What concentration of an aqueous solution of NH4+ has the same pH as that of 6.8 × 10–5 M HCl? The pKb of NH3 is 4.74

Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

Q: CH₂NH₂ is a weak base (K₁ = 5.0 x 10-4), so the salt CH₂NH₂NO3 acts as a weak acid. What is the pH…

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Q: Calculate the pH of a 5.3 x 10-3-M solution of H2S04 (Ka, = 1.2 x 10-2). pH =

A: Given-> Concentration of H2SO4 = 5.3 × 10-3 M

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

A:

Q: What is the hydroxide-ion concentration in a 0.10 M solution of Na2CO3? For carbonic acid, Ka1 = 4.2…

A: Given,  Thr hydroxide-ion concentration in a 0.10 M solution of Na2CO3 is: For carbonic acid,…

Q: What concentration of oxalic acid, HOOCCOOH(H2A), will have a pH of 2.50 (pKa1 = 1.25; pKa2 = 4.14)?

A: Given:pH = 2.5pKa1 = 1.25pka2 = 4.14The pH of a solution is determined using the negative logarithm…

Q: What concentration of oxalic acid, HOOCCOOH(H2A), will have a pH of 50 (pKa1 = 1.25; pKa2 = 4.14)?

A: Given:pH = 50pKa1 = 1.25pka2 = 4.14The pH of a solution is determined using the negative logarithm…

Q: Calculate the pH at 25 °C of a 0.81M solution of potassium acetate (KCH3CO₂). Note that acetic acid…

A: Acetic acid pKa = 4.76Acetate pKb = pKw - pKaAcetate pKb = 14.0 - 4.76Acetate pKb = 9.24Kb =…

Q: What is the pH of a 0.190 M C6H5CO2H M solution if the K₂ of C6H5CO2H is 6.5 x 10-5?

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Q: a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; +…

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Q: What is the pH of a 0.290 M solution of aniline (C6H5NH2, Kb = 4.3 x 10-10)?

A: In the given question we have to calculate the pH of Aniline. concentration of Aniline = 0.290 M  Kb…

Q: Given are the following acid and base: Ca(OH)2 (aq)  + H2SO4 (aq) ---->  What is the major product…

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Q: The OH concentration in an aqueous solution at 25 °C is 3.1 x 103. What is [H*]?

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Q: 1. Which of the following solutions are acidic? Which are basic? Distilled H2O NaCl NH4Cl NaCH3COO…

A: Salt of strong acid and strong base is neutral  Salt of strong acid weak base is acidic  Salt of…

Q: Calculate the pH of a 0.0058 M solution of ascorbic acid (a weak acid).  Ka = 7.9×10-5 Express your…

A: Ascorbic acid is an weak monoprotic acid.

Q: Calculate the pH of a 6.9 × 10¬³-M solution of H2SO4 ( -3

A: The pH is used to determine the acidity or alkalinity of a solution. Molarity of a solution is used…

Q: What is the pH of a 0.01 M CH3COOH solution? (Ka= 1.74 x 10-5)

A: Given that  Ka of Ch3COOH is 1.74× 10^-5    Concentration of Ch3COOH is 0.01M

Q: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

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Q: What is the concentration of K+ ions in a 0.045 M K2CO3 solution assuming complete dissociation?…

A: Given: Concentration of K2CO3 = 0.045 M

Q: equilibrium constant, K, for this reaction.

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Q: The Ka of a weak acid is 3.33 x 10-5, what is the pKb of it's conjugate base?

A: The objective of this question is to calculate the pKb of the conjugate base of a weak acid given…

Q: What was the original 1. concentration (M) of an aqueous acetic acid (CH3COOH) solution whose pH is…

A:

Q: What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is…

A: Concentration of KOH solution as 0.0125 M at 100 °C

Q: Given are the following acid and base: Cа(ОН)2 (аq) + Н2SO4 (aq) ----> What is the major product of…

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Q: Calculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+ , in a 0.10 M…

A: Pyridine is a weak base which dissolves in water, dissociates partially into ions. The ions will be…

Q: Complete the balanced chemical reaction for the following weak base with a strong acid. In this…

A: In this question, we will complete the following Reaction and balanced the chemical reaction.  You…

Q: needs from the soil if its pH is above 6.5. (a) The hydrogen ion concentration of a soil sample is…

A: A) [H+] =1.58×10-7 pH = -log([H+])  = -log(1.58×10-7) = 6.8 So, pH = 6.8

Q: Calculate the pH of a 0.591 M aqueous solution of benzoic acid (CH₂COOH, K₂ = 6.3x10-5). pH =

A: Here,concentration of benzoic acid = 0.591 MKa = 6.3×10-5We have to find out pH.. Herw first we need…

Q: What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when…

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Q: Determine the pH of a 1.2 M solution of ammonia, NH3, with K 1.8 x 105

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Q: The value of K₂ for nitrous acid is 4.50×10-4. What is the value of Ko, for its conjugate base, NO₂?…

A: Since you posted multiple type question, then according to the guideline, post first solution for…

Q: Aspirin (acetylsalicylic acid, C9 HgO4) is a weak monoprotic acid. To determine its…

A: Solution:- Given - Aspirin (C9H8O4) is a monoprotic acid. 2.00 g of it dissolved in 0.600 L of…

Q: Based on the Lewis structures of the reactants and product of the following equation, identify the…

A: The compounds which has lone pair of electron to donate is called Lewis base and the compound which…

Q: What is the pH of a 1.00 M solution of Na2CO3? Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11

A: The objective of this question is to calculate the pH of a 1.00 M solution of Na2CO3. The…

Q: The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving…

A: Acid is compound that dissociates in water to give H+ ions

Q: What is the pH of a 0.02 M solution of acetic acid (pKa = 4.84)?

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Q: b. An aqueous acetic acid (HOAC) solution is 1.00 % dissociated. What will the concentration of H30+…

A: • With the help of given value of amount  of Sodium Acetate (NaOAc) i.e. 0.82 gms.,  we can…

Q: The pKa of a particular weak acid is 4.85. What is the pH of the weak acid solution when exactly…

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Q: Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid,…

A: According to the Brønsted-Lowry concept :-  An acid is a proton donor  A base is a proton acceptor

Q: A diprotic acid (H₂A) has Kal = 4.54 x 10-7 and K₁2 = 5.59 x 10-11. What is the pH of a 0.396 M H₂A…

A: we have to calculate the pH of 0 .396 M diprotic weak acid

Q: Consider a weak acid "HA". What is the pH of a 0.957 mol L-1 solution of HA? The KA of HA is 7.09 x…

A: The acid dissociation constant for the HA is = 7.09×10-7 The concentration of HCN solution is =…

Q: 2- Suppose a 0.13M aqueous solution of oxalic acid (H2C2O4) is prepared. Calculate the equilibrium…

A: Step 1: Oxalic acid (H2C2O4) is a diprotic acid. It can donate up to two protons. When it…

Q: Calculate the pH of a 0.597 M solution of chloroacetic acid (CICH;CO,H, K, = 1.36 x 10-3).

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Q: Fill in the left side of this equilibrium constant equation for the reaction of trimethylamine…

A: Answer: When a weak base is added into the water, it dissociated partially and an equilibrium is…

Q: Suppose a 0.018M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium…

A: Step 1:[H3PO4] = 0.018 M[HPO42-] = ?Ka1 = 7.5 * 10-3 Ka2 = 6.2 * 10-8 Step 2: First…

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.