Find the [OH-] and pH of a 0.100 M NH3 solution.

Q: What is the [H3O+] of a solution if [OH−] is 5.0 × 10−8 M?

A:

Q: 1. Recall that pH is shorthand for -log[H*] (a) If [H*] is 1 M, then log[H*] is so pH = (b) If [H*]…

A:

Q: Determine the [OH-] concentration in a 0.235 M NaOH solution.

A:

Q: Which of the following statements is true about the pH value of a solution? Oa If the pH is exactly…

A: A solution can be divided into 3 types based on the pH of the solution as acidic, basic, and…

Q: If a solution has pH of 5.50, calculate its [OH-]*

A: Given  PH = 5.50  [OH- ]  = ?

Q: Calculate the ph of the [OH-] = 2x10^-3 M.

A: We have to calculate the pH of given solution.

Q: Calculate the pH of a solution with a [H 30*]=5.6x10 -9 M.

A: Formula to calculate pH :- pH = -log[H3O+]

Q: Find the pH of a 0.010 M HNO2 solution.

A: HNO2 is a weak acid with dissociation constant, Ka = 7.2 X 10-4  Hence HNO2 will dissociate…

Q: Determine the [H+], [OH-], and pH of a solution with a pOH of 12.67 at 25 °C. [H*] : [OH] = pH =

A:

Q: Determine the [OH-] concentration in a .235 M NaOH solution.

A: The Concentration of OH- will depend on the base from which it is dissociated and the concentration…

Q: What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-5 M?

A: Given information is as follows: The concentration of H3O+ = 1.0×10-5 M The concentration of OH- = ?…

Q: What is the pH of a strong acid (HA) of concentration 0.0135 M?   What is the pH of a strong base…

A:

Q: Calculate the [H3O+] ,[OH-], pH & pOH of a 0.10 M HCl.

A: pH = -log [H3O+]  [H3O+].[OH-] = kw  pOH = -log [OH-]

Q: Calculate [OH-] for each of the following solutions, andindicate whether the solution is acidic,…

A:

Q: What is the pH of a 0.325M solution of NH4Cl?

A:

Q: Fill in the missing terms (strong or weak) and formulas in the following table.

A: The relationship between base strength (or) acid strength and the strength of conjugate acid (or)…

Q: What is the pH of a 0.02M solution of HCl? What would the H+ concentration be? What would the OH-…

A: HCl is a strong acid  and it completely dissociates into H+ and Cl- ions. The pH of a solution is…

Q: Find the [OH-] and pH of a 0.33 M methylamine solution.

A: Methyl amine is basic in nature. When dissolved in water, it takes up the hydrogen ion from water as…

Q: What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-8 M?

A:

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 8.52.         [OH−]= M

A: Given pH = 8.52  pH = - log [H+] 8.52 = - log [H+] log [H+] = - 8.52 = -9 + 0.48 log [H+] = log (…

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 13.23 at 25 °C. [H*] =

A:

Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

A:

Q: Find the [OH-] and pH of a 0.010 M Ba(OH)2 solution.

A: Given, 0.010 M Ba(OH)2

Q: What is the [H+], [OH-], pH and pOH of a 2.7x10-4 M HNO3 solution? Is this solution acidic, basic,…

A: Given : Concentration of HNO3 = 2.7 x 10-4 M

Q: Determine the H"|, |, and pH of a solution with a pOH of 8.50 at 25 °C. [H*] = M [OH-] = M pH =

A: pH is expressed mathematically as - pH = -log H+pOH = -log OH- Where, [H+] and [OH-] are the molar…

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 1.90 at 25 °C. [H*] : M [OH"] = M pOH…

A: Given, PH = 1.90  PH us defined as negative logarithm of concentration of H+ ion.

Q: Find the pH of a 0.0025 M HCl solution.

A: Here we are required to find the pH of 0.0025M of HCl solution

Q: Given 1.5 M of NaOH, calculate the following: pH = POH = [H*] = M [OH] = M

A: NaOH is a strong base. So, pOH of NaOH can be expressed as -log [OH-] (where [OH-] = concentration…

Q: What is the [OH-] in a solution that has a [ H3O+] = 2.0 × 10-4 M? Is this solution acidic, basic,…

A:

Q: At 25 degrees C, a solution has a pH of 10.69. What is the [OH-] in the solution?

A: Given : pH = 10.69

Q: Calculate the hydroxide ion concentration, [OH^−], for a solution with a pH of 8.55…

A: Using the given pH value first the hydronium ion concentration is calculated first.

Q: Find the [OH-] of the solution, if the [H3O+] is: 2 ´ 10-11 M

A: Given that,  Concentration of [H3O+]   = 2×10-11 M

Q: What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M?

A:

Q: Please answer fast.

A:

Q: A solution has a pOH = 9.18. Calculate the following: [OH] = M pH = [H,O*] = M

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the [OH-]  in a solution with a pH of 2.50?

A:

Q: Based on the auto-ionization of water, draw a graph showing the relationship of [OH-] and [H+].…

A: Auto ionisation of water means that water self ionises to give H+ and OH- ion.

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 pH and concentration of OH- of 0.0200 M NH3?

A: Given:Concentration of NH3= 0.02MThe objective is to determine the pH and the concentration of OH-.

Q: What is the pH of a 6.20 x 10-3 M NaOH solution?  (This solution is basic, concentration is of OH-)

A:

Q: The pH of a solution is 5.330. The [OH-] is [concentration]

A: Given information,        pH of the solution = 5.330

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

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

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

A:

Q: 2. Calculate the pH of each of the following solutions: А. 0.0010 М НCІ В. О.76 М КОН C. A solution…

A: Following are the pH of the given solutions.

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 7.53 at 25 °C. [H*] = M [OH"] = M pOH…

A: Multiple  questions PH = -log [H+] PH + POH = 14 GIVEN PH=7.53 at 25 °C

Q: Calculate [OH-] and pH for eachof the following solutions: (a) 0.10 M NaBrO, (b) 0.080 M NaHS,(c) a…

A:

Q: If the hydroxide concentration is 5.77E-7 M, then what is the pH of this solution? (pH = -log[H 1)

A: The pH of a solution is the measure of the acidic strength of the solution. The lower the value of…

Q: Calculate the [OH-] of a solution with 10.0 M H3O+ and classify as acidic, basic, or neutral.

A: Given : Concentration of H3O+ in the solution = 10.0 M

Q: The pH of 0.10M HNO3 is When a solution has pOH = 5.30, the [OH-] is

A: pH = -log[H+]  pOH = -log[OH-]

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.