What is the [H+] when [OH-] = 8.1 x 10-5?

Q: NH4Cl pH of 0.1 M NH4Cl: 4.51     [H+] for NH4Cl     [OH−] for NH4Cl     Ka or Kb Value for NH4Cl?

A: As you have posted multiple sub-parts, and have not mentioned which question you want us to solve,…

Q: solution 0.1 M NHACI 0.1 M NaCN 0.1 M KCI 0.1 M C6H5NH3Br PH choose one 1 (lowest) 2 4 (highest)…

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Q: Calculate [OH-] and pH for a 1.5 x 10-3 M solution of Sr(OH)₂. b. a. [OH-] = 3 × 10-³ M; pH = 16.52…

A: The objective of this question is to calculate the concentration of hydroxide ions [OH-] and the pH…

Q: pH + pOH = 1.0 x 10-14  is this true or false?

A: pH + pOH = 1.0 * 10-14  This statement is false

Q: Ka for hypochlorous acid, HClO, is 3.50 × 10-8. K₂ for formic acid, HCOOH, is 1.80 × 10-4. Ką for…

A: Acids are chemical compounds which release H+ ons in solution. Higher the amount of H+ released,…

Q: Show computations for  [H+], pOH, [OH-] of the following substances. pH is already given.

A: Given: pH of baking soda = 10 pH of Kremil-S = 8 pH of Ascorbic acid = 4 pH of coffee = 5 We have to…

Q: The pH of a 3.65 M ammonia NH3 solution (Kb = 1.8 x 10-5) is? If hypochlorous acid HClO (Ka = 3.0 x…

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Q: Consider the following data on some weak acids and weak bases: acid base K. name formula formula…

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Q: Which of the following is the strongest acid? Group of answer choices hypoiodous acid (molar mass:…

A: In this question, we will see which acid is a strongest acid ( strongest acid means releasing H+ ion…

Q: The concentration of hydronium, [H 30 *], in a solution that contains a weak acid is 5.28 x 10-5 M.…

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Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: According to the Bronsted Lowry acid-base concept, an acid is a substance which loses H+ ions to…

Q: Calculate [H+], PH and POH respectively of CH3COOH solution has concentration 1.0 x 10-3 M and the…

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Q: True or False  Potassium hydroxide will produce less OH-1 ions when dissolved in water than…

A: Strong base produces more OH-1 ions in water than weak base.

Q: Consider the following data on some weak acids and weak bases: acid base K. K3 name formula name…

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Q: conjugate acid formula HNO₂ H₂CO3 Ka 4.5 x 10 4.5 X 10 -4 -7 formula 0 0 conjugate base CIO K₂ 0 0…

A: Answer:- This question is answered by using the simple concept of writing the formula for the…

Q: The K₂ of propanoic acid (C₂H₂COOH) is 1.34 × 10. Calculate the pH of the solution and the…

A: Given,                 Ka= 1.34 x 10-5                 [C2H5COOH] = 0.267 M

Q: Fill in the table rows. Maintain the same number of significant digits. pH [H+] [OH] pOH 1.9 4.73…

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Q: Determine the pH of a 0.275 M KOH solution. Give your answer to 2 decimal places in regular…

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Q: Consider the weak acid reaction:  HA + H2O  H3O+ + A-1 and the reaction of its conjugate base:  A-1…

A: The weak acid reaction is as follows: HA + H2O <-> H3O+ + A-1 The reaction of its conjugate…

Q: acid base Ka formula formula 9. name name hydrofluoric acid HF 6.8 × 10¬4 pyridine C3H;N |1.7× 10¬º…

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Q: acid base Ka name formula name formula hydrofluoric acid HF -4 6.8 × 10 hydroxylamine| HONH2 |1.1 ×…

A: Weak acids and weak bases have a common tendency of having a strong conjugate base and conjugate…

Q: Consider the following data on some weak acids and weak bases: base acid Κα name formula name…

A: The objective of the question is to classify the solutions in order of increasing pH.

