The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the majorspecies present at equilibrium. You can leave out water itself.Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases inthe 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row.You will find it useful to keep in mind that NH, is a weak base.acids: O0.11 mol of HCI is added to1.0 L of a 1.0M NH3bases: 0solution.other: O0.44 mol of NAOH is addedacids: Oto 1.0 L of a solution that is1.1M in both NH, andbases: ONH,CI.O other: O

Weak electrolytes are those which do not dissociate completely in its solution. There exists an…

Answered: acids: O 0.11 mol of HCI is added to…

acids: O 0.11 mol of HCI is added to 1.0 L of a 1.0M NH, bases: U solution. other: O 0.44 mol of NaOH is added acids: U to 1.0 L of a solution that is 1.1M in both NH, and bases: U NH CI. O other: U

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 17STP

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The reaction just described is reversible. Deprotonation of the conjugate acid of an organic base by water provides another example of simultaneous making and breaking of sigma bonds. Thus, in the deprotonation of anilinium ion by water, the base is water, which has unshared electrons on the ________ atom. The acid is ________ ion. A pair of ________ electrons on the oxygen atom of water is pushed toward the ________ atom. Simultaneously, the pair of ________ electrons between the hydrogen and ________ atom of the anilinium ion is pushed toward the ________ atom. Thus, the oxygen- ________ sigma bond is made and a hydrogen- ________ sigma bond is broken. The nitrogen atom, which possessed a positive charge, is now ________, and the oxygen atom, which was neutral, now possesses a formal ________ charge.
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base.
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. 0.26 mol of HCl is added to 1.0L of a 1.2M NH3 solution. acids: bases: other: 0.06 mol of HBr is added to 1.0Lof a solution that is 0.2M in both NH3 and NH4Cl. acids: bases: other:
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. 0.5 mol of NaOH is added to 1.0L of a 0.5M HF solution. acids: bases: other: 0.076 mol of HI is added to 1.0L of a solution that is 1.3M in both HF and KF. acids: bases: other:
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row.You will find it useful to keep in mind that NH3is a weak base.
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCH3CO2 is a weak acid. 0.2 mol of KOH is added to 1.0Lof a 0.2M HCH3CO2 solution. acids: bases: other: 0.2 mol of HBr is added to 1.0L of a solution that is 0.7M in both HCH3CO2 and KCH3CO2. acids: bases: other:
Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. F- + H2CO3 (aq) ⇌ HF (aq) + HCO3- Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase Brønsted-Lowry _____acidbase In this reaction: The formula for the conjugate _____acidbase of F- is The formula for the conjugate _____acidbase of H2CO3 is
1. In each of the equations below, label the acids, bases and their conjugates. HCOOH + H2O ↔ HCOO- + H3O+ HPO42- + H2O ↔ H2PO4- + OH- NH3 + H2O ↔ OH- + NH4+ 2. Decide which of the following statements are True and which are False about equilibrium systems: A large value of K means the equilibrium position lies far to the left. For a reaction with K >> 1, the rate of the forward reaction is greater than the rate of the reverse reaction at equilibrium. For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are the same. For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression. The value of K at constant temperature does not depend on the amounts of reactants and products that are mixed together initially. 3. Given the following equilibrium constants at 427°C:…
HF is a weak acid, whose conjugate base is F-. Write the reaction that corresponds to Ka and Kb for the respective species. Write the equilibrium expression for each reaction.
dentify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCN (aq) + H2PO4- ⇌ CN- + H3PO4 (aq) Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate of HCN is The formula for the conjugate of H2PO4- is