A weak base, B, has a concentration of 0.155 M. If the pH of the solution is 11.24, what is the K of the base?

Q: What is the concentration of the sodium ion (in M) in a solution of 0.714 M sodium carbonate?

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Q: Calculate the pH of a 2.44 M HCIO3 solution. Ka for this acid is 1.5x10³. HCIO3 is a weak acid.

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Q: Calculate the pH of the following: - 0.10 M disodium hydrogen arsenate

A: To calculate pH , we would use dissociation equation of disodium hydrogen arsenate and it's Ka…

Q: What is the concentration of lithium ions in 0.395 M Li HPO,?

A: The volume of the solution remains constant. When Li2HPO4 dissolve, it gives rise to two moles of…

Q: If the pH of a solution is 0.8, what is its hydronium ion concentration ?

A: pH = -log[H3O+]

Q: The pH of a 0.173 M solution of a weak acid, HB, is 2.53. What is Ka for the weak acid?

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Q: The molar concentration of OH- in a water solution is 8.5× 10−12 M. What is the concentration of H+…

A: It is given that the concentration of OH- ions in water is 8.5×10-12 M,

Q: You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the Kb of NaIO?

A: Solution pH, pKa, pKb, Ka, and K ar employed in chemistry to explain however acidic or basic an…

Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: If 0.235 g of KHP (potassium hydrogen phthalate) require 15.5 mL of NaOH solution to neutralize it,…

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Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: In the laboratory, a student adds 24.2 g of ammonium chloride to a 500. mL volumetric flask and adds…

A: Given - mass of ammonium chloride = 24.2 g  And, mass of the solution = 500 mL    Then , Molarity of…

Q: Calculate the K, of a weak acid if a 0.047 M solution of the acid has a pH of 3.57 at 25°C.

A: Given :-  Concentration of weak acid = 0.047 M  pH of solution = 3.57  To calculate :-  Ka

Q: What is the molarity of ions in a 0.706 M solution of KNO, assuming the compound dissociates…

A: Potassium nitrate KNO3 is a soluble ionic compound that dissociates completely in aqueous solution…

Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide…

A: The formula for Barium Iodide id BaI2  When it is dissolved in solvent it dissociates in the…

Q: Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a)…

A: Given The acid-dissociation constant (Ka) for hypochlorous acid is 3.0 x10-8. The initial…

Q: What is the concentration of OH– in a solution with a pH of 3.91?

A: The concentration of OH– in a solution with a pH of 3.91 is to be calculated.

Q: Find the pH of a 0.2 M solution of H2SO3

A: Given,  The pH of a 0.2 M solution of H2SO3 is:

Q: The pOH of a basic solution is 3.91. What is [OH⁻]?

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Q: If log K, for Ag(NH3)2* is 3.31 and log K2 is 3.91, what is K,?

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Q: What is the pH of a 0.103 M aqueous solution of potassium hypochlorite, KCIO? This solution is pH =

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Q: The pH of a 0.152 M solution of a weak acid, HB, is 2.53. What is K. for the weak acid?

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Q: the pH of an acid solution is 3.59. If the concentration of the acid in the solution is 0.200 mol/L,…

A: Given Concentration of the acid=0.2 mol/LpH of the acid solution=3.59Ka of thel acid=??

Q: What concentration of nitrous acid has a hydronium –ion concentration of 0.01 F?

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Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: What is the concentration of potassium ions in a solution which is 0.836 M in potassium phosphate?

A: The complete dissociation reaction of K3PO4 is,

Q: -SO,Na СHCI; ? + КОН > ? +

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Q: Nitrous acid, HNO₂, has a Kₐ of 7.1X10⁻⁴. What are[H₃O⁺], [NO₂⁻], and [OH⁻] in 0.60 M HNO₂?

A: First of all we have to write the equation for nitrous acid.     HNO2+H2O⇔H3O++NO-2…

Q: 3. How is K, obtained by the half-neutralization method?

A: Since you have posted multiple questions, we will solve the first question. Please post rest of the…

Q: A study of the acid shows that the pH of an acid HA O.12 MIK2.62. What is the K, of this acid?

A: Acid Dissocaition constant, Ka has to be determined for the Acid HA of 0.12 M with pH 2.26.

Q: For  K w, the product of [H 3O +] and [OH -] is

A: Kw is the water constant and is defined as product of hydronium ion and hydroxyl ion  Kw = [H3O+]…

Q: ) What is the pH of a solution of 0.626 M of a weak base if K, = 3.2x10-³? (Assuming X is very…

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Q: 6. What is the pH of a solution with a hydrogen concentration of 2.3x10-5M?

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Q: 2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NAOH, what is the initial concentration…

A: Answer: 2 Given: Volume of H2SO4 = 358mLConcentration  of  H2SO4 =?? Volume of NaOH=…

Q: What is the pH of a 0.380 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What is the pH of a 0.330 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)

A: Given : Concentration of C₅H₅NHBr = 0.330 M And Kb of C₅H₅N = 1.7 X 10-9  Since the salt C₅H₅NHBr is…

Q: The pH for 0.050 M of CH3NH3Cl ?

A: Methylammonium chloride (CH3NH3Cl) dissociates into quaternary ammonium ion (CH3NH3+) and chloride…

Q: What is the concentration of hydroxide ions with a pH of 4.76?

A: Given : pH = 4.76

Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What is the concentration of potassium ions in a solution which is 0.531 M in potassium phosphate?

A: The given compound is potassium phosphate.The molecular formula will be K3PO4.Dissociation of…

Q: How many grams of LiC2H3O2 are needed to prepare 1.83 L of a solution that has an ion concentration…

A: Consider the given information is as follows; Volume of the solution = 1.83 L Concentration = 0.745…

Q: If pH = 5.7, what is [OH ] ?

A: Given a PH = 5.7  Calculate the [OH-] concentration.    calculate the [OH-] of first of calculate…

Q: Determine the pH of a solution that is 0.00542 M HCl and 0.0513 M HClO2. The Ka of HClO2 is 1.1 ×…

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Q: а. What is the hydroxide ion concentration in a solution of sodium hydroxide having a pH value of…

A: Given, pH of NaOH(sodium hydroxide) solution is ------- 11.6 Since, pH+pOH=14⇒pOH=14-pHand…

Q: 2) A weak acid has a K,= 6.62 x 10. What is the pH of a solution of this acid that is 2.65 M?

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Q: Given the general equation illustrating the reaction of the acid HA in water, HA (ag) + H2O(1) H3O*…

A: According to the Bronsted Lowry theory, a base is a substance that accepts a proton whereas an acid…

Q: Fill in the left side of this equilibrium constant equation for the reaction of ammonia (NH,), a…

A: From given  Initially we are giving reaction of ammonia with water and Kb is calculated and the…

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.63. What is Ka for the weak acid?

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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.