determine the [OH-] in a 0.24 M solution of HClO4. answer in units of M

Q: What is the [H3O+] of a solution if [OH−] is 5.0 × 10−8 M?

A:

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: What is the pH of a 0.00349 M solution of HCl?

A: HCl is a strong, monobasic acid and dissociates completely as per the following reaction:- HCl (aq)…

Q: 2. One mole of H* is always neutralized by mole of OH-.

A: -> If water form from combination of ions  then it is neutralization .

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: What is the [OH-] if the [H+] concentration is 3.1x10^-4 Molar?

A: The concentration of H+ ions is 3.1×10-4 M. The relationship between the concentration of H+ ions…

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

A:

Q: 1. The formula for the conjugate base of H2S is 2. The formula for the conjugate acid of H2PO4" is

A: Determine conjugate base and acid of the given substance----

Q: Calculate the percent ionization of hydrazoic acid (HN3)in solutions of each of the following…

A: The dissociation constant of HN3 i.e Ka is = 1.9 X 10-5  And the dissociation reaction of HN3 is…

Q: Calculate the [OH-] of a solution at 25°C, if [H*] = 4.4 x 10-3 M. (answer in scientific notation)…

A: Given :- [H+]  = 4.4 × 10-3 M To calculate :- [OH-] at 25°C

Q: Oxalic acid 1H2C2O42 is a diprotic acid. By using data in Appendix D as needed, determine whether…

A: According to Bronsted acid- base theory, the compounds which donate protons (H+) are known as…

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: Determine the [OH-] and pH of a solution that is 0.250 M in HCO3-.

A: Kb is the base dissociation constant, which measures the dissociation of base into its ions…

Q: Convert each of the following OH- concentrations to pH. 0.00079 M

A: The pOH of the solution containing 0.00079 M of OH- is calculated as shown below.

Q: For a given aqueous solution if [H+]=1.0x10^-9 M, what is [OH-]

A: Concentration of [H+]=1.0x10^-9 M in aq.solution. Concentration of [OH-] = ? Formula: Ionic…

Q: Complete the following sentence. A5.3x10 M solution of HF has a pH __3.3. Select an answer and…

A: The answer is given as follows

Q: Determine the [OH-], pH, and pOH of a solution that is 0.125 M in CO3 2-.

A: Given information: Concentration of carbonate ion = 0.125 M

Q: In most solutions containing a strong or weak acid, the autoionization of water can be neglected…

A: Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

Q: Calculate the percent ionization of a 0.577 M solution of hypochlorous acid. % Ionization:

A: Given : Concentration of hypochlorous acid i.e HClO = 0.577 M The Ka of HClO = 2.8 X 10-8…

Q: Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution

A: Construct ICE table and calculate the required values,

Q: Determine the [H*], [OH-], and pOH of a solution with a pH of 13.23 at 25 °C. [H*] =

A:

Q: A solution has an [H_O*] = 8.25 x 109. Calculate each of the following values for this solution [OH]…

A: We have given that [H3O+] = 8.25 × 10-9 We Know that                     [H3O+] [OH-] = 10-14…

Q: Determine the [OH-] in a solution with a pH of 4.963.  Your answer should contain 3 significant…

A: Given data: The pH of a solution=4.963. To calculate: The concentration of hydroxide ion is [OH-].

Q: Fill in the missing chemical formulae in the tables below. base conjugate acid H,0 ? HSo, NH,

A:

Q: 1. The formula for the conjugate base of H2S is 2. The formula for the conjugate acid of HCO3 is

A:

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

A:

Q: A. Write the formula of the conjugate acid or base of the following substances: 1. Acids a. HC1O b.…

A:

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

A:

Q: How much more H+ is there in an acidic solution at pH 3 than a neutral solution?

A: The pH scale is a logarithmic one, meaning that each pH unit has 10 times as many hydrogen ions as…

Q: Calculate the percent ionization of a 0.355 M solution of nitrous acid. % Ionization =

A:

Q: Find the [OH-] of the solution, if the [H3O+] is: 2 ´ 10-11 M

A: Given that,  Concentration of [H3O+]   = 2×10-11 M

Q: What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M?

