Determine the concentrations of the following ionic species present in a 0.350 M solution of Na2SO3. For H2SO3, Ka1 = 1.4E-2, Ka2 = 6.3E-8.

Q: Calculate the pH of a solution that contains 3.9 x 104 M H3O* at 25°C. 4.59 3.41 10.59 9.41 0.59

A: Given, Concentration of H3O+ ion = [H3O+] = 3.9 × 10-4 M Temperature (T) = 25°C pH of the solution =…

Q: The pH of a solution for which [OH-] = 1.0 x10-6 is %3D

A: pH stands for Hydrogen potentials. pH is a negative logarithm of the concentration of hydrogen ions.…

Q: arrange the following oxoacids in order of decreasing acid strength: HClO, HClO2, HClO3, and HBrO

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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: Determine the concentrations of the following ionic species present in a 0.271M solution of Na2SO3.…

A: ANSWER : (i) Concentration of OH- ion  =  0.000207 M (ii) Concentration of HSO3- ion  =  0.000207 M…

Q: Calculate the molar concentration of OH− ions in a 0.069 M solution of ethylamine (C2H5NH2;…

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Q: How would the pH of a 0.175 M solution of NaC4H,O2 compare with that of a 0.175 M solution of…

A: The salt gets hydrolyzed when dissolved in water. Both salt have the same acid and similar strong…

Q: A substance which can act both an acid and a base is: A. allotropic B. amphoteric C. isotopic D.…

A: We are given terms : Allotropic, Amphoteric , Isotopic and Amorphous

Q: What is the % ionization of 1.75 M NH3 (aq) from the previous problem? O .00551 % O.00180 % 0.00321…

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Q: and react to form Salt and Water. O Base, Acid O Compound , H2 O Base and Alkali O Acid, Base

A: Explanation to the correct answer given below

Q: Determine the pH of each of the following solutions. (a) 0.762 M hypobromous acid (weak acid…

A: Here, we have to calculate the pH of the given solutions: 0.762 M hypobromous acid (weak acid with…

Q: Calculate the concentration of all species in a solution prepared by dissolving 75.2 g of solid Na2S…

A: A numerical problem based on molarity, which is to be accomplished.

Q: Which of the following is a non-electrolyte?   AsBr3 Na2SO4 ZnCl2 Al(C2H3O2)3 HNO3

A: An electrolyte is the substance which when dissolved in the solvent provide an electrical conduction…

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: Write the equations for the dissocation of the following in aqueous solution:Na2S:[(NH4)2]CO3:KHSO3:

A: A compound dissociates into its corresponding ions in aqueous solution.a) Sodium sulphide…

Q: Determine the pH of each of the following solutions. (a) 0.549 M hydrogen peroxide (weak acid with…

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Q: Determine the pH of a 0.461 M C3H5CO,H M solution if the K, of C6H5CO2H is 6.5 x 105. 4.52 11.74…

A: pH  is commonly known power of hydrogen,  it measures the concentration of hydrogen ion in the…

Q: calculate the ph of a 0.600 solution of Na2S

A: When Na2S dissolved in water - Na2S + 2H2O <===> 2NaOH + H2S Thus, sodium Sulfide is a salt of…

Q: "For H3PO4, Kay = 7.3 x 103, Kaz = 6.2 x 106, and Kag = 4.8 x 1013. An aqueous solution of NaH2PO4…

A: So in the first equation,, H2PO4- is acting as a base and removing a proton from water. In the third…

Q: Calculate the pH and [S2−] in a 0.10-M H2S solution. Assume ka1= 1.0 × 10−7; ka2= 1.0 × 10−19.

A: Answer:- This question is answered by using the simple concept of calculation of pH of a weak acid…

Q: 1.Calculate the molarity of the hydrogen ion for each of the following solutions: a. pOH = 4.99 b.…

A: Four numerical problems based on pH concept, which are to be accomplished.

