what is the Ph of [H3O+] = 2.5x10-5

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: 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: If [H3O+] = 2.7x10^-5m  Find [OH-], pH

A: Given : [H3O+] = 2.7 * 10-5 M we have to find pH and [OH-].

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

A:

Q: Match the 0.10 M aqueous solution to the approximate pH range. HNO3 1. pH under 2 CH3NH3B

A: Acids are substances that donate protons in aqueous solutions whereas bases are substances that…

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

A:

Q: A solution of 0.00100 M HCI has a pH of: (HCl is a strong acid and dissociates completely in…

A: Given that, Concentration of HCl acid = 0.00100 M Since, HCl is a strong acid, it completely ionised…

Q: Determine the pH of a 0.20M CH3NH3I solution.

A: Given that: [CH3NH3I] = 0.20M  CH3NH3I is salt made up of weak base CH3NH2 and strong acid HI.

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10^-6 M.

A: Given that, in a solution, the hydrogen ion concentration is [H+] = 4.5×10-6 M. We have to calculate…

Q: Determine the pH of the 1.5M HNO2. The Ka = 4.0 x 10^-4 . HNO2(aq) + H2O(l) ↔ NO2 - (aq) + H3O ^+…

A: Given that Ka for HNO2 = 4.0 x 10^-4 write the ICE Table and solve for the x by writing the Ka…

Q: Calculate the pH of a 1.60 M KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10

A: In case of conjugate acid-base pairs,  Ka is acid dissociation constant and Kb is base dissociation…

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

A:

Q: alculate the pH of the following solutions. a) [H3O*] = 1.0×10-4 M pH=| b) [H;O*] = 0.10 M pH = «)…

A:

Q: Calculate the pH of a 0.018M H2SO4 solution that has a Ka1=strong and Ka2=1.2•10-2

A:

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

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: what is the pH of a 0.140 M solution of NH4Cl? ka for ammonium is 5.68x10^-5

A: A salt that contains either weak acid ions or weak base ions does not exact 7 pH values. Its pH…

Q: What is the pH of 2.9x10 M

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Q: When the pH is 7, there is no H30* or OH in solution.

A: A question based on pH concept, which is to be accomplished.

Q: 6. Calculate the pH of the solution if the concentration of [H3O] ion is 2.0x10 M at 25°C.

A:

Q: Calculate [OH-] for a solution where [H3O+]=0.00461 M. [OH-J= Calculate the hydronium ion…

A: Note: As per our guidelines, we are supposed to answer only one question. Please repost the other…

Q: What is the pH of a 1.00 molar solution of NH4Cl(aq)? The Kb for NH3 = 1.8 × 10–5 .

A: Ammonium chloride dissociates completely into ammonium and chloride ions. The ammonium ion is the…

Q: Calculate the pH, pOH, and [OH-1] of solution in which the [H3O+]=1.2x10-3

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Q: Calculate the pH of a 0.36M methylamine (weak base) (CH3NH2) solution, if Kb = 4.4x10-4

A: In aqueous solution, methylamine undergoes the acid base reaction: CH3NH2 aq + H2Ol  → CH3 NH3+ +…

Q: What is the pH of a 3 M HNO2 solution if the Ka of HNO2 is 4x10^-4

A: pH helps in determining the level of acidity or basicity of any chemical. Mathematically, pH is…

Q: Calculate the pH of a 0.188 M NH3 solution. The Kb of NH3 is 1.76 x 10-5 O 5.480 O 12.656 O 11.260…

A: NH3 dissociates in water as,                                     NH3 +H2O -----> NH4+ + OH-…

Q: What is the pH of the following solution. 0.035 M HNO3

A: Given data contains, Molarity of nitric acid is 0.035 M.

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

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Q: The pH of a 0.02 M NgOH solution at 25 °C is: O 12.8 O 13.7 O 1 1.5 O 12.3 O 13.1

A:

Q: What is the pH of a 0.0001OM solution of HCI? * O 1.0x10-4 0.30 2.0

A: Given The  concentration of HCl=0.00010 M.

Q: What is the pH of 0.0005 M HNO3?

A: The given data is as follows: The concentration of HNO3 = 0.0005 M As we know that HNO3 is a strong…

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

A:

Q: Calculate the pH of a 0.052 M (C2H5)2NH solution (Kh = 1.3 × 10). pH =

A:

Q: 2. Complete the following table: [H;O*] [OH] pH Solution is acidic, basic or neutral 4.56 X 102 3.5…

A: In the given problem we are required to complete the table in which we have to calculate the pH,…

Q: What is the pH of a solution that has a [OH] = 3.3 x 10-³ M

A: pH is the negative logarithm of the concentration of H+. pOH is the negative logarithm of the…

Q: Determine the pH of the following solutions at 25°C. (a) H30*= 2.19 × 10-10 M pH %3D (b) [H,0*] =…

A:

Q: What is the pH of the following solutions? [H+] = 1.5 × 10-3 M ▪ [H+] = 8.7 × 10-12 M %3D [OH-] =…

A: The solutions are given below -

Q: What is the pH of a 0.150 M NH4Cl solution? Kb of NH3 = 1.76 × 10−5

A: Given, Concentration of NH4Cl solution (C) = 0.150 M Kb for NH3 = 1.76 × 10-5 pH of a NH4Cl solution…

Q: Calculate the pH. 0.5 M H3PO4

A: pH is used to determine the concentration of hydronium ion.

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: 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 pH of a solution with [H3O*] = 3.2x10-5M H3O*?

A:

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

A:

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: What is the pH of a 0.233M solution of aniline hydrochloride?           C6H5NH3+(aq)  +   H2O(l)…

A: The acid dissociation constant of anilinium is calculated as,

Q: Calculate the pH of the following aqueous solution:           0.62 M H2S (pKa1 = 7.00; pKa2 =…

A: H2Saq⥪H+aq+HS-aq                                       pKai=7.00                PKa1=-log Ka1…

Q: Determine the pH of a 0.18M H2 CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 x 10-7…

A: In this question, we will determine the pH of the solution.  Here, in diprotic acid case first…

Q: Calculate the pH of a solution with a H3O+ concentration of 5.8 × 10^-4 M

A: Given: Concentration of H3O+ = 5.8*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.