find the pH of the 1 M solution, H2SO4 given that in the second stage of dissociation the acid H2SO4 behaves like a weak electrolyte K (HSO4 -) = 1.2

Q: 2. The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5).What is the pH of a 0.258 M…

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Q: Calculate the pH of a 0.274 M aqueous solution of quinoline (C9H7N, Kb = 6.3×10-10) and the…

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Q: Calculate the pH of 0.10 M solution of hypochlorous acid, HOCl, Ka = 2.9 x 10-8 (Weak acid) HOCl ⇌…

A: In multiple questions we solve only first question according to the Bartleby guideline. First find…

Q: Ka for nitrous acid, HNO2, is 4.50×10-4. Ka for benzoic acid, C6H5COOH, is 6.30×10-5. Ka for…

A: A question based on equilibrium concept that is to be accomplished.

Q: 5,Calculate the [OH-]of the solution with pH=10.50 Group of answer choices 1.05 x 10-10 5.0 x…

A: According to guidelines i can answer only first question, please repost the other one.

Q: Calculate the pH and pOH of the following substances: 1. 0.3 M sulfuric acid (H2SO4) solution 2.…

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Q: H3 is a weak base (?b=1.8×10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: Acetic acid (HC2H3O2) is a weak acid (Ka = 1.8 x10-5). Calculate the pH of a 10.6 M HC2H3O2…

A: Dissociation of acetic acid and pH calculation

Q: Calculate the pH of a solution containing 0.0361 M benzoic acid (HC>H502) and 0.0263 M sodium…

A: The given mixture is a buffer solution mixture. So, this can be solved from the Henderson…

Q: Calculate the pH of a solution of 0.15 M C5H5N. (Kb = 1.7 x 10^-9)

A: It is weak base so we will use concept of weak base.

Q: Complete the reaction H₂SO4 + 2 H₂O mplete ionization of HSO4-¹ What is the pH of a 0.001000 M H₂SO4…

A: ->H2SO4 is strong acid which can dissociate completely into ions H+ and SO42-. Molarity of H2SO4…

Q: What is the pH of a solution which is 0.023 M in weak base and 0.035 M in the conjugate weak acid…

A: The solution is as follows:

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: Arsenious acid is a weak acid HAsO2 AsO2- + H+ Ka = 10^-9.22 If 10-3 moles of arsenious acid are…

A: Arsenious acid is a weak acid which undergoes partial dissociation with degree of dissociation…

Q: Write an equation in which H2PO3 acts as an acid. (Use the lowest possible coefficients. Be sure to…

A: According to Bronsted Lowry concept, an acid is a substance that donates proton in solution while…

Q: Determine the pH of a 0.10 molL-1 solution of carbonic acid, H2CO3 HCO3 (aq) H20() = CO3²(aq) +…

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

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (C6H8O7)?   C6H8O7(aq) +…

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Q: Calculate the pH for a 0.0183 M pyrophosphoric acid solution (H4P2O7).  Pyrophosphoric acid has…

A: Pyrophosphoric acid has three dissociable protons. The dissociation reactions are as follows:…

Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: Which of the following is the pH of a solution with [H3O+] = 1.0 x 10-9? Select one: a. 1.00 b.…

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Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: Calculate the pH of a 0.0076 M solution of acetic acid, CH3COOH. The Ka of acetiç acid = 1.8 x 10-5.…

A: Kaa of acetic acid = 1.8× 10- 5  initial concentration of acetic acid = 0.0076 M

Q: Calculate the pH for a 0.0183 M pyrophosphoric acid solution (H4P2O7).  Pyrophosphoric acid has…

A: pH is the hydrogen ion concentration present in the solution. It is calculated by taking the…

Q: A weak base has K, = 2.4 x 10-4 at 25°C. By adding a strong acid to solution, there is an acid-base…

A: Weak base = B Kb = 2.4×10-4

Q: Determine the pH of a 1.30 M solution of CH3COOK. Ka(CH3COOH) = 1.8×10-5 Express your answer to

A: 1- First Calculate the OH- ion concentration :  CH3COO- + H2O <------> CH3COOH + OH-   The…

Q: Find the ph and the percent hydrolysis of a 0.0335 M solution of pyridine hydrochloride (the salt of…

A: Given : Concentration = 0.0335M

Q: Calculate the pH of 0.30 M methylamine, CH3NH2, which has a Kb of 4.4 x 10-4.

