2. Find the pH if the [OH-] is equal to 1.0 x 10-6 M.

Q: Calculate the pH of these solutions: a) H2SO4 with a [H3O+] = 2.5 x 10 -5 M b) KOH with a [OH-] =…

A: The question is based on the concept of concentration. We have to calculate pH of the solutions…

Q: A solution for which [H +] = 1.0 ´ 10 -3 will have a pH of

A: Using the formula of pH = -log10[H+] we can find pH.

Q: Calculate the pH of a solution if the concentration of H+ is 5.8 x10^(-6) M

A: pH = - log (H+) (H+)  = 5.8 × 10-6 M Substituting the concentration of hydrogen ion in above…

Q: Determine the pH for [OH-]=2.9x10^-4 M

A:

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

A: Given: pH = 8.75.

Q: Determine pH if [H^ + ]=9.18e-11M

A: [H+] = 9.18 × 10-11 M  By the definition of pH, we know that ; pH = - log [H+]  pH = - log (9.18 ×…

Q: Calculate the pH of a 2.4 x 10-5 M solution of LiOH.

A: Lithium hydroxide (LiOH) will dissociate to form hydroxide ions in a 1:1 ratio as per the equation…

Q: Find the [OH-] in an acidic solution where [H+] = (6.0x10^-5)

A: An acid is a molecules which can donates protons or they are capable of donating hydrogens. Bases…

Q: The pH of an aqueous solution that contains 3.4 x 10-2 M NaOH is What is the pOH? Circle one: ACID…

A: Answer :- 1) i) pOH = 1.47  ii) the given aqueous solution is a Base.…

Q: Calculate the pH from the H+ concentration. 5.2 x 10-12 M

A:

Q: Calculate the concentration of H30" in a solution of H,S04 that has a pH of 3.5.

A: Given: pH=3.5 To Find: [H3O+] =?

Q: Calculate the pH of a solution that has a pOH of 8.70.

A: Given,  pOH of the solution = 8.70  Calculate the pH of the solution = ?  Use the formula :  pH +…

Q: Calculate the pH of 0.050 M of H+

A: We know that, pH can be expressed as the negative logarithm of hydrogen ion concentration. i.e.…

Q: Determine if this solution is acidic or basic and find the pH, [OH], and the [H] if the pOH = 9.38

A:

Q: Calculate the pH of 0.02 M H;PO4

A:

Q: Find the pH of a 0.2 M solution of H2SO3

A: Given,  The pH of a 0.2 M solution of H2SO3 is:

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H, O0*], of 5.24 × 10-³ M.

A: pH is defined as the negative logarithm of the activity of hydronium ion. But in dilute solutions,…

Q: Calculate the pH of a solution that has [OH-] = 5.9 x 10 -5 M

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

Q: Find the pH if the concentration of OH- is 0.52 M?

A: [OH-] = 0.52 M

Q: Calculate [H'] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: The concentration of hydrogen ions in an aqueous solution is measured in pH scale. Mathematically,…

Q: 3. Calculate the value of [H3O*] from the given [OH ]in each solution and label the solution acidic…

A: pH  of any solution is expressed as the negative logarithm of hydrogen ion or hydronium ion…

Q: What is the pH of 0.005 M NaH2PO4

A: NaH2PO4 is a weak acid. Hence, pH = 1/2 pKa -1/2 logC formula can be used to determine pH of…

Q: Find the pH of 0.99 M solution of LIOH.

A: pH is power of hydrogen or potential of hydrogen. pH scale is used to determine the nature of a…

Q: Calculate the pH of a solution when its [OH-] = 8.2 x 10-3 M.

A: Given a solution in which the concentration of [OH-] =8.2×10-3 Mwe are asked to calculate the pH of…

Q: Calculate the pH if the [OH-] = 2.16 × 10-12

A:

Q: 1. Calculate [H] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: given a) pH = 4 b) pH = 8.52 c) pH = 12.60

Q: Calculate the pOH of a solution  with [OH-]  = 4.5x 10 -14 M

A:

Q: Calculate pH of [H+] concentrations of 5.42x10-6 M and 9.98x10-12 M.

A:

Q: 2. If the [H'] in a certain tap-water sample is 2.6x107 M, what is the OH° concentration? Determine…

A: Answer 2 :  Given : [H+] = 2.6 × 10-7 M             [OH-] = ?             pH = ?

Q: Calculate the pOH of a solution with [OH-] = 6.8 x 10-9 M

A: Given  ; [OH-] = 6.8 × 10-9 M  To calculate the pOH of the solution.

Q: Determine the pH of a 0.500 M HA solution if the Ka of H

A: Welcome to bartleby !  Introduction :  We have to calculate pH .

Q: Calculate the concentration of an aqueous solution ofNaOH that has a pH of 11.50.

A: Given: pH of NaOH solution is 11.50

Q: Find the pH if the concentration of H+ is 0.487 M?

A:

Q: Calculate the pH of a solution if the concentration of OH- is 6.79 x10^(-8) M

A: Given, [ OH-] = 6.79 *10-8M

Q: What is the [H*] and pH of a sample with [OH] = 1 x 105?

A: Given,  [OH-] = 1 × 10-5 We know that  [H+][OH-] = 10-14

Q: find [OH-] and [H3O+] if the pH= 2.75

A:

Q: Find the pH of 0.10 M ammonia.

A: pH: pH of any solution is defined as it is the power of hydrogen atoms into the solution. Here , we…

Q: Calculate the pH of a 0.0500 M  solution of NaOH. Calculate the pOH of a 0.0500 M  solution of NaOH.

A:

Q: Calculate [H3O+] for a solution with a pH of 8.37.

A: The given data contains, pH =8.37

Q: Determine [OH-] in a solution where [HBr] = 0.0607 M.     [OH-] = ___ × 10 ___M

A: The concentration of HBr is 0.0607 M.

Q: 1. What is the pH of a solution in which the [OH-] is 1.5 x 10-52

A: Given:                            [ OH- ] = 1.5 ×10-5 Asked for:                            pH =…

Q: Calculate the pH of a solution that is 0.0400 M in "(a) H,PO4. (Ь) Н.С.О. "(c) H,PO3.

A:

Q: What is the pH of NaOH that has a concentration of 0.013 M?

A: NaOH is a strong base and dissociates completely as Na+ and OH- in solution. As it dissociates…

Q: Find the pH of a solution with [H*] = 1 x 10-4 M. Is this solution acidic or basic? %3D

A: Given :-  [H+] = 1 × 10-4 M  To determine :- pH and nature of solution i.e. acidic or basic

Q: Determine the [H30+] for a solution that has a pH of 7.45.

A: The concentration value for the species hydrogen ion can be investigated with the solution pH value.

Q: Calculate the pH of a solution that has a 0.0025 M [H3O] +

A: PH= -log[ H3O +] NEGATIVE LOHARITHAM OF HYDRONIUM ION CONCENTRATION

Q: Given [OH-]=5.2x10-6 M, Calculate its pH.

A:

Q: Determine the pH of a solution that is 0.00542 M HCl and 0.0513 M HClO2. The Ka of HClO2 is 1.1 ×…

A:

Q: Calculate the pH of a solution with [H+]= 1×10−4 M .

A: The pH of a solution is calculated by using the hydrogen ion concentration by using the following…

Q: Determine the H*]. [OH , and pH of a solution with a pOH of 2.65 at 25 °C. (H = M %3D M pH =

A: Given data is as follows: The pOH of the solution = 2.65 As we know that; pH+pOH=14        At 25 °C…

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.