's Decreases the electrons charges density…

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: 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: 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: 7. Write a chemical equation showing how each of the following species can behave as indicated when…

A: The species which increases the H+/H3O+ ion concentration acts as an acid  The species which…

Q: The graph given below (Figure 1) shows [H+] vs. concentration for an aqueous solution of an unknown…

A: A) Since strong acids completely dissociates in solution producing H+ ions hence the concentration…

Q: The pH of a 4.6 x 10 -4 M Ca(OH) 2 solution at 25 °C is _____. Note that Ca(OH) 2 is a strong base.…

A: Given: The concentration of the Ca(OH)2 solution = 4.6 x 10 -4 M We have to calculate the pH of the…

Q: Determine the pH of 100.00 ml solution of 0.150 M oxalic acid following the addition of a. 50,00 ml…

A: The objective of the question is to determine the pH of the given cases.The pH is the measure of the…

Q: Question 11 Calculate the pH of a 0.30 M HNO3 solution. O 2.00 O 1.25 O 0.52 O 13.50 Question 12…

A: Given, [HNO3] = 0.30 M we know, HNO3 dissociate into one moles of H+ and one moles of NO3- which…

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: A given weak base solution is found to have [H+] = 4.3 x10-11 M. What is the [OH-] in this weak base…

A: In any aqueous solution at 25 degrees Celsius, the product of the hydrogen ion concentration [H+]…

Q: Calculate the value of [H3O+ ]and [OH− ] in each solution: a. 0.0001 M NaOH b. 0.0001 M HCl

A: Here, we have to calculate the value of [H3O+] and [OH-] for: 0.0001 M NaOH 0.0001 M HCl

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 .00055 M soln of NaOH?   A. 3.3 B. 1.3 E-3 C. 10.7 D. 1.55 E-7

A: Given  [ OH - ]   = 0.00055 M   PH         = ?

Q: The pH scale is used to express: a. The amount of water in a solution b. The concentration of salt…

A: We have to choose the pH scale is used to express for the following given options as follows in step…

Q: What is the pH of a solution with H306 M? A 5.8 b. 11.0 C.6.2 12. 4.3

A:

Q: 3. If the H+ concentration in an aqueous at 25.0 C has a value of 0.100M, what is the pOH of the…

A: pH of the solution can be calculated as below:

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: A solution has an OH- concentration of 1.0 x 10-3 mole/L. What is the solution's pH? a. 3.0 b. 4.0…

A:

Q: A 0.10 M solution of an acid has a pH of 3.0. The percent ionization is_________     0.30…

A:

Q: A given weak base solution is found to have [H+] = 4.3 x10-11 M. What is the [OH] in this weak base…

A: Step 1:     Option a is correct answer   Step 2: Step 3: Step 4:

Q: What is the pH of 0.010 M aqueous hypochlorous acid? (K, of HOCI=3.5 x 10-8) a. 4.73 b. 7.45 c. 4.50…

A: The concentration of the hypochlorous acid is [HOCl]=0.010M Ka=3.5×10-8 pH=?

Q: In the reaction NH3  +  H2O  →   NH4+  +  OH–, the Bronsted-Lowry base is

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= ?

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.