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: The pH of the solution of NaBr will be close to 7 because NaBr is the salt of a strong acid (HBr)…

Q: Find the concentration of [H+] in 0.057M NaHSo3 H2So3 Pk1= 1.87 Pka2 =7.172

A: 2nd dissociation of H2SO3 i.e dissociation of HSO3- will give H+.

Q: What is the pH of a solution that is 0.040 M formic acid and 0.10 M formate (the conjugate base)?…

A: The objective of this question is to calculate the pH of a solution containing both a weak acid…

Q: Phenol, C6H5OH, is an acidic organic compound for which K₂ = 1.3 x 10-10. The structure of phenol is…

A: we have to calculate the pH of solution

Q: What is the H+ concentration of a solution with pH = 3.4 ?   What is the pH of a solution with…

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Q: ex: If [H₂0] in blood is 4.0 x 10% M, what is [OH-]? Isi acidic, basic, or neutral? KW = [H₂O"] [OH]…

A: Before solving the problems, we need to know about few relations.For determining [H3O+] or…

Q: © Macmillan Learning Classify each aqueous solution as acidic, basic, or neutral at 25 °C. Acidic…

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Q: Consider the following data on some weak acids and weak bases: acid Ka formula name name 8…

A: First two is acid and second two is base. So obviously HF and HClO will have lowest PH compared to…

Q: For propanoic acid (HC3H5 O2, Ka = 1.3 x 10°), determine the concentration of all species present,…

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Q: [H+] [OH-] pH Acid, Base, Neutral [OH] = (1 x 10 -14):1 x 10- %3D pH = (-)log(10^-5) 1 x 10-5…

A: pH < 7: acid pH = 7: neutral pH > 7: base

Q: The [OH1-] with a pH of 5 is Group of answer choices 1 x 10-5 M 1 x 10-7 M 1 x 10-9 M 1 x 10-10 M

A: Given: pH of solution = 5.

Q: ase help! Formic acid (Ka = 1.8 x 10-4) is used as a preservative on hay and animal feed.…

A: Ka of Formic acid = 1.8 x 10-4   Ka of Hypobromous acid = 2.0x 10-9 The concentration of Formic…

Q: Complete the table below  pH  [ H3O1+ ]  pOH  [ OH1– ]  ACID or BASE?  3.78…

A: The relationship between pH and pOH is  pH + pOH = 14 And pH = -log[H3O+] = 14 + log[OH-] And pOH =…

Q: [Review Topics] [References] Calculate the [OH] of each of the following solutions at 25°C. Identify…

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Q: alculate the [H+] of a substance with pOH =8.3 alculate the [H+] of a substance with pH =8.3

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Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: Step 1: Step 2: Step 3: Step 4:

Q: K, for benzoic acid, C6H; COOH, is 6.30 × 10-5. K, for phenol (a weak acid), C,H;OH, is 1.00 ×…

A: From the above data, Ka for acid is more = So, forming acid is the strongest acid. compared to…

Q: Reaction 1: NaOH(s) -> Na+(AQ) + OH-(AQ) Reaction two: Na+(AQ) + OH-(AQ) + H+(AQ) + -> H2O(I) +…

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Q: acid base K. K, name formula name formula HNO2 4.5 x 10 -4 nitrous acid pyridine C3H;N 1.7× 10-9 --…

A: pH of a compound is measured to determine the acidity of the respective compounds. Ph is negative…

Q: Be sure to answer all parts. What H3O+ concentration corresponds to each pH value: (a) pH = 12;…

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Q: What is the pH of a solution with [H3O+] = 4.5 x 10-5M?

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Q: Select the solution below that is the most acidic.     [OH–] = 1.0 × 10–12 M     [H3O+]…

A: The objective of the question is to identify the most acidic solution from the given options. The…

Q: Ph c) Ph 0= + hy Ph——CH

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Q: 1. Calculate the pH of each solution, given the hydronium ion concentration. a) [H,O'] = 0.0027…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Consider the following data on some weak acids and weak bases: acid base Bo Ka K, name formula name…

A: The given compounds are salts of given weak acids and base.  Weak base have conjugate acid salt and…

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.