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Q: Calculate the pH of each of the following solutions at 25°C. 0.135 M HONH2 (Kb = 1.1 x 10-8) 0.135…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: The pH of a 0.65 M solution of acrylic acid (HC, H,CO,) is measured to be 2.22. Calculate the acid…

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Q: Calculate the pH of 0.389 M KHA solution. (Kal -5.3 x 10-6, K2 = 5.8 x 10-10 for H2A) Please keep…

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Q: Calculate the pH of a 10 M C5H5NHCI (aq) (pyridine chloride salt of pyridine) at 25 °C. The base…

A: Concentration of C5H5NHCl= 10M Kb=1.7×10^-9

Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…

A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…

Q: 1. Acetic acid at 1.80 M concentration partially dissociates in water with dissociation constant of…

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

Q: Calculate the pH of a solution (aq., 25 oC) prepared by dissolving 23.632 g of solid methylammonium…

A: Given: Mass of CH3NH3Cl = 23.632 g Molar mass of CH3NH3Cl = 67.518 g/mol Molarity of CH3NH2 = 1.10 M…

Q: Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5.  Calculate the equilibrium…

A: Given : Initial concentration of HN3 = 0.0750 M Since HN3 is a weak acid. Hence it will dissociate…

Q: Calculate the pH of a 0.094 M solution of formic acid, H2CO2. The Ka of formic acid 4 x 10-4 Submit…

A: In case of weak acids , the H+ ion concentration is given by the following formula  [H+] = (Ka×C)1/2…

Q: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa + log ([A–]/[HA])…

A: The Henderson-Hasselbalch equation for the reaction can be written as :  pH = pKa +log[salt][acid]…

Q: The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5).What is the pH of a 0.258 M…

A: 1) Given: Concentration of C6H5COOK = 0.258 M The hydrolysis reaction of C6H5COO- coming from…

Q: What is the pH of a 0.350 M solution of lithium citrate? (Ka Citric Acid = 7.4 x 10-4) I am only…

A: pH generally known as power of hydronium ion,  it tells the solution is acidic or basic .

Q: find the  pH of a 0.00250 M solution of dimethylamine, (CH3)2NH? : Atoms First.  The ionization…

A: pH is used to determine the concentration of hydronium ion.

Q: What is the pH of an aqueous solution at 25.0 °C in which [OH−] is 0.0050 M? A. 11.70 B. -2.30 C.…

A: The pH of any solution is given by  pH = -log[H+] = 14 + log[OH-]  where [OH-] = concentration of…

Q: The base protonation constant K, of lidocaine (C„H2,NONH) is 1.15 × 10 °. 14 Calculate the pH of a…

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Q: Calculate the pOH of the following solutions: (i) 8.24 x 10-3M KOH (ii) 3.98 x 10-2 M Mg(OH)2 A.…

A: Solution (i) pOH = -log[OH-] Since KOH shows 100% dissociation [OH-] = Molarity of KOH = 8.24 x…

Q: The pH of an aqueous solution of sulfurous acid, H2SO3, that has a concentration of 0.60 mol/L and…

A: The solution is as follows:

Q: Sodium bisulfate, NaHSO4, is used in some household cleansers as a source of HSO4- ion, a weak acid.…

A: [HSO4- ] = 0.75 M HSO4-1+ H2O ------> SO42- + H3O+

Q: Calculate the pH of the solution formed when 34.80 mL of 0.0270 M NaOH is added to 43.10 mL of…

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Q: Calculate the pH of the solution formed when 0.00 mL of 0.0440 M NaOH is added to 48.20 mL of 0.0440…

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Q: Acetic acid (CH, COOH, K, = 1.80 x 10-5) is a weak acid, so the salt sodium acetate (CH,COONA) acts…

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Q: Calculate the pH of a 0.20 M C2H5NH2 solution. Kb=5.6x10-4

A: C2H5NH2 is a weak base. pH of this solution  = 12.04

Q: Calculate the pH and % dissociation of a 0.100 M solution of propanoic acid (HC3H5O2). K,= 1.3x10-5…

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

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.