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

Q: Calculate the pH of a solution with [OH-]= 4.6x10-5 M

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pH of a solution with [OH-]=2.2 x 10^-7M?

A: In this question, we will determined the pH of the basic solution. So, first we need to determine…

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

A:

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

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: What is the pH of a solution with a [H+] = 0.001 M? 4 13.999 3

A: Given that, [H+]=0.001M so,

Q: 2) What is the concentration of [H3O+] in a solution with [OH-] = 1 × 10-12 M? Is the solution…

A: As you have posted multiple questions, we will solve only first one as per our guideline. Please…

Q: What is the pH of a solution with [H 3 O^ + ]=1*10^ -9 M?

A:

Q: What is the pH of a solution if the concentration of H 3 O^ + is 5.6 * 10 ^ - 5 M?

A: Given data contains, Concentration of H3O+ is 5.6×10-5.

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

A:

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

A:

Q: Determine the pH of a solution with [OH-] = 1.50 x 10-5 M

A: Given [OH-] = 1.50 x 10-5 M

Q: What is the pH of a 0.0355M KOH solution?

A: pH can be defined as negative logarithm of concentration of [H+] ions as the KOH is a base first we…

Q: Which of the following is the most basic solution (highest [OH ])? O pOH = 1.0 O pH = 12 O [OH¯] =…

A:

Q: What is the pH of a solution at 25 C if the [OH-] = 5.0 x 10-3 M?

A: pH measures the acidity of a solution. If pH is greater than 7 then solution is basic. If pH is less…

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: 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: Determine the [H+][H+] , [OH−][OH−] , and pH of a solution with a pOH of 10.8710.87 at 25 °C.

A: Given data is as follows: The pOH of the solution = 10.87 The pH of a solution can be calculated as…

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: 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: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

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 would be the pH of 0.00551 M H2SO4 solution?

A:

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

A:

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

A:

Q: What is the pH of a 0.0075 M KOH solution?

A: The pH of a solution measures the acidity of a solution. If the pH of the solution is more than 7,…

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 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–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

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

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

Q: What is the pH of an aqueous solution with an OH- concentration of 0.00250 M?

A: Solution:- Given concentration of OH- = 0.00250 M  [OH-] = 0.00250 M  As we know, p(OH) = -…

Q: If the [OH-] is 3.5 x 10 then what is the pH of the solution?

A: Given, [OH-] = 3.5 x 10-5  PH = ?

Q: What is the pH of a solution with [OH-] = 1.00 x 10^-5 M?

A:

Q: What is the pH of a solution with hydroxide concentration, [OH--] = 4.83×10-5 M?

A: According to the question,  We need to calculate the pH of a solution with hydroxide concentration,…

Q: What is the pH of a solution with [H+] = 3.51x10-5 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 the pH of a solution if [OH-]=2.4 x 10-6?

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

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

A:

Q: Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.

A: Hydrazine is a weak base.We have to calculate pH given hydrazine solution. Recall the following…

Q: What is the pH of a solution in which [OH⁻] = 0.000005 M?

A: The concentration of OH- = 0.000005 M OH-=0.000005 M=5×10-6 M

Q: What's the pH of a solution with an H+ concentration of: 1.247 x 101º. Round to 2 decimal places.

A: pH measures how the solution is basic or acidic lower the pH value the solution will be more acidic…

Q: What is the concentration of hydronium ion H3O+ in a solution with a pH -1.3?

A: pH of any solution is given by  pH = -log[H3O+ ]  where [H3O+ ] = concentration of hydronium ion

Q: calculate the pH of a solution that has H3O =3.9x10^-8 M

A:

Q: What is the pH of a 0.0235 M H* solution?

A: pH :-  It is defined as , the negative logarithm to the base 10 of hydrogen ion concentration…

Q: What is the pH an pOH of a solution of a strong acid of a concentration of 0.005 M?

A: Here given that,  Concentration of strong acid = 0.005 M And acid is strong so it's dissociated…

Q: If the pH of a solution is 6, then O [OH--] = 1 x 10 8 M O [H+] = 6 M O [H+] = 1x 106M O pOH = 1

A: Given that pH of a solution is 6.We know pH = - log [H+].Thus we can get the [H+] as 10^…

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.