Calculate the pH of 1.0M NaHSO2 solution. (Ka1=1.2x10-2 ; Ka2=6.6x10-8). Show the complete solution

Q: Determine the pH of a 2.50 M of a diprotic acid (DA) whose Ka1 = 2.60 x 10-4 and Ka2 = 1.60 x 10-12.

A: Given,The molarity of diprotic acid ( DA ) = 2.50 MKa1    and Ka2 = 1.60 x 10-12

Q: The acid dissociation constant K of alloxanic acid (HC, H, N₂O₂) is 2.24 × 107. Calculate the pH of…

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Q: Calculate the pH of 58.2 mL of a 0.507 M hypoiodous acid (HIO, Ka = 2.3 × 10−11) solution after 10.2…

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Q: Calculate [H+] and pH in a solution in which [HNO2] is 0.10 M and [NO2:] is0.20 M. Given Ka = 4.5x…

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Q: What is the pH of a solution that is 0.10 M HNO2 and 0.10 M NaNO2 (the conjugate base)? Ka of HNO2 =…

A: To solve the pH of the solution, you can use the Henderson-Hasselbalch equation, which…

Q: Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

A: Dear student,  As you have asked multiple question but according to guidelines we will solve first…

Q: A solution is prepared at 25 °C that is initially 0.38M in diethylamine ((C₂H₂)₂NH), chloride…

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Q: Calculate the pH of a solution when 21.0 mL of 0.050 M hydrazine (N2H2, Kb=8.9E-7) is titrated with…

A: pH of a weak base titration with strong acid can be determine using Henderson hasselbalch equation.

Q: Calculate the concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data:  Ka1 = 4.2×10-7…

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: Which is a stronger base S^2- or Se^2-? Explain your answer.     Please provide answer correctly…

A: Given -> S2- & Se2- -> order of Basicity of conjugate base is same as order of basicity of…

Q: Calculate the pH of a 0.40 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5…

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Q: What is the pH of a 0.459 M solution of NaCIO. K₁ = 2.87 × 10-8

A: Given that, the concentration of the NaClO is C = 0.459 M. The Ka = 2.87×10-8. We have to calculate…

Q: Enough base was added to an amount of water to produce an aqueous solution with [OH-] = 2.4 x 10-5.…

A: Given, Concentration of Hydroxide ion = [OH-] = 2.4 × 10-5 M Concentration hydronium ion = [H3O+] =…

Q: 16. Look at the salts listed below. Label these as acidic, basic or neutral. Ka & Kb values…

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Q: Calculate the pH of 4.0 X10 -4 M KOH

A: Please find your solution below : pH is a measure of acidity or basicity of a substance. It is…

Q: Calculate the pH of a 0.57 M CH3COONa solution. (Ka for acetic acid=1.75 × 10 )

A: Answer:As we know,Also,

Q: Calculate the pH for a 15.9 M aqueous solution of NH3. (Kb = 1.8 x 10-5 for NH3)

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Q: A diprotic acid, H, A. has acid dissociation constants of K₁1 = 4.63 x 10 and K₂ = 5.82 x 10-12.…

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Q: Calculate the pH of an aqueous solution at 25°C that is 0.29M in phenol (C,H;OH ). (K, for phenol =…

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Q: Calculate [OH-] of NaClO, 0.110M; KaHClO = 3.0 x 10-8.

A: Given: Concentration of NaClO is 0.110 M Ka (HClO) is 3.0×10-8 To determine: [OH-]

Q: 1.50 mol of calcium chlorite is dissolved in enough water to produce 4.50 L of solution. K₂2.9 x…

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Q: Calculate the concentration at which a monoprotic acid with K, = 3.0 x 10 will be 1.6% ionized.

A: Dissociation constant (K) - In dissociation reaction, ratio of concentration of product (dissociated…

Q: Which of the following statements is correct? O The pH of a 0.05 M solution of H2SO3 is equal to 1.0…

A: Solution: The correct statement among the given statements is as follows --- b) In a neutral…

Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56

A: The concept used here is based on the acid dissociation constant of an acid which is used for…

Q: A solution with a pH of 7 has a [OH1-] of Group of answer choices 1 x 10-7 M 0 M 1 x 10-14 M 7 M

A: Given is, pH= 7

Q: Write the conjugate base of each acid in HNO2,  Ka = 4.6 x 10-4; HClO2,  Ka = 1.1 x 10-2; HCN,  Ka…

A: If an acid lose one proton, then the formed species is a conjugated base.

Q: Hi, I am in chemistry 2 and am working on acids and bases. However im struggling with identifying a…

A: The question is based on the concept of salt hydrolysis. We need to identify the nature of given…

Q: The Kb for NH2OH = 6.6 × 10-9. What is the pH of a 0.50 M solution of NH2OH?

A: Given Kb for NH2OH = 6.6 × 10-9  Concentration = 0.50 M

Q: . Morphine is a weak base for which Kb is 8 × 10-7 . Calculate the pH of a solution made by…

A: Let 'B' represents morphine. Initial concentration of B=moles/volume…

Q: Calculate the pH of a solution containing 0.03 M NaH2VO4 and 0.05 M Na2HVO4. (Ka1 = 1.11×10-2, Ka2 =…

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Q: Maleic acid (H,C,H,O,) is a diprotic acid with Kal = 1.20 × 10-3 and Ka2 = 5.37 × 10-7. Determine…

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Q: Determine who the stronger acid and base are based upon the following information: a HA+H₂O=H₂O* +…

A: The objective of the question is to determine the stronger acid and base based on the given…

Q: which of the following would have the strongest conjugate base?

A: The equilibrium constants, Ka and Kb of weak acid and conjugate base are related through the below…

Q: Calculate the pH at 25°C of a 0.0045 M solution of a weak base with a K, of 9.8 x 10⁹. pH =

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Q: Based on the pH, determine [OH ] at equilibrium for this weak base solution. Express your answer to…

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Q: Find the pH of a 0.50 M solution of NH4NO3 at 25 given the following values (also at 25 °C). Kb for…

A: Given,Molarity of NH4NO3 = 0.50 Mat 25 oC,     Kb of NH3 = 1.8 x 10-5                   Ka of HNO3…

Q: the two ammonia species are ammonia (NH3) and the ammonium ion (NH4+. The total ammonia…

A: NH4+= NH3+ H+  pka =6.34  pH = 8 Concentration of…

Q: Fill in the rest: (Use only the exponent for H and OH) pH:  H+:  pOH:  OH-: 10-4

A: [OH-] = 10-4 (given )  pOH = - log [OH-]  pOH = - log (10-4)  pOH = 4  Since, we know that ; pH +…

Q: Calculate the pH of a 0.29 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.6…

A: The question is based on pH calculation. we have been given a weak acid. we have to calculate its…

Q: Which of the acids listed below has the weakest conjugate base? O H₂02; K₂ = 2.400x10-12 O HBr, K₂=…

A: The larger the value of ka stronger the acid and weaker the conjugate base.

Q: 2. Solution of ammonium chloride, NH4CI has a pH = 5.05. Calculate the volume of water to be added…

A: NH4Cl is a salt of strong acid and weak base.Initial pH of solution is 5.05 and final ph of solution…

Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?

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Q: 3. What is the pH in a solution with [H*]=2.5x10-5? %3D

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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.