For  1.15×10−2 M Ba(OH)2, determine [OH−] and [H3O+]

Q: Calculate [OH-] when given the [H3O+] in each of the following aqueous solutions and classify the…

A: The OH- has to be calculated for the given aqueous solutions and whether they were acidic, basic or…

Q: Explain why pH of 0.1M HCl is not the same as the pH of 0.1M HF?

A: Answer  Explain why pH of 0.1M HCl is not the same as the pH of 0.1M…

Q: Determine the H+], OH-|, and pOH of a solution with a pH of 2.70 at 25 °C. [H*] = [OH] = РОН %3

A: Solution : pH       pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: Determine the [OH-] concentration in a 0.235 M NaOH solution.

A:

Q: Determine the [OH], [H;O*], pOH and pH of a 0.001 M KOH solution.

A: Given,

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: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: Which of the following is the formula for a weak acid? О А. НF B. HCIO4 C. H2SO4 O D. HNO3

A: Weak acid  is partially  dissociate into its  ion in aqeous  solution  (I.e. water) . And strong…

Q: Determine the [OH-] concentration in a .235 M NaOH solution.

A: The Concentration of OH- will depend on the base from which it is dissociated and the concentration…

Q: What is the pH of a 0.010 M solution of HF?

A:

Q: What is the pH of a 0.00360 M solution of HCI?

A: Given, [HCl] = 0.00360 M PH is defined as negative logarithm of concentration of [H+] ions.

Q: Consider the compound H2S Why does the charge change between the acid and conjugate base?

A: The compound, H2S behave as an acid in it's aqueous solution. When it is dissolved in water , it…

Q: Given a solution in which the pH = 4, determine [H+], [OH-] and pOH.

A: Inorganic chemistry.

Q: Question 17 of 25 Submit which of the following pH values? H2N. A) 1 B) 4

A: Given is deprotonated amino acid.

Q: Arrange the following in order of highest to lowest concentrations of [H3O'), that is, the most…

A: pH = -log[H3O+]  log[H3O+] = -pH So, [H3O+] = 10-pH  As pH + pOH = 14.0  So, pH = 14.0 - pOH

Q: W

A:

Q: 2. Complete the following table with the needed [H3O*], [OH]], and pH, and classify the solution as…

A:

Q: Which of the following describes a base using the Bronsted-Lowery theory? A. produces OH⁻ in…

A: Bronsted-Lowry deals in classifying acids-base as per their ability to gain/loss of protons. Species…

Q: Using the Arrhenius theory, classify the compounds as either an acid or a base.   Al(OH)3 CsOH…

A: According to Arrhenius theory if an atom/ion/species gives proton(H+ ion or H3O+ ion)on dissolving…

Q: Calculate [H3O1] in a solution that has [OH-] = 6.7  M at 25 degrees celcius. Is the solution…

A:

Q: Determine the [H3O+] concentration and whether the solution is acidic, basic, or neutral : a) [OH-]…

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: Calculate the value of [OH−] from the given [H3O+] and label the solution as acidic or basic. a.2.6…

A:

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

A:

Q: What is the pH of a 0.00560 M solution of HCl?

A: pH = -log[H+]

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

A:

Q: Determine the pH of the following: 1. 0.02850 M µM Mg(OH)2

A: [OH]- = 2 × [Mg(OH)2] + 10-7 M = 2 × 0.02850 × 10-6 + 10-7 M = 1.57 × 10-7 M

Q: Calculate the pH of each of the following solutions. Round each of your answers to 2 decimal places.…

A: Ba(OH)2 dissociate as follow Ba(OH)2 + H₂O → Ba²+ (aq) + 2OH(aq) According to dissociation reaction…

Q: Calculate [OH-] if [H3O+]=4.01x10^-4 and [H3O+]=7.22x10^-6

A: Given the concentration of [H3O+] =4.01×10-4 and [H3O+] =7.22×10-6we are asked to calculate the…

Q: Determine the pH of a 0.15 M solution of hydrabromic acid, HBr, at 25"C.

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

Q: What is the pH of a 0.00890 M solution of HCI?

A:

Q: Calculate [H3O+]and [OH−]or each of the following solutions at 25 ∘C given the pH pH=8.76 pH= 11.29…

A: pH is used to determine the concentration of hydronium ion . The expression for the pH is shown…

Q: Determine the pH of the following solutions: a) 0.01 M HNO; b) 8.750 x 10“ M HCI c) 0.0005 M KOH 13)

A:

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

A: We know that ., PH = 14 - POH POH = - log [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 0.020M HBr solution?

A: 4th ans is correct but not the 5th one Since in 4th we have reaction  HBr ----> H+ + Br-  Hence…

Q: Given 0.035 M of HCI, calculate the following: pH = pOH = [H] = M JOH:1 =

A: pH is the power of hydrogen or potency of hydrogen. The range of pH scale is from 0-14. The range…

Q: What is the formula for calculating the [OH−] from the [H3O+]?

A: ANSWER

Q: Determine the [OH'], [H;O*], pOH and pH of a 0.001 M KOH solution.

A: KOH ----> K+  + OH-  [OH-] = [KOH] = 0.001 M [ H3O+ ] = Kw÷ [ OH- ]               = 10-14/0.001 =…

Q: e) CSOH f) NH3

A: SOLUTION  CsOH is a strong base. NH3 is a weak  base. Hydrolysis of bases CsOH (aq)  --> Cs+ (aq)…

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

A:

Q: For the strong acid 0.0750 M HCl, determine [H3O^+] and [OH^-].

A:

Q: Calculate the [H3O+] in solutions with the measured pH values shown here:A.pH = 7.35 B.pH = 3.45

A: Provided pH of solution (A)=7.35 Provided pH of solution (B)=3.45 Since, Concentration of H3O+=10-pH

Q: A: Classify the following as Brønsted acids, bases or both. Write the letter that corresponds to…

A: According to Bronsted acid-base theory, acid is the the proton (i.e. hydrogen ion) donor and base is…

Q: Classify the following solutions as acidic, basic, or neutral at 25°C.

A:

Q: What is the pH in a 0.0001 M solution of LiOH?

A: Given, Concentration of LiOH solution = 0.0001 M  pH of the solution = ? Lithium hydroxide (LiOH) is…

Q: Consider the reaction.   CH3CH2O−+HC≡CH↽−−⇀HC≡C:−+CH3CH2OH   Classify each reactant and product…

A: According to the Brønsted theory of acids and bases, 1) Acids are those substances which donate…

Q: Complete the following table with the needed [H3O*], [OH'], pH, and pOH. Then, classify the solution…

A: We know that the concentration of hydromium ion and hydroxide ion are same in the solution. We also…

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.