3. Calculate the [H3O+], [OH-], pH, and pOH of a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

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Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: The given data contains, Ka= 7.10×10-4 Concentration of HNO2 = 0.120 M

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Q: Which of the following relationships in incorrect? Assume 25°C. a. pH + pOH = 14.00 b.…

A: b. [OH-] = 10pOHExplanation:Incorrect Option:Option b:[OH-] = 10pOH: This relationship is…

Q: 2. Calculate the following (report to 2 decimals, use scientific notation when calculating H3O*) and…

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Q: Calculate the [H3O+] of 0.15 M hypobromous acid, HOBr. Ka = 2.40 x 10-9

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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: Complete the table. (The first row is completed for you.) Acidic or [H3O*] [OH] POH pH Basic 1.0 ×…

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Q: [H3O+] 3.2X10-7 6.9 x 10-8+ Inf0% 8.7 x 10-7 [OH-] 2.4 x 10-¹0 pH 1.7 7.16 6.06 11.1 Acidic, basic…

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Q: Calculate the [H +], [OH -], pH , pOH of 005 M NH3     Kb=   1.8 x 10 -5

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Q: Calculate [H+] for a 3.41×10-2 M aqueous solution of nitrous acid (HNO2; Ka = 4.0×10-4).   2.…

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Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: pH of a solution is given by the negative logarithm of hydrogen ion  concentration in the solution…

Q: Calculate the [H+] and pH of a 1.97 × 10-4 M nitrous acid solution. The K, of nitrous acid is 7.10 x…

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Q: What is the pH of a 0.04 Mof the diprotic acid H2CO3 solution? Kal= 4.3 x 10-7; Ka2 = 4.8 x 10-11.…

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Q: a. Calculate the pOH of the solution given the [H₃O⁺]= 1.0 x 10⁻⁸ M b. Calculate the pH of the…

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Q: Use the concentrations of [H3O*] and [OH] to calculate the missing concentration and indicate…

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Q: Maleic acid (H,C,H,O,) is a diprotic acid with Kal = 1.20 × 10-3 and Ka2 = 5.37 × 10-7. Determine…

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Q: Calculate the [H​3​O​ +​ ], pH, [OH​-​ ] and the pOH for a 0.015M HNO​3​solution.

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Q: Calculate the concentration of OH-(aq) in a solution in which [H3O+] is 2 × 10-6 M.

A: [H3O+] [OH-] = kw  kw = 1 × 10-14

Q: Which of the following is the most acidic (lowest PH) pOH of 2.0 [OH-] = 1 x 10-7 m [H+]=4.6 x…

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Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. O 4.3 x 10-4 8.6 x 10-6 O 4.9 x…

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Q: The Ka for lcarbonic acid is 1.8 × 10–5. Which of the following statements best describes the pH of…

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Q: propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M

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Q: What is the [H3O+¹] of a solution with pH = 5.900 ? OA. 9.00 x 10-5 M OB. 1.26 x 10-6 M OC. 5.00 x…

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Q: If pH = 9.3, what is [H* ] ? pH pOH [H*] [OH ] 9.3 ? O 2.0 x 10° M O 1.1 x 10-15 M O 2.0 x 10-5 M O…

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Q: Calculate the [H +], [OH -], pH , pOH of 0.005 M NH3 Kb= 1.8 x 10 -5

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Q: 15. Calculate the pH for these solutions which have the following H3O+ concentrations.  [H3O+] pH…

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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.