Explain how ammonia can act as both an acid and a base. Which of these roles does it commonly fill in aqueous solutions?

Q: Explain Acid Strength and Molecular Structure?

A: Acidic strength is the measurement of ability of an acid to lose its H+ ions. It has further…

Q: What is the strongest base that can exist in liquid ammonia as a solvent?

A: Strongest base that can exist in liquid ammonia as a solvent.

Q: Which of these may be classified as a Lewis base? O Fe O Zn2+ O CO2 O CH3NH2

A: CH3NH2 is lewis base.

Q: What substances remain undissolved by the acid and alkali

A: ANSWER IS DISCUSSED BELOW

Q: Malonic acid (Ka1 = 1.42 x 10–3, Ka2 = 2.01 x 10–6) can exist as one of the 3 forms shown below.…

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Q: Calculate the concentration of OH− and the pH for a 0.15 M aqueous solution of morphine (C17H19NO3,…

A: Recall the following relation to calculate pOH and pH of the given morphine solution…

Q: Write an equation for the proton-transfer reaction between a phosphate ion (PO43–) and water, and…

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Q: Why does the concentration of H3O+ and OH- equal each other in neutral water?

A: pH = -log[H3O+]   [OH-].[H3O+]  = kw  Kw = 1.0 × 10-14 M2

Q: The reaction of ammonia with copper(II) ions is an example of a Lewis Acid–Lewis Base reaction.…

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Q: Which one of the following is more acidic and why? ОН OH NO2 NH2

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Q: a net ionic equation to show that morphine, C17H19O3N, behaves as a Bronsted-Lowry base in water.

A: Since in morphine we have N with lone pair present in it Hence it will react with water and produce…

Q: What is the pH of .03 M NH4Br (aq)? O 3.13 O 9.25 O 10.87 O 1.52 O 5.38

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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: OH OH (i) (ii) O= O= 0=

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Q: Which compound of each of the following pairs is the STRONGER BASE? (A) (B) O Option A Option B…

A: On going from left to right along a period, the basicity of MO32- species decreses. More…

Q: .Write a balanced equation for the dissociation of each of the following Bronsted- Lowry acids in…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: Draw the Lewis structure of PF3 and PI3.  Determine which statement best describes the Lewis acid or…

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Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: What is the pH of 7.8 x 105 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 O 3.7 O 4.1

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Q: Suppose .0274 g of HCIO4 is dissolved in 425 mL of aqueous solution. What is the pH? O 4.19 O 1.19 O…

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Q: Identify the Lewis acid in the following reaction. FeBr3 Br2 FeBr4 Br I3D II IV

A: Lewis acid is the species,  that accepts electron pair. And form ionic species.

Q: Nitric acid reacts with ammonia to yield ammonium nitrate. Write the reaction and identify the acid,…

A: Given here, Nitric acid reacts with ammonia to yield ammonium nitrate and we are asked to write the…

Q: 1. Methanoic acid, HCO,H, also known as formic acid, is partly responsible for the characteristic…

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Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: Use Le Chatelier's Principle to qualitatively determine what the pH of a 0.2 M NH4Cl would be…

A: Le Chatelier's Principle :  At equilibrium the change in any property like, temperature,pressure and…

Q: Which is the strongest acid of the following? A)HClO3 B)HClO2 C)HBrO D)HIO

A: In case of oxyacids, increase in oxidation number of a particular halogen atom increases the acidic…

Q: How do I write the chemical equation for the reaction of NaOH and HC2H3O2?

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Q: 1 You are presented with a solution that has a pOH of 2.13,What is the pH of this solution? O 11.87…

A: The pOH of the solution is = 2.13 The pH of the solution is =?

Q: what is the formula of the conjugate acid of SO32-

A: Given species: SO32- We have to write the formula of the conjugate acid of SO32-.

Q: Write the products of the following acid-base reaction. CH3OH NaNH2 ?

A: The reactants given are  1) CH3OH  2) NaNH2

Q: Write a net ionic equation to show how ammonia behaves as a base in water. + H2O

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Q: What are three possible sources of error in the Determination of Ionization Constant of Acetic Acid…

A: An acid ionization constant (Ka) is the equilibrium constant for the ionization of an acid. The…

Q: Write the reaction that occurs, and identify the conjugate acid-base pairs of the following…

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Q: How can we describe the acid-base interaction in terms of boundary orbitals?

A: When any reaction occurs between two reactants, the reaction occurs between HOMO(Highest occupied…

Q: Which of the following is a BrØnsted-Lowry acid? O C Cl 4 Ο ΝΗ O PH, Ο ΝΗ5 O Br 2

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Q: Write the formula of the conjugate acid of the Brønsted-Lowry base, C₄H₃N₂O₃⁻ ?

A: If we add H+ in base then it will convert into conjugate acid   C₄H₃N₂O₃⁻ +H+= C4H4N2O3

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 pH of a 0.0670 M solution of methylamine (CH3NH2, Kb = 4.4 x 104)? %3D

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Q: Organic molecules often have polar covalent bonds. How does this provide opportunities for chemical…

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Q: What is the pH of 1.75 M NH3 (aq)? O 9.50 O 4.50 O 4.74 O 2.25 Ο 11.75

A: Solution :

Q: Write an equation to show how HC204 can act as an acid with HS¯ acting as a base.

A: Bronsted-Lowery acid base theory :   Bronsed acid : Proton (H +) donar is acid  Bronsted base :…

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: What effect does element size have on acidity?

A: There is significant effect of element size on acidity. With increasing size of atom acidity…

Q: In the following reaction, identify the Lewis acid. Co** (ag) + 6NH3 (ag) - Co(NH3),**(aq)

A: Lewis acid is an electron-pair acceptor. That is Lewis acid is any substance which can accept a pair…

Q: Arrange the Lewis acids GaCl3, BCl3 en AlCl3 in order of increasing acidity.

A: The substance which can accept a pair of non-bonding electrons are called Lewis acids or we can say…

Q: The Lewis acidities of silicon halides follow the order SiI4< SiBr4<SiCl4< SiF4. Explain.

A: The Lewis acidities of silicon halides follows the order, SiI4 &lt;  SiBr4 &lt; SiCl4 &lt; SiF4.

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitri acid and sodium…

A: The explanation is given below-

Q: Which of the following is a Lewis base? A) CO2 B) BF3 C) NH3 D) NO2

A: Lewis base is the substance which have tendency to donate lone pair of electron.

Q: One aqueous solution of a strong acid has pH = 1.20, another pH = 1.80. If equal volumes of these…

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Q: The conjugate acid of H2O is

A: Conjugate acid is a chemical species same as original species combined with H+ ion.  In general, a…

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates). 

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.