CHEM1407 Homework Ch 16, Sec 6A Name: #3) A 2.5x10-³M of an unknown acid has a pH of 3.80 at 25C. What is the hydronium ion concentration of the solution?

Q: If a solution has a pH of 5, what is the [OH-] of that solution?

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Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.15×10-3 M  solution…

A: [H+] [OH-]  =  10-14 PH + POH  = 14 [OH-]  = 10-14/ [H+] [H+]  =  10-14               [ OH-]

Q: Why is the ph of NH4C2H3O2 nearly 7

A: The question is based on the concept of salt hydrolysis . we need to calculate pH of ammonium…

Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

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Q: A certain weak base has a K₁ of 7.70 × 10-7. What concentration of this base will produce a pH of…

A: The objective of this question is to find the concentration of a weak base that will produce a…

Q: A sample of grape juice has a pH of 3.92. What is the hydroxide-ion concentration of this solution?…

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Q: What is the pH of an aqueous solution of KOH with a concentration of 0.035M? Respond with the…

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Q: The difference between each pH unit is a factor of 10. If the pH of a grapefruit is 3 and the pH of…

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Q: a solution has a concentration of OH- =4.0x10-5 M. what are the concentration of H3O+ and the pH of…

A: pH of a solution can be defined as negative of logarithm of concentration of hydronium ions

Q: Determine the pH of a 0.62 M NH4NO3 solution at 25°C.  The Kb for NH3 is 1.8 × 10-5. Express your…

A: NH4NO3 is a salt of strong acid and weak base.  Given Kb of ammonia is 1.8×10-5 and concentration of…

Q: What is the pH for a solution with [OH-] = 8.9 x 10-⁹ M?

A: We have to calculate the pH of solution

Q: Oven cleaner has a pH between 13 and 14. What two whole-number values of x should be used in…

A: pH = -log[H+]  so, [H+] = 10-pH

Q: Calculate the pH of 9.3×10−2  M propionic acid (C2H5COOH). Ka= 1.3x10-5

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Q: A certain weak base has a Kb of 8.40 × 10-7. What concentration of this base will produce a pH of…

A: A weak base accepts proton from H2O in aqueous medium to form conjugate acid and generates OH-…

Q: Calculate the pH, pOH, and [H+1] of a solution in which the [OH- ]=2.34x10-5

A: Given [OH-] = 2.34*10-5

Q: To a precision of 2 significant figures, what is the pH of a solution containing a concentration of…

A: Given, Concentration of KOH solution = 1.0x10-14 M pH of the solution = ? Note: KOH is a strong base…

Q: A solution has a pH = 13.42. What is the concentration of H3O+ in the solution, in mol L-1?

A: Hydronium ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The concentration [H*] of a substance is 3.7×10 10. Calculate the pH value of the substance and…

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Q: A concentrated acid is fully neutralized with a dilute base. What is the most logical expectation…

A: Given that, a concentrated acid is fully neutralized with a dilute base. Now, when a solution is…

Q: Morphine C17H19NO3 is a weak base and a powerful painkiller. A solution of morphine has a…

A: Given,  Concentration of morphine (C17H19NO3) say B = 0.011 mole/L  Base dissociation constant of…

Q: What is the hydrogen ion concentration of a solution with pH 9.75? -10 [H*] = 8.37 x10

A: Given pH = 9.75

Q: What is the pH of a solution with a hydroxide ion (OH-) concentration of 10-10M?

A: pH is related to pOH by the following expression: pH + pOH = 14  ⋯⋯⋯⋯(1) Also pOH is related to the…

Q: Provide the correct IUPAC name for the compound shown here. Question 16 of 20 OH CH₂-CH-CH₂-CH₂-CH₂…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: A solution has a pH = 2.56. What is the concentration of H3O+ in the solution, in mol L-1?

A: The concentration of the hydronium ion in a solution is calculated in terms of pH.

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: What is the pH of a 2.5 M solution of HC1O4? pH

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Q: What is the hydroxide ion concentration of a solution with pOH =1.5?

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Q: What is the pH of a solution that has a hydroxide ion (OH-) concentration of 1.51 x 10-4 M?

A: The first step is to calculate the pOH of the solution. The pOH is the negative logarithm (base 10)…

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.15×10-3 M  solution…

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Q: What is the pH if a solution has a H3O+ concentration of 1.0 ´ 10–10 M?

A: pH: It can be defined as the potential of hydrogen in any solution. Depending upon this factor we…

Q: A certain weak base has a K₁ of 7.90 × 10-7. What concentration of this base will produce a pH of…

A: The objective of this question is to find the concentration of a weak base that will produce a…

Q: What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOO-K?

A: Weak acid is the one which undergoes partial dissociation. Formic acid (HCOOH) is a weak acid. The…

Q: Tartaric acid (H₂C4H4O6) is found in many fruits, including grapes, and is partially responsible for…

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Q: A certain weak base has a ?b of 7.70×10^−7. What concentration of this base will produce a pH of…

A: As per the given information certain weak base has a kb is 7.70 × 10-7.pH=10.0The chemical balanced…

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.10×10-3 M  solution…

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Q: What is the concentration of [OH] if the solution with a pH=6.9?

A: Given : pH = 6.9

Q: What is the concentration of a solution of Ca(OH)2 for which the pH is 11.68?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

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.