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

Q: What is the pH of a solution that has [OH-] = 6.0 × 10−12 M?

A: pH: pH is  justified  as power of hydrogen. pH=-log[H+] Or in general we can say that it helps us to…

Q: find the pH and [OH-] if [H3O] = 7.8 x 10^-8

A:

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

A: Given  PH = 5.50  [OH- ]  = ?

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

A:

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: What is the pH of a solution that has a concentration of 2.0x10-5 M to 2 decimal places?

A: The PH of a solution can be calculated as follows

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

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

Q: What is the pH of a solution with a hydronium (H3O+) concentration of 10-4 M? Is the solution…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: If the pH of a solution is 1.78, what is the concentration of [H+]?

A: pH = -log [H+]

Q: Calculate the pH of an aqueous solution; 0.015 M KOH

A: Given: Concentration of KOH = [OH-] =  0.015 M

Q: If in a solution [H,01-10 [OH ], what is the pH of the solution?

A: Given that :  [H3O+] = 10 [OH-]  We need to determine pH of this solution.

Q: em101 The pH of a 0.0049 M solution of Ca(OH), is

A: Given that: molarity of Ca(OH)2 = 0.0049 M To find: pH of 0.0049 M Ca(OH)2 solution?

Q: What is the pH of a solution with [H3O+]=1x10-9M?

A:

Q: What is the pH of an aqueous solution if the [H+] = 0.1M?

A: Given Data :  [H+] = 0.1M  To calculate : pH.  Formula : - log [H+]

Q: What is the pH of a 0.00235 M solution of HCl?

A: Given that : pH of HCl = 0.00235 M HCl is a strong acid, so it will dissociate completely.  HCl  →…

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

A:

Q: calculate the {H3O} of the solution of hydrochloric acid with pH = 2.00

A: Given, PH = 2.00 PH is defined as negative logarithm of concentration of [H+] ions.

Q: Consider a solution with a concentration of H3O+ of 10-3 M. What is the concentration of OH- in…

A: concentration of solution is defined as moles of solute dissolved in per l volume of solution

Q: The pH of an acidic solution is 5.05. What is [OH^-]

A:

Q: In an aqueous solution the  [OH-] is 1.0 x 10- 6 M. What is the [H+]

A: At 25oC, the mathematical relation between molarities of H+ and OH- is given as: [H+][OH-]=1.0×10-14…

Q: calculate ph of 7*10^-3 M aqueous solution of Ca(OH)2 at 25 degrees

A:

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

A:

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

A:

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the [H3O+].

A: Given: The concentration of hydroxide ions is provided,i.e. [OH-] = 1.0 x 10-5 M. The hydronium ion…

Q: Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.

A:

Q: an aqueous solution has an OH- concentration of 5.753 x 10^-3 M. calculate the pH of this solution.

A:

Q: The pH of a solution is 6.88. Find the H + and OH- concentrations and pOH

A: pH is a scale used to determine the H+ ion concentration of a solution. pH is numerically negative…

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pH of the solution. Calculate the…

A: Applying formula [H+][OH-] = 1×10-14 And PH = -log[H3O+]

Q: Calculate the pH of an aqueous solution where the [OH-] is 6.9 × 10^-9 M.

A:

Q: What is the pH of a 0.200 M solution of HCOOH? Ka of HCOOH = 1.8 × 10−4

A: We know that, pH is defined as the negative logarithm of hydronium ion, i.e.…

Q: What is the pH of a solution with molar concentration of Ht, [H*] = 1.0 x 10-9 M?

A:

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

A:

Q: What is the pH of a solution that has an [OH-] of a 7.3 x 10^-9 M?

A: Given, Concentration of the OH- ion = [OH-] = 7.3 x 10-9 M pH of the solution = ? The formula used…

Q: What is pH of a solutionwith a H+ concentration of 10^-4M

A:

Q: What is the [H3O+] in a solution that has a pH of 9.1?

A:

Q: Given the following values of [H3O+], calculate a) [OH-] and b) pH for each solution. 1 x…

A: We have given that [H3O+]  1) 1 x 10-11 M  2) 1.5 x10-3M and we know that  [H3O+] = [H+]

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: What is the [OH-] concentration of a solution with a pH of 3?

A:

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

A:

Q: A solution with (OH- )of 5 x 10^3 has a pH of? A.-2.3.   B. 11.7.   C 7.0. D. 2.3

A: (b) 11.7 Concentration of OH- ions = 5×10-3 Now, pOH = -log[OH-]                    = -log (5×10-3)…

Q: Calculate the pH of each solution. H3O+][H3O+] = 6.0×10−7 M

A: pH  calculation using concentration of H+ :

Q: What is the pH of a solution if the concentration of H+ is 5.3x 10^-9

A: pH of solution = ? H+ = 5.3 × 10-9  We know that, pH = - log [H+]

Q: pH of a 10 M KOH solution is: O-10 O 10 O-4 4

A: Given , [OH-] = 10-4 M  PH = ? PH is defined as negative logarithm of concentration of H+ ions.

Q: calculate the ph of [OH-]=8.7x10-6M

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

Q: If the pH of a solution is 9.7, calculate [H*]. O 70794.578438414 O 5011872336.272714615 O…

A: pH = - Log[H+] [H+]= -antilog[pH] [H+]= antilog[-9.7] [H+] = 1.99 * 10-10

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 1.87x10^-3 M solution of OH^-?

A: Given: Concentration of OH- ions, [OH- ] = 1.87 × 10-3 M

Q: In a solution, [H+ ] = 3.25 x 10-10 M. What is its pH and is it considered an acid or a base?

A: A solution can be classified as acidic or basic or neutral depending on the pH value. For a solution…

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.