Why is (CH3)3Cl considered to be a Lewis Acid?

Q: What is the pH of a 0.55 M solution of (CH3)3N?

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Q: Which is a stronger acid, H2O or H2S?

A: According to Arrhenius theory an acid is the substance which gives H+ ions when dissolved in water.…

Q: Which is the stronger acid, NH4+ or HBrO?

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Q: What is the pH of a 0.710 M solution of C5H5NHB (Kb of C5H5N is 1.7 x 10-9)?

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

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: Write the chemical reaction for the conversion of CO2 to HCO3-, including the enzyme that catalyzes…

A: The chemical reaction involved in the conversion of CO2 to HCO3- is, CO2 + H2O <=> H2CO3…

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: which is the MOST acidic hydrogen? II I III IV

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Q: Which is the stronger acid, NaHSO3 or NaHSO4?

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Q: What is the pH of a 7.7 × 10⁻⁴ M HClO₄ solution?

A: The HClO4 is a strong acid and it fully dissociates in water as H+ and ClO4- So the concentration of…

Q: What is the pH of a 0.050M solution of (CH3)3NHC1?

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Q: What is the pH of a 0.0037 M solution of H2CO3?

A: pH is a negative logarithm of the concentration of H+ ions. A pH scale is used to measure the…

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What is the pH of 1.5M solution of H2SO4?

A: pH is a measure of strength of H+ ion concentration in a solution. It can be calculated as: pH  =…

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: When a solution is prepared by dissolving one pellet of KOH weighing 128 mg in 500 ml of dH2O…

A: Mass of KOH = 128 mg1mg = 10-3 gMass of KOH = 0.128 gMolar Mass of KOH = 56.1 g/molMoles of KOH =…

Q: What is the pH of a 0.22M NaH2PO4 solution?

A: NaH2PO4 is a weak.Ka for NaH2PO4 is 6.23×10-8.Calculate concentration of H3O+:

Q: Calculate pH of a 0.1 M solution of AlCl3.

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Q: What is the pH of a 0.193 M w. acid HA solution? Ka = 6.61 x 10−6?

A: The acid is weak so it weakly dissociates in the solution. That is it gives an H+ ions slowly in to…

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: What are the [H,O*| and [OH] of Diet Coke that has a pH of 3.17? ()

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Q: What is the pH of a 0.870 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Answer:- This question is answered by using the simple concept of hydrolysis of the salt formed by…

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

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Q: Calculate the pH of a 0.20 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

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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: What is the pH of a 0.600 M solution of Na2S?

A: In this question, we want to determine the pH of the salt solution ( Na2S ) How we can calculate,…

Q: What is the pH of a 0.650 M solution of C5H;NHB (Kb of CsH;N is 1.7 × 10-º)?

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Q: -NH2 но NH b. OH

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Q: Which one of the following is more acidic? CO2H CO,H а) b) NO2 ОН NH2 c) d) i. b

A: Acidity is defined as the ability of a molecule to release protons.  if a compound  easily donate…

Q: What is the pH of a 2.7 × 10⁻⁴ M HClO₄ solution?

A: The question is based on the concept of PH calculations. we have been given perchloric acid. We have…

Q: What is the pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

A: Given,  The pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

Q: What is the pH of a 0.660 M solution of C3H;NHB (Kb of C5H5N is 1.7 x 10-9)?

A: Given information, [C5H5NHBr] = 0.660 M Kb of C5H5N = 1.7*10-9 Calculate: pH = ?

Q: What is the pH of a 6.7 × 10⁻⁴ M HClO₄ solution?

A: Consider the dissociation of HClO₄ in water is as follows;      It is given that one molecule of…

Q: What is the pH of a 0.40 M solution of K₂SO3?

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Q: Calculate the pH of a 0.1M solution of protonated methylamine (pKa =7)

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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: Arrange the following in order of INCREASING acidity. I. II. II. IV. ... CI CI OH OH CI CI

A: Correct option is • B    I < III < Iv < II Acidiity depends on the conjugate base…

Q: Based on the pH measured for the solution of (NH4)2CO3, is NH4+ is a stronger acid or is CO2−3…

A: Given: To determine whether (NH4)2CO3  is strong acid or strong base.   Definition: (NH4)2CO3 is…

Q: What is the conjugate acid of potassium hydrogen phosphate, K2HPO4?

A: K2HPO4 is a base. Its conjugate acid can be obtained by adding a hydrogen atom to it. The net ionic…

Q: Explain protonation of HNO3 ?

A: The protonation of HNO3 has to be explained below.

Q: Give the formula of the conjugate acide of H2O ?

A: Conjugate acid, according to Bronsted-Lowry-acid-base theory, is chemical compound that is formed…

Q: Deionized water at 10c  in which Kw = 2.89e-15 , pkw= 14.539  what is the pH , poH , [OH], [H3O+]?

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Q: Arrange according to decreasing acidity .cO,H .CO2H .COH CH3 ČI C A В C>A>B C>B>A B>A>C B>C>A

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Q: What is the pH of a 0.500 M solution of trimethylamine (pKb = 4.13)?

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Q: What are the pH, pOH and [H3O]+ for a 2.37 x 10-2M HClO4 solution? HClO4 is a strong mineral acid.

A: Given Data

Q: What is the pH of a 2.12.1 M solution of HClO4?

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Q: The pH for 0.0850 M solution of C6H5CH2COOH is 2.68. Determine the value of Ka for C6H5CH2COOH.

A: Given pH of C6H5CH2COOH is = 2.68. We Know, pH = - log[H3O+] So, 2.68 = - log[H3O+] Or, log[H3O+] =…

Q: Which is the stronger acid, H2SO4 or H2SeO4? Why?

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Q: Write an expression for the equilibrium constant  for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)

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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.