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: 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: w: In pure water at 25°C, [H30+]=1x10¬7. What is the pH of pur water at 25°C?

A: Given that: [H3O+] = 1×10-7 pH of pure water = ?

Q: Which of the following is the weakest acid? OH A OH OMe B OH NO₂ C OH D OMe

A: The objective is to determine the weakest acoid.

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

A:

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: What is the pH of a solution with an H+ concentration of 3 x 10-6 Molar

A: pH is equal to the negative logarithmic of hydrogen ion concentration             given.        H+…

Q: The hydronium ion concentration in a bottle of household muriatic acid is 0.0082 M. What is the pH,…

A: Given: [H+]=0.0082M Formula used:-  pH = -log[H+] poH = -log[OH- ]

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: What is the pH of lemon juice with a [H+] of 2.0x10-3?

A:

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: The auto-ionization of water is shown in the reaction below. Given that this reaction is…

A: Given, the auto-ionization reaction of water: H2O ⇌ H+ + OH- Given, ∆H = +55.89 kJ/mol We have to…

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: What is the pH of 0.180M NH4Cl. Ka NH4+: 5.80x10^-10

A:

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.310 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

A: pH of buffer solution is calculated by using Henderson Hesselbalch equation

Q: What is pH of H2SO4 solution of 10 mg/L?

A: pH :-        It is a scale to measure the acidic or basic property of any substance . That tells…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.100 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

A: Concentration of CH3NH2 = 0.400 M Concentration of CH3NH3I =  0.100 M Kb for CH3NH2 = 4.4 × 10-4  pH…

Q: What is the pH of a solution with a concentration of hydronium ions of 5.11×10 with a little arrow…

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Q: ▼ Determine the [OH] of a 0.10 M ammonia solution. Express your answer using two significant…

A: we have to calculate [OH-] pH pOH for the ammonia solution

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: 1) Which of the following compounds are amphoteric? -both HSO3^- and O^2- -HF -CO3^2- -O2 -BF3…

A: A solution is said to be acid if the solution contains amount of H+ higher than amount of OH- , then…

Q: What is the pH of a solution that has [OH–] = 6.92x10-11 M.

A:

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.240 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

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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: A solution has a pH = 9.55. What is the concentration of H3O+ in the solution, in mol L-1

A: Here we are required to find the concentration of H3O+.

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

A:

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

A:

Q: Which would have a higher pH, a solution whose pOH is 5.00 or a solution whose hydrogen ion…

A: pH of solution is calculated based on the hydrogen ion concentration. pH = -log[H+] pH = 14 - pOH

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 [H+] of a solution whose pOH = 2.11 ?

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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: Calculate the pH of a solution that has a concentration of OH- equal to 5.92 x 10^ (- 9) M.  (Write…

A: The objective of this question is to calculate the pH of a solution given the concentration of…

Q: At 25 °C, a solution has a

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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…

Q: The Kb for NH2OH = 6.6 × 10-9. What is the pH of a 0.50 M solution of NH2OH?

A: Given Kb for NH2OH = 6.6 × 10-9  Concentration = 0.50 M

Q: Rank the solutions in order of decreasing H3O|.

A: Acids donate [H+] ions and increase H+ ions concentration in the solution  Strong acids…

Q: Q1-SOLVE mathematically, then choose the correct answers: 1- Calculate the pH of solution made by…

A: Answer - The correct option is (a)  = 3 According to the question - Given values - Ka = 1.8 x 10^-5…

Q: What is the pH of a 8.1 × 10-6 M KOH solution?

A: The pH scale is introduced by the scientist Sorensen in order to express the [H3O+] ion of a…

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: identify each substance Acid Base conjugate acid Conjugate base

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Q: A solution has a hydronium concentration of 7.50 x 10-5. What is the hydroxide concentration in M?

A: Given = Hydronium ion concentration (H30 +) =7.50*10-5 Hydroxide ion concentration (OH-) =?

Q: pH of a solution having OH-  concentration 10-5

A: We know that, pOH = -log[OH-]                { [OH-] is the molar concentration of OH- ion} Again,…

Q: The pOH of pure water at 40 C is 6.8. What is the hydronium concentration, [H30+], in pure water at…

A: Given: pOH=6.8;[H3​O+]=???MThere are two ways to get the concentration of H3O+ This is the first…

Q: What is the relationship between H+ and OH- concentrations in a solution that has a pH of 11?

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Q: The pH of an acidic solution is 4.77. What is [OH-]?

A: Given :- pH of solution = 4.77  To calculate :- concentration of OH- i.e. [OH-]

Q: Which has highest pH at 25c-    NaClO4, NaCLO,NaNO3

A: The pH of a salt solution depends on the strength of the acid and the base by which the salt is…

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.