39. What is the [H3O-] and [OH-] ion concentration respectively in a solution that contains 0.155 M HNO3?

Q: What is the pH of a solution that has [H3O*]= 4.5x10-³ M?

A:

Q: Calculate the [H+] or [H3O+] in a solution that has a pH of 8.75.

A: Given: pH = 8.75.

Q: + The pOH of an acidic solution is 9.47. What is [OH-]? 1 2 4 7 +/- 5 8 . M 3 6 9 0 冈 с x 100

A: The pOH of an acidic solution is 9.47. What is [OH] ?

Q: In an aqueous solution the [H3O+] is 2.0 x 10 -6 M. What is the [OH-]?

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Q: What is the pH of a solution with a hydronium concentration shown below? Round answers to 2 decimal…

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Q: The pOH of a basic solution is 3.89. What is [OH-]?

A: Since, Negative logarithm of concentration of OH- ion is known as pOH of the solution. i.e. pOH =…

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

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Q: Calculate the OH- concentration for a solution with a pH of 3.66

A: Since pH = 14 + log[OH- ]  where [OH- ] = concentration of OH-  ion

Q: concentration of OH

A:

Q: What are the hydronium and hydroxide ion concentrations in a solution whose pH is 7.95? [H*]. [OH-]-

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Q: Is HNO3 an acid, base, or neither?

A: Ans Acid Acid : Substance which donate H+ ion called acid  Base : Substance which accet H+ ion…

Q: What is the pH of a solution that has an OH- ion concentration of 3.20 M?

A:

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

A:

Q: the

A: Given data set: pH = 6.84 We need to determine the [OH-] Now, we know that: pH = -log[H+] [H+][OH-]…

Q: What is the [OH -] in a solution with a pH of 8.97?

A: Since pH = -log[H+] = 14 + log [OH -]

Q: A solution has a pH of 3.76. What is the molarity concentration of H3O+ and OH¹ in this solution? A)…

A: The objective of this question is to determine the molarity concentration of H3O+ and OH- in a…

Q: Calculate [OH-] given pH=13.58

A: The sum of the pH and pOH is 14. here, pH and pOH are the log concentrations of the protons and…

Q: What is [OH ] in a 0.0058M HI solution?

A: The dissociation of HI takes place as,                                             HI (aq) ---->…

Q: Calculate [OH-] given pH=1.92

A: Acidity of the aqueous solution is given in the term of pH. pH is given as,…

Q: Calculate the [OH-] in a solution with a pH of 6.59? * O 7.4 M O 6.6 M O 3.9 x 10^-8 M O 3.9 x 10^6…

A: pH in the calculation of H+ concentration. But we can evaluate HO- concentration also.

Q: a) A solution has an [H3O+] of 4.77 x 10-6M. What is the [OH-]? What is the pH?…

A: a. . To find  and pH.b. The value of pH is 1.499. To find  and .c. . To find  and the value of pH.

Q: 2. One mole of H* is always neutralized by mole of OH.

A: Neutralization occurs when moles of acid are equal to moles of base and reacts with each other to…

Q: Determine the [H3O+], [OH-] and pH for a 0.2 M solution of H2SO4.

A: Given, Concentration of H2SO4 solution = 0.2 M [H3O+] = ? [OH-] = ? pH = ?  Note: H2SO4 is a strong…

Q: What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of…

A:

Q: Calculate [OH-] given pH=2.82

A: Acidity of the aqueous solution is given in the term of pH. It is given as,…

Q: 6. A substance has a [H,O'] of 5.21 x 10³, determine [OH], pH and pOH and determine if the substance…

A: [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] pOH = -log[OH-] pH < 7 , acidic pH > 7 , basic pH = 7,…

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: Calculate [OH-] for each solution. pOH = 13.28     pH = 1.82     pOH =

A: The question is based on the concept of hydronium ion and hydroxide Ion concentration. We have to…

Q: What is the pH of a solution with [OH-] = 1 x 10-4 M?

A: Given information: Concentration of hydroxide ions = 1×10-4 M

Q: If the [OH-] of a solution is 1 x 10-14,  what is the ph of the solution? what is the [H3O+]?

A: Given,[OH-] = 1 x 10-14  M we know, => pOH = -log[OH-]on substituting the value => pOH =…

Q: 1.Why does the autoionization of water occur? 2.What is the definition of a strong acid? The…

A: Note - Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: A solution has a pOH of 2.00. What is the [H+] and [OH-]?

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Q: What are [H3O+], [OH−], and pOH in a solution with a pH of 10.65?

A: Given : We have to calculate the pH , pOH .

Q: Which statement is true if an aquous solution is not neutral at 25°C. ? Explain your reasoning in a…

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Q: What is the [H3O+] of a solution that has a pH of 4.6? What is the pH of a solution whose [OH-] =…

A: PH = -log H3O+PH = 4.6Calculate H3O+ concentration4.6 = -logH3O+logH3O+ =-4.6H3O+ =Antilog…

Q: What is the pH of a solution with [OH-] = 4 × 10-8 M? What is the pH of a solution with [H3O+] =…

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Q: A solution of H2S had a pH of 10.01. What was the [OH-]?

A:

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.