Find the pH of H₂M in a 0.100 M H₂M (Ka1-1.42 E-3) O 11.95 O 3.40 1.92 8.35

Q: If [OH" ] = 5.2 x 10-4 M, what is the pH ? pH РОН [H* ] [OH ] ? 5.2 x 10-4 M O -3.3 O 10.7 O -10.7 O…

A: given, [OH-] = 5.2 ×10-4 M

Q: What is the pH of 0.0085 M of the strong acid H₂SO4 (Ka2 = 0.012)? 1.90 2.29 1.42 2.42

A: Given,Molarity of H2SO4 = 0.0085 MKa2  of H2SO4 = 0.012

Q: What is the pH of [H30+]= 2.4 * 10 3 M?

A: Given :- [H3O+] = 2.4 x 10-3 M  To calculate :- pH of solution   pH = -log[H3O+]

Q: Which one is correct? What is the [H3O+] in a solution with pH=8? 10+8 M 10-8 M 8.0 M 6x10-8 M…

A: Given, pH = 8 PH is defined as negative logarithm of concentration of [H+] ion.

Q: If pOH = 9.7, what is [H*]? pH РОН [H*] [OH ] 9.7 ? O 2.0 x 10-10 M 04.3 М O 5.0 x 10-5 M O 2.0 x…

A:

Q: What is the pH of a solution in which [H3O]+ is 2.2 x 10-12 M? Group of answer choices 2.34 4.54…

A: It is given that the concentration of H3O+ in the solution is 2.2×10-12 M

Q: [H;O1+] 9.84 x 109M

A:

Q: 15. The [H3O+] of a solution with pH = 2 is Group of answer choices 1 × 10-12 M 1 × 10-2 M -10. M…

A: PH = -log[H3O+] Where, [H3O+] is the concentration of H+ in the solution So, PH is 2 when…

Q: What is the [H+] in a solution with a pH of 3.75?     Group of answer choices 5.6 x 103 7.5 x…

A:

Q: 13. What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?   Group of answer choices 3.0 2.52…

A: pH :-  The negative logarithm to the base 10 of hydronium ion concentration , [H3O+] expressed in…

Q: What is the pH of a solution with [ H3O+] = 1 × 10-7 M? Group of answer choices -7.0 5.0 -5.0…

A: To calculate pH of solution:

Q: What is the hydroxide ion concentration, [OH-], for a solution having a pH of 9.60? OA 2.5 x 10-10 M…

A:

Q: By what factor does an increase of 1.00 in pH change [H3O+]? 02 01/2 O 10 O 1/10

A:

Q: 2.s) Calculate the [H,O] in a solution with [OH]=6.5 x 10¹. Is the solution acidic, basic or…

A:

Q: The Kb for C₂H5NH2 = 5.6 x 10-4. What is the pH of a 0.60 M solution of C2H5NH2? 9.84 O 11.53 12.26…

A: Kb for C2H5NH2 = 5.6 ×10-4 Concetration  = 0.60 M

Q: The Ka for HN3 is 1.9 x 10-5.  What is the pH of a 0.35 M solution of HN3?

A: The pH of a weak acid can be calculated by the following formula. pH=-logCα   since…

Q: What is the hydroxide ion concentration of a NaOH solution that has a pH of 12.20? Choose from one…

A: Given :-we have to find the hydroxide ionconcentration of a NaOH solutionthat has a p H of 12.20.

Q: What is the concentration of [OH-] in chocolate milk if [ H3O+] = 4.5 x 10-7 M? Is chocolate milk…

A: Given, [H3O+] = 4.5 × 10-7 M We know, Kw = [H3O+] [OH-] = 10-14

Q: What is the pH of a solution with [H3O+] = 7.3 x 10-4 M? 4.00 -3.14 7.30…

A:

Q: What is the [H*] (M) of a weak basic solution with a concentration of 1.4 x 10-2 M and Kp is 6.4 x…

A: Given,  Base dissociation constant of weak base (say B) = Kb = 6.4 x 10-4  Concentration of B = 1.4…

Q: Overall: What is the pH of a 0.50 M solution of phosphoric acid? R I с E H3PO4 0.50 - X 0.50-x H₂PO4…

A:

Q: "Vhen 4.73 g of the weak acid HC6H4CIO is dissolved in 800 mL of olution, he pH is 5.25. What is the…

A: Ka is acid dissociation constant.

Q: Calculate the [OH-], pH and percent ionization for a 0.20 M aqueous NH3 solution.          NH3 + H2O…

A: The Kb is the equilibrium constant for the reaction of the base ammonia combining with water to…

Q: A flask of 0.70 M HBrO2(aq) has what pH? (Ka = 1.2 x 10-5) A 2.18 B 2.16 C 3.20 D 2.66 E 1.90

A: Given data contains, Molarity of HbrO2 is 0.70 M. Ka is 1.2 x 10-5.

Q: 3 of 15 If [H] in a solution at SATP is 0.0067 M, [OH]= O 6.7x10 17M O 1.5x10 12M O 2.2 M O 0.0063 M…

A:

Q: Calculate pH when given the following - [OH-]= 3.81 x 10-9M A. pH= 0.000000381 В. рH- 9.22 C. pH=…

A:

Q: If pH = 11.65, calculate [H+].

A: pH is defined as the negetive logarithm of the hydrogen ion concentration. That is, pH = - log [H+]…

Q: If a solution has a [OH] of 2.6 x 10-2 M. what would be the [H3O+]? A B 1 x 10-7 M 2.6 x 10-¹2 M C)…

A:

Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kai= 4.3 x 10-; Ka2 = 4.8 x 1011 %3D…

A:

Q: B. What is the pH of 0.75 M HC:H3O2 solution? K.= 1.8 x 105 and Kw=1.00 x 10-14 HC:H3O2 + H2O H30 +…

A: Calcuation as shown below

Q: Calculate the pH of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10-5) HC2H302 - H* + C2H3O2…

A: pH measures the strength of acids and base that how the solution is acidic and basic lower the pH…

Q: Question 3 What happens to the pH value as the concentration of OH increases? O It decreases O It…

A: pH is a scale used to measure acidity or basicity of an aqueous solution.

Q: weak base, B, has a pOH of 9.50. What is the value of K, for the solution? a 3.2 x 10-5 b) 6.3 x…

A: The pOH of weak base is 9.50We have to find Ka.

Q: What is the [H₂O*] in a solution that has a [OH-] = 8.30 × 10-7 M? X A) 2.0 × 10-10 M (B) 5.0 ×…

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.