Q: Determine the pH of a 0.227 M C,H,N solution at 25°C. The K, of C,H;N is 1.7x 10°. 4.59 9.41 4.71…

A: Hence last option is correct that is 9.29

Q: Use the References t The pH of an aqueous solution of 0.177 M sodium fluoride, NaF (aq), is This…

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Q: Explain why KNO3 is a suitable salt to be used in salt bridge.

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Q: For a 1.0 x 10-6 M solution of HNO3(aq) at 25 °C, arrange the species by their relative molar…

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Q: What concentration of barium hydroxide is needed to give an aqueous solution with a pOH of 1.720?

A: Since barium hydroxide is a strong base Hence it will dissociate completely as per the reaction…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.7 × 10⁻⁴ M, then [OH⁻] is

A: In an aqueous solution [H₃O⁺] ×   [OH⁻]  = Kw

Q: A 1.2 · 102 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of, O 12.38 O 12.08 O 1.62 O 2.4 · 102…

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Q: When placed in water, which of the following will likely produce the weakest electrolytic solution?…

A: The solution is given below -

Q: determine the [H3O+] in a 0.24 M solution of HClO4. Answer in units of M

A: HClO4 is strong acid so it wil completely break into ions when we put this into water.

Q: Determine the concentrations of the ionic species present in a 0.367 M solution of the H2SO3. (pKa1…

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Q: In a neutral aqueous solution at 25°C, the molarity of hydronium ions is O 7 10-7 O 14

A: We are having a neutral Solution at 25° C. We have to calculate the Molarity of hydronium Ion.

Q: What is the percent ionization of an 3.5 M HF solution? (Ka=6.6 x 104) O 1.4 % O 0.22 % O2.4 % O 1.7…

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Q: Be sure to answer all parts. Enter your answer in scientific notation. The concentration of…

A: Given, Concentration of hydroxide ions = 4.9*10-4M. Equilibrium constant of water, Kw = 1.0*10-14.

Q: arrange hypochlorous acid, chloric acid, chlorous acid and perchloric acid in correct order of their…

A: HClO = Hypochlorous acid (oxidation state of chlorine = +1)HClO2 = Chlorous acid (oxidation state of…

Q: The concentration of charge contributed to a solution by [PO4°] is: O (PO1 [PO, ] O 1/2[PO4-] O…

A: Given: specie is PO43-.

Q: Calculate the theoretical number of moles of HCl equivalent to 1 mole of Al2O3

A: HCl is a strong acid and Al2O3 is an amphoteric oxide. Al2O3 reacts with acid and form salt and…

Q: Calculate the hydronium ions concentration, [H3O+ ], for a 0. 01 M HClO4 aqueous solution

A: Strong acids are completely dissociate in aqueous medium. HClO4 is strong acid.

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: Determine the concentrations of the following ionic species present in a 0.320 M solution of Na2SO3.…

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Q: Rank the following acids in order of increasing strength: ClCH2SH, CH3SH, H2S.

A: The acidic strength of any acid is proportional to the stability of the anion formed by removing the…

Q: What is the net charge on Arg at neutral pH (for the dominant ionic species)?

A: We have to predict the net charge at pH of 7 on arginine.

Q: What is the % ionization of .03 M HC2H3O2 (aq) from the previous problem? 0.00180 % 0.060 % 0.0137 %…

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Q: Your task is to create a schematic diagram on how to separate the following ions CO3-2, Cl-, NO3-,…

A: Solution -

Q: Calculate the hydrogen ion concentration in mol/l for solutions with the following ph values: (a)…

A: The relationship between pH and concentration of hydrogen ion is given as pH = -log[H+] where [H+] =…

Q: Arrange the following oxoacids in order of decreasing acid strength: HCIO, HCIO2, HCIO3, HBrO

A: Acidic strength is directly proportional to electronegativity  of the central atom. So HBrO is least…

Q: Calculate the pH of water containing 0.05 M NaCl at 25°C. Given: YH = 0.86 and %3D YOH- = 0.81. O…

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Q: Arrange the following substances in decreasing order of strengths: I-, V3+, Sn2+, Co2+, Ag, H2S, Ni,…

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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.