Calculate the hydroxide ion concentration, [OH"], for a solution with a pH of 11.35.

Q: What is the pH of a 0.087 M solution of HCl?

A: Given  [H+]     = 0.087 M  PH       =  ?

Q: Calculate the pH of a solution that has [ OH-] = 5.2 x 10-7 M pH=  _?_

A: Given, Concentration of OH-, [OH-] = 5.2*10-7M. The pOH of the solution can be calculated as…

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: What is the pH of a 0.00535 M solution of NaOH?

A: Number of moles of solute present in one litre of Solution is called Molality (M)  Units: mol/L  pH…

Q: water has a hydroxide ion concentration of 2.0 x 10-6 M. What is the pH of seawater?

A:

Q: Calculate the pH corresponding to each of the hydroxide ion concentrations given below, and indicate…

A: pH of any solution in terms of hydroxide ion concentration is given by  pH = 14 + log[OH- ]  where…

Q: Determine the [H*],[OH-], and pOH of a solution with a pH of 13.34 at 25 °C. H*] 4.571 x10-14 OH] =…

A:

Q: What is the pH of a 0.0 solution of HBr?

A:

Q: Calculate the pH of a 1.33x10-9 M solution of LiOH.

A: The reaction will be as shown below. LiOH ----> Li+ + OH-  Assuming complete reaction, we can say…

Q: pH, [OH-], and pOH

A:

Q: A neutral solution is at a temperature of 100 degrees C. Its pH is determined to be 6.15. Calculate…

A: Given :- pH of solution at 100°C = 6.15  To determine :- hydrogen ion concentration i.e. [H+]

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 6.02.

A:

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: Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution

A: Construct ICE table and calculate the required values,

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: Calculate the hydroxide ion concentration, [OH], for a solution with a pH of 5.1I3.

A: Given, pH of solution =5.13we are asked to calculate the concentration of [OH-]

Q: Calculate the hydroxide ion concentration, [OH–], for a solution with a pH of 5.68.

A: The concentration of hydroxide ion from the given pH is determined as,

Q: What is the hydroxide ion, pH, and pOH of a solution with a hydrogen ion concentration of 3.25 x…

A: Given:  [H+] = 3.25 x 10-3 M  Kw = 10-14    Since [H+] < 10-7 M so solution is acidic in nature.…

Q: pH

A:

Q: What is the pH of a 0.00350 M solution of NaOH?

A: To determine the pH of a 0.00350 M solution of NaOH

Q: What is the pH of a solution ten times as acidic as one of pH 5?

A:

Q: What is the theoretical pH of a 0.00001 M HBr solution?

A:

Q: Show the calculation required to determine the pH of a solution that has H3O+ concentration of…

A: pH of solution is defined as negative logarithm of hydrogen ions.

Q: CALCULATE THE [H30+] CONCENTRATION OF A SOLUTION WITH A PH OF 5.5

A: Given pH = 5.5

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: calculate the Ph of a 0.050M HCl solution

A:

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 8.89. OH- =

A: The acid solution increases the concentration of hydrogen ions (H+) in the solution. Similarly, the…

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 10.32   [OH^-]= ? M

A: PH is defined as negative logarithm of concentration of [H+] ions.  PH + POH = 14  Given , PH =…

Q: What is the [H3O+] concentration of a solution that has pH + 11.61, 7.156, 0.015

A:

Q: Calculate the concentration of H3O+ and OH- in a sample of pH 3.30 solution?

A: As we know  pH = -log [H+] and pOH = -log[OH-]  and also pH+ pOH = 14

Q: Determine the [OH-] in a solution with a pH of 4.358.  Your answer should contain 3 significant…

A: The relationship between the pH and [OH-] is given by  pH = 14 + log[OH-]  where [OH-] =…

Q: What is the pH of a 0.00585 M solution of NaOH?

A: We know that ., PH = 14 - POH POH = - log [OH-]

Q: Calculate the [OH-] using the equation that relates hydroxide to hydronium ion concentration with…

A: Here, Given          Kw=H3O+OH-                               ......................(1) Kw is the…

Q: For each of the following strong base solutions, determine [OH−] and [H3O+] and pH and pOH. 1.…

A: 1.Given, 1.15*10-2M Ba(OH)2

Q: What are the H3O+ and OH- concentrations of solutions that have the following pH values? pH4, pH 11

A: Ionic product of water, Kw:                                        Kw=[H3O+][OH-] = 10-14…

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

A:

Q: Calculate the hydronium and hydroxide ion concentrations in solutions with the following pH: a. pH…

A:

Q: What is the concentration of hydroxide ion in a solution with a pH of 3.767?

A: pH of a solution is determined from the concentration of H+ ion in solution.  Now, pH = -log[H+]…

Q: Calculate the pH of a solution that has [OH-] = 1.0 * 10 -6 M

A:

Q: Show complete calculations Calculate the pOH, H3O+, OH- if the pH is: 1. pH = 8 2. pH = 7.4

A:

Q: Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

A:

Q: Calculate the hydroxide ion concentration of a solution with pH = 6,4.

A: pH of solution is 6.4 We need to determine [OH-]

Q: Calculate the pH of a 0.74 M solution of NaOH.

A:

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 1.10 × 10-º M. pH

A:

Q: determine the [H+], [OH-] , and pOH of a solution with a pH of 2.63 at 25 degrees Celsius.

A:

Q: Calculate the hydrogen-ion concentration and pH of 0.0350 M KOH.

A: KOH completely dissociate into  KOH ------>K +  + OH- At 25o C  Ionic product (K w )   of  water…

Q: Calculate the hydroxide ion concentration of a solution with a pH of 12.65.

A: Given :- pH of solution = 12.65  To calculate :- hydroxide ion concentration i.e. [OH-]

Q: Calculate the pH of a solution that has [H3O+] = 3.9 × 10−8 M.

A: We are given  [H3O+]  = [H+] = 3.9 × 10−8 M we are to calculate the pH.

Q: Calculate the pH of a 0.00118 M solution of HBr.

A: Given data contains, Concentration of HBr is 0.00118 M. Hydrobromic acid is a strong acid so it gets…

Q: [H*] = 7.23×104M 9.41 pH 4.59 РОН Choose one: acidic basic neutral

A: Given : [H+ ] = 7.23 X 10-4 M

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.