What is the pH of a NaOH solution that has a H* concentration of 8.5 x 10-¹² M at 25 °C?

Q: Write the formula of the conjugate base of CH3CO2H

A: Conjugate base of an acid contains one less proton.

Q: The base protonation constant K of azetidine (C3H6NH) is 1.5 × 10 -8 Calculate the pH of a 0.17 M…

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Q: The acid dissociation constant Ka of hypobromous acid HBrO is 2.3 x 10^−9. Calculate the pH of a…

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Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.7 × 10⁻³. What is [H⁺]?

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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: Calculate the pH and pOH of the following substances: 1. 0.3 M sulfuric acid (H2SO4) solution 2.…

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Q: What concentration of an aqueous solution of NH4+ has the same pH as that of 6.8 × 10–5 M HCl? The…

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Q: Calculate the pH of a .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

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Q: Complete the balanced chemical equation for the following reaction between a weak acid and a strong…

A: Balanced chemical equation is the equation in which number of atoms on both sides of equation are…

Q: The OH concentration in an aqueous solution at 25 °C is 7.1 x 10-5. What is [H*]?

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Q: The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10¯4) is

A: Concentration of HF solution (C) = 0.532 MKa for HF = 7.20 × 10-4 pH of the solution = ?

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 8.9 × 10⁻³. What is [H⁺]?

A: Product of hydrogen ion concentration and hydroxide ion concentration is equal to the ionic product…

Q: What is the pH of a 0.1 M solution of methylamine hydrochloride (CH3NH3Cl), if pKb of CH3NH2 = 4?

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Q: What is the pH of 8.1 x 10-5 M HClO4 solution?

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Q: The base protonation constant K₁ of lidocaine (C14H21 NONH) is 1.15 × 10 Calculate the pH of a 0.88…

A: Step 1: The base lidocaine (C14H21NONH) is a weak base, which is obvious from its small value of the…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 8.5 × 10⁻³. What is [H⁺]?

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Q: A chemist dissolves 706. mg of pure potassium hydroxide in enough water to make up 50. mL of…

A: Mass of potassium hydroxide = The volume of the solution  =

Q: Calculate the pH of a 0.591 M aqueous solution of benzoic acid (CH₂COOH, K₂ = 6.3x10-5). pH =

A: Here,concentration of benzoic acid = 0.591 MKa = 6.3×10-5We have to find out pH.. Herw first we need…

Q: What is the pH of a solution that has an H+ concentration of                        (a) 1.75 × 10 –5…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: The pH of an aqueous solution of formic acid (HCOOH) is 3.318. What is the initial molar…

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Q: Calculate the pH at 25 °C of a 0.24M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

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Q: Phthalic acid is a diprotic acid with ionization constants K₁1 = 1.12 x 10 and K = 3.90 x 10.…

A: Given,Molarity of potassium hydrogen phthalate ( KHP ) = 0.284 MKa1 of phthalic acid = 1.12 x…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 8.3 × 10⁻³. What is [H⁺]

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Q: Calculate the molar concentration of OH- in a water solution that has a molar concentration of H+…

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Q: do write the chemical formula for the conjugate base of selenic acid, H₂SeO04. e Write the chemical…

A: According to Bronsted and Lowry concept an Acid is a substance that has the tendency to donate a…

Q: What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH?

A: Given information: Concentration of benzoic acid = 0.40 M

Q: Calculate the pH at 25 °C of a 0.23M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

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Q: The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10¯¹⁰. Calculate the pH of a…

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Q: The value pKw is 11.05 at 78 °C. What is the pH of a neutral solution at the same temperature? Enter…

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Q: The OH⁻ concentration in an aqueous solution at 25 °C is 5.3 × 10⁻⁵. What is [H⁺]?

A: The sum of the concentration of hydroxide and hydronium ion is always 10-14. that means,…

Q: The ka of an unknown acid, HYO₂,  is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1…

A: The objective of this question is to calculate the pH of a 0.1 M solution of an unknown acid HYO2,…

Q: The base protonation constant K, of lidocaine (C4H2 NONH) is 1.15 x 10 . Calculate the pH of a 1.0 M…

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Q: Calculate the pH and the pOH of these solutions:

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Q: The base protonation constant K₁ of ammonia (NH₂) is 1.8 × 10¯5. Calculate the pH of a 0.10 M…

A: We would write base protonation reaction of ammonia and use its Kb value and expression to calculate…

Q: The base protonation constant K of ammonia (NH3) is 1.8 × 10. Calculate the pH of a 1.2 M solution…

A: The question is based on the concept of equilibrium.   we have to determine pH of the given ammonia…

Q: The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0.  What is the initial molar…

A: The relationship between pH and H+ ion concentration is: pH=-logH+ Given: pH of an aqueous solution…

Q: -6 The base protonation constant K of morpholine (C₂HONH) is 2.14 × 10 Calculate the pH of a 1.0 M…

A: Answer:Ostwald's dilution law is applicable for the weak electrolytes and as morpholine is a weak…

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

A: The quantity pH (potential of hydrogen) is the numerical representation of the basicity or acidity…

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.