Fill in the missing formuias below.AcidConjugate BaseНСОЗНРОДНРО, 2-

According to Bronsted-Lowry theory of acids and bases a conjugate acid and base pairs are species…

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Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 32QAP

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The formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why.
Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?
For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.
Ammonia can react as an acid or a base. a) What is the conjugate acid of ammonia? b) What is the conjugate base of ammonia? c) arist dit ons servbed as Complete the following acid-base reaction in which NH3(e) acts as both an acid and a base: OcH 6 HOONH3() + NH3() = OOH (d FOZH (s *АНИ (1 sqz ions to biosqu adtavið
8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)
3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
Is H2Cr2O2 an acid, base, or neutral? please justify your answer with an equation showing its dissociation.
(a) Hydrogen peroxide, H2O2, is a Brønsted Lowry acid. It is used as an antiseptic and bleaching agent. Write the formula for the conjugate base of hydrogen peroxide. (b) Hydrazine, N2H4, is a Brønsted-Lowry base used as a rocket fuel. Write the formula for the conjugate acid of hydrazine. (c) Phenol, HOC6H5, is a Brønsted-Lowry acid used to make plastics, nylon, and slimicides. Write the formula for its conjugate base. (d) Aniline, C6H5NH2, is a Brønsted-Lowry base used to make polyurethane. Write the formula for its conjugate acid.
What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.
Given that pKa = 3.14 at 25 deg C for HNO2, what is the pH of 0.173 mol L-1 NaNO2(aq) at 25 \deg C? What is the equilibrium concentration of HNO2? pH = Number (Give your answer accurate to 2 decimal places.) [HNO2]eq = Number mol L-1 (Give your answer accurate to 2 signficant figures.)
If the Kb for hydrazine, N2H4(aq), is 1.7 x 10-6 , calculate the pH of a 1.8 mol/L solution of hydrazine.

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Fill in the missing formuias below. Acid Conjugate Base НСОЗ НРОД НРО, 2-