The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶. What is [OH⁻]?

Q: rite the formula of the conjugate base of the Brønsted-Lowry acid, H₂C₂O₄

A: H2C2O4

Q: How many grams of ammonium sulfate (NH4)2SO4 are needed to make 6.0 liters of a 2.5 M concentration?…

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Q: An aqueous solution at 25°C  has a OH− concentration of 4.6 x 10^−9M. Calculate the H3O+…

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Q: If the H+ concentration in a carbonated beverage is 4.7 ´ 10-5 M, what is the OH- concentration? (Kw…

A: The H+ and OH- concentration in aqueous solution is related by the following relation- H+ + OH- = Kw…

Q: The hydroxide ion concentration, [OH-], of an aqueous solution of 0.458 M dimethylamine (a weak base…

A:

Q: What is the [H30+] concentration in a solution that is 4.25x10^-4 M C6H5NH3+? Kb = 3.98 x 10^ -10

A: Given data, Kb of C6H5NH2 = 3.98*10-10  [C6H5NH3+]=4.25*10-4 M  Then, [H3O+]=?

Q: A solution has [OH- ] = 4.0 x 10-8. What is the value of[H+] for the solution?(a) 2.5x 10 -8 M (b)…

A: Concentration of OH- ion is 4.0×10-8 M. Product of [H+] and [OH-] is equal to the ionic product of…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.3 × 10⁻⁵. What is [H⁺]?

A: Given: [OH- ] = 2.3 × 10-5 M

Q: Write the formula of the conjugate base of C6H5NH2.

A: The conugate base is formed by removing one H+ ion from any molecule.

Q: c. 1.520M HCN solution, KA= 4.12x 10 d. 3.85 x 10° M CH,NH, solution that is 0.900% ionized e. 2.35…

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Q: The OH- concentration in an aqueous solution at 25 °C is 6.5 x 10-5. What is [H*]?

A: The given data is as follows: The concentration of the hydroxide ion, OH-=6.5×10-5 M H+=? The…

Q: Classify each of the following substances as either a strong or weak acid, strong or weak base, or a…

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Q: An aqueous solution at 25 °C has a OH concentration of 3. × 10 M. Calculate the H,0' concentration.…

A: Given: [OH-]=3×10-9 MTemperature=25oC To find: [H3O+]

Q: Please solve for part a & b. Assume complete neutralization.

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Q: What is the pOH of a 6 x 10-7 M aqueous solution of HCl?

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Q: Which of the following (assuming the same concentration in water) would make a solution with the…

A: Strong acid: Strong acids completely dissociate into their ions in water. Let HA is strong acid then…

Q: Use the following information to answer question 36. Trichloroacetic acid, CC13COOH(aq), is used in…

A: Acidic species after loosing proton form conjugate base. Amphiprotic species is species which can…

Q: Write the formula of the conjugate base of the Brønsted-Lowry acid, HCOOH

A: A conjugate base contains one less H atom and one more - charge than the acid than the acid that…

Q: Calculate the volume of concentrated HCl necessary to prepare 12 mL of 6M HCl

A: Molarity is defines as total no of moles of Solute dissolve 1000 ml of solution  Consider molarity…

Q: Which of the following solutions is the most basic solution? A) POH = 5.0 B) PH=10.0 C) [H+] = 1.0 x…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the neutral pH of water at 40 degrees celsius?

A: In the neutral solution:

Q: The (OH-] concentration of an aqueous solution is 1.0 x 10-4, what is its [H3O+] concentration? O 1x…

A: The ionic product of water (Kw) is given by the following equation:  Kw=H3O+·OH- The Kw is an…

Q: Write the formula of the conjugate base of the Brønsted-Lowry acid, C₆H₅COOH?    The OH⁻…

A: Given,  (a). Write the formula of the conjugate base of the Brønsted-Lowry acid, C₆H₅COOH?   (b).…

Q: The hydroxide ion concentration of an aqueous solution of 0.502 M nitrous acid is [OH]=| M. %3D

A: pH is the negative logarithm of proton.