A:

Q: Calculate the pH of each of the following strong acid solutions: 5.00 mL of 0.250 M HClO4 diluted to…

A:

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

A:

Q: Determine if the following substances act as an acid or base in the given reaction. 02- + so3 →…

A: Given, The chemical reaction,  O2- + SO3 ---------> SO42-

Q: Calculate the [OH-] of [H+] = 5.4 x 10^-5 M at 25 degrees Celsius. Identify the solution as neutral,…

A:

Q: Determine the (a) degree of ionization and (b) percent ionization of ethylamine, C2H5NH2 in an 0.85…

A: Given concentration of ethylamine = 0.85 M Standard value Kb for ethylamine = 4.3*10-4

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: For an aqueous solution of 0.045 M HNO3, calculate the values of the following parameters:  [H+ ],…

A:

Q: What is the pH of a 0.00810 M solution of HCl?

A: pH of a Solution pH of a solution can be determined by the following formula pH = -log[H+ ] Where…

Q: Determine the [OH-] in a solution with a pH of 4.358.  Your answer should contain 3 significant…

A: The relationship between the pH and [OH-] is given by  pH = 14 + log[OH-]  where [OH-] =…

Q: The pH of a solution is (6.5x10^0). What is the [OH-]? Report your answer to 2 sig figs. Note: Your…

A: Given, pH of the solution = 6.5 × 100 = 6.5 Concentration of the OH- ion = [OH-] = ? The formula…

Q: cle the solution that is most acidic in the list below. Aqueous HCI, pH 1.0 NaOH(aq), pH 11.5 Water,…

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

Q: Given an OH- concentration of 0.10 M, calculate the H3O+ concentration, then identify the solution…

A:

Q: The hydroxide ion concentration of an aqueous solution of 0.365 M hypochlorous acid is

A: The hypochlorous (HOCl ) is an acid weak acid and it partially dissociates as…

Q: what is the hydrogen (hydronium) ion concentration (in M)?

A: We know that pH + pOH = 14  ...(1)  Given that pOH = 13.933  Putting it into the above equation, we…

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

A:

Q: The hydroxide ion concentration of an aqueous solution of 0.533 M acetic acid is [OH-] =  M.

A: Consider the given information is as follows; Concentration of acetic acid CH3COOH = 0.533 M OH- = ?…

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

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

Q: The [OH-] of an aqueous solution is 3.5x10 -5. What is the [H+]

A: The relationship between pH/pOH and concentration is :   pH= -log [H+]             pOH= - log [OH-]…

Q: What is the pH of a 0.00670 M solution of HCl?

A: pH = -log [H+]

Q: If the [OH^-] of a solution is 1 x 10^-6M, what is the concentration of the hydronium ion ? __ Is…

A: Given : [OH-] = 1 x 10^-6M

Q: 1. The formula for the conjugate base of HNO2 is 2. The formula for the conjugate acid of CH3COO is

A: Write conjugate base and conjugate acid of the given---

Q: Calculate the [OH-] of a solution with 10.0 M H3O+ and classify as acidic, basic, or neutral.

A: Given : Concentration of H3O+ in the solution = 10.0 M

Q: Determine the concentration of OH- and H3O+ in a 0.0123 M solution of sodium cyanide, NaCN.

A:

Q: Household ammonia is a solution of the weak base NH3 in water. List, in order of descending…

A: To arrange all the ionic and molecular species present in a 1-M aqueous solution of weak base NH3

Q: What is the [H'], [OH], pH and pOH of a 1.89x106 M HCl solution? Is this solution acidic, basic, or…

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

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: HCl (hydrochloric acid)     NaOH (sodium hydroxide

A:

Q: determine the pH of a 0.0006 M NaOH solution

A: We know that, Negative logarithm of H+ ion is know as pH. pH= -log[H+] & pH + pOH =14 & pOH…

Q: Calculate the [H;O*] for a solution in which [OH] = 2.7 x 1011 M. Is this solution acidic, basic, or…

A:

Q: Arrange the following 0.10 M solutions in order of most acidic to most basic. KOH, KNO3, KCN, NH4Cl,…

A: The given species has to be arranged from most acidic to most basic.

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.