Q: 1.243 grans di bm ne ( dissolved ina 2ohkolaquedus olunon How manyP DABA

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

Q: An aqueous solution at 25 °C has a H,O' concentration of 3. x 10 'M. Calculate the OH concentration.…

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Q: Find the molarity of a KOH solution if 13ml of 2.1M HCl solution is neutralized by 13ml of KOH…

A: The equation to find the unknown quantity from the known values is given by, M1V1=M2V2 where M is…

Q: The hydronium ion concentration of an aqueous solution of 0.377 M ethylamine (a weak base with the…

A: Given, Concentration of of ethylamine solution (C) = 0.377 M [H3O+] = ? M ethylamine (C2H5NH2) is a…

Q: A solution that is found to have a hydroxide concentration of 4.69 x10-5 that is at the freezing…

A: Please find the attachment

Q: A solution that is found to have a hydroxide concentration of 4.69 x10–5 that is at the freezing…

A: Solution:-  Given:            The  hydroxide ion concentration of the solution=[OH]-=4.69 x 10-5…

Q: How much more/less concentrated is a solution with a pH of 2 than a solution with a pH of 5? 10 x…

A: Given , pH=2 and pH = 5 We know that, pH= -log[H+] Where [H+] is concentration of solution. The…

Q: Complete the table below. (All solutions are at 25 °C) [H3O +] pH РОН L но 9.42 2.5 x 10-10

A: The relationships are as shown below  pH = -log[H3O+] = 14 + log[OH-] = 14 - pOH pOH = -log[OH-]…

Q: How many of the following compounds are insoluble in water? NaC2H3O2 SrSO4 BaS AlPO4

A: At a certain temperature, the dissolving property of any compound in a liquid in order to make…

Q: If the concentration of H+ ions in a solution is 3.16x10^-4mol/L, then what is the concentration of…

A: Given, Concentration of H+ ion = [H+] = 3.16 × 10-4 mol/L Concentration of OH- ion = [OH-] = ? Some…

Q: calculate the molar concentration of OH- in water solutions to H3O molar concentrations

A: According to the question, we are asked how to calculate the molar concentration of OH- in water…

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pOH of 1.300?…

A: Given, pOH of the solution = 1.300 Concentration of potassium hydroxide, [KOH] solution = ? Note:…

Q: 4. pH = cermine the pHof each solutions 5. [H*] = 1.0 x 106 M 6. [H*]= 0.00010 M 7. [H*] = 1.0 x 10²…

A: pH = -log[H+]  pH + pOH = 14

Q: Of the following substances, which will form a basic solution in water? NaCIO2 Cu(NO3)2 KHCO3 NaF O…

A: NaClO2 dissociates in water to form strong base NaOH and weak acid HClO2. Therefore, the overall…

Q: What are all the ionic and molecular species present in a 0.001 - M aqueous solution of C6H4OH(CO2H)…

A: The answer is as follows:

Q: 9. Which types of solutions contain equal [H30*] and [OH¯]? Acidic solutions Basic solutions Neutral…

A: Classify when [H3O+] = [OH-]

Q: Which of the following compounds is insoluble in water? (NH4)2S CaCO3 NaOH Ag2SO4 Pb(CH3COO)2

A: Observing all five given compounds show that except Calcium carbonate all other are soluble in…

Q: An aqueous solution at 25C has a hydronium ion concentration of 9.7x10^-5 M. What is the hydroxide…

A: Acid are the substances that have tendency to donate proton in solution. HCl→H++Cl- Acid has pH…

Q: Urine  has an [OH-] concentration of 2.0 x 10-9. What is the pH of urine?

A:

Q: hat is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH?…

A: The dissociation of hydroxylamine

Q: What type of solution has a hydroxide ion concentration, [OH-], that is greater than a hydronium ion…

A: Acidic solutions are those which have pH < 7 and basic solutions are those which have pH > 7

Q: The following table summarizes the [H*], [OH-], pH, pOH, and type of solution of some common…

A: Formula used :- pH = -log[H+] , pOH = -log[OH-]  pH + pOH = 14  [H+][OH-] = Kw

Q: Write the formulas of the conjugate base of the Brønsted-Lowry acid: 1. HF 2. HC₃H₅O₃   3. HC₂O₄⁻ 4.…

A: Bronsted-Lowry acid base theory states that acids are the species with the ability to donate protons…

Q: please highlight the correct answer

A: The addition of an acid to water decreases the pH of water by introducing hydrogen ions in the…

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.