Reacting GeO2 with H20 forms the tetraprotic (four H* ions) acid, H4GEO4. On a piece of paper, write down the chemical equations for the four acid dissociation equilibria. Match each chemical species below with its correct role in this polyprotic acid system. H4GEO4 v [ Choose ] the conjugate acid of H3GEO4 - this species' conjugate acid is HGEO4 3- the acid in the second H+ dissociation H3GEO4 - the conjugate base in the third H+ dissociation the conjugate base of H3GE04 - H2GEO4 2- [ Choose ] HGEO4 3- [Choose] GeO4 4- [Choose]

Reacting GeO2 with H20 forms the tetraprotic (four H* ions) acid, H4GEO4. On a piece of paper, write down the chemical equations for the four acid dissociation equilibria. Match each chemical species below with its correct role in this polyprotic acid system. H4GEO4 v [ Choose ] the conjugate acid of H3GEO4 - this species' conjugate acid is HGEO4 3- the acid in the second H+ dissociation H3GEO4 - the conjugate base in the third H+ dissociation the conjugate base of H3GE04 - H2GEO4 2- [ Choose ] HGEO4 3- [Choose] GeO4 4- [Choose]

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section4.6: Molecular Structure And Acidity

Problem 1Q: Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity,...

See similar textbooks

Similar questions

I need help with this problem. Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM using the "Arrhenius Concept". Include:a balanced equation describing the acid-base reactions involvedThe calculation of the pKa for bothThe calculation of the two pH's (of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM)and A calculation of the percent of dissociation of both propionic acid and nitric acid.The gibbs free energy ΔG are listed as the following:Nitric acid: -152 kJ/molPropionic Acid : -291 kJ/molPropionate: -361 kJ/mol
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 × 10-4 and Ka2 = 9.0 × 10-5.a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2 . Write the chemical equation that represents Ka1 × Ka2. b Qualitatively describe the relative concentrations of H2A, HA-, A2-, and H3 O+ in a solution that is about one molar in malic acid.c Calculate the pH of a 0.0175 M malic acid solution and the equilibriumconcentration of [H2 A].d What is the A2- concentrationin in solutions b and c?
Reacting GeO2 with H2O forms the tetraprotic (four H+ ions) acid, H4GeO4. write down the chemical equations for the four acid dissociation equilibria. Match each chemical species below with its correct role in this polyprotic acid system. H4GeO4 H3GeO4 - H2GeO4 2- HGeO4 3- GeO4 4- Answer Choices: the conjugate base in the third H+ dissociation the acid in the second H+ dissociation the conjugate base of H3GeO4 - this species' conjugate acid is HGeO4 3- the conjugate acid of H3GeO4 -
Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+1aq2 as a product and then with the hydronium ion: (a) C6H5COOH, (b) HCO3 -.
If enough of a monoprotic acid is dissolved in water to produce a 0.0124 M solution with a pH of 6.72, what is the equilibrium constant, p?a, for the acid? kindly consider the following when answering the question For weak acids that are so dilute or so weak that the pH of the solution lies between 6 and 7, the autoprotolysis of water must be taken into account when determining the p?a value. At equilibrium, there are four species in solution, the weak acid, HA, its conjugate, A−, H3O+, and OH−. Start by developing four equations that describe what is occurring in the solution at equilibrium.
1. Arrange the following in order of increasing pH of their corresponding solutions. a. CH3NH3Cl, NaCH3COO, RbBr b. K2C2O4, C2H5NH3Br, Ba(ClO4)2 2. Oleic acid (which can be denoted as HOL), is a weak acid. Considering its sodium salt, sodium oleate (NaOL), calculate the pKa of HOL given that a 0.100 M solution of NaOL has a pH of 9.01. (hint: Kw=Ka * Kb).
Bronsted-Lowry acid/base strengths are dictated by the proton donor/acceptor propertiesof the reaction media. With this in mind, write out chemical reactions emphasizingproton transfers occurring in the following processes:a) Phosphoric acid (H3PO4) functions as base in concentrated H2SO4. b) Perchloric acid (HClO4) and nitric acid (HNO3) are both strong acids in water. In glacialacetic acid HClO4 functions as a strong acid whereas HNO3 is substantially weaker. c) Oxalic acid (HOOC-COOH) is a weak acid in water (Ka1 = 5.6×10-2; Ka2 = 1.5×10-4). Itbehaves as a strong monoprotic acid in liquid ammonia. d) Hydrogen fluoride (H-F) functions as a base in liquid anhydrous HClO4.
Selenic acid, H2SeO4, is a diprotic acid that actually is a strong acid for the donation of its first proton and has a pKa2 = 1.7. What will be the Ka and the chemical equation for showing the donation of the second proton? (hint: products will be H3O+ and SeO42-) I take 2.00 g the pure compound and dilute it to 100.0 mL of solution. Find the initial concentration and use two ICE tables to show the equilibrium concentrations of [H3O+], [OH-], [HSeO42-] and [SeO42-]. What will be the concentration of H2SeO4? (hint: no math is necessary here as this is a strong acid).
HIn(aq) + H2O(l) H3O+(aq) + In-(aq)red yellowThe acid base indicator methyl orange is red at pH values below 3 and is yellow at pH values above 6. Usingyour knowledge of pH, indicators and pKa values, predict the pKa of methyl orange.
Acidified potassium bromate(V), KBrO3, reacts with hydrogen sulfide, H2S, to give a yellow solid and an orange solution. On shaking the solution with trichloroethane, the trichloroethane layer turned orange-red. (a) Suggest the identity of yellow solid and the orange solution. Describe the type of reaction taking place. (b) Construct a balanced equation for the reaction between KBrO3 and H2S. (C) BrO3- is the conjugate base of HBrO3. Draw the dot and cross structure of HBrO3. (d) HBr is a stronger acid than HCl. However, HBrO3 is a weaker acid than HCIO3. Explain the difference in acidities.
Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25? For the best choice, calculate the ratio of the conjugate base to the acid required to attain the desired pH.chlorous acid (HClO2) pKa = 1.95 formic acid (HCHO2) pKa = 3.74nitrous acid (HNO2) pKa = 3.34 hypochlorous acid (HClO) pKa = 7.54
it is stated that alkyl halides (such as n-butyl bromide, sec-butyl bromide, tert-butyl chloride, benzyl chloride, and bromobenzene) make a carbocation and the halide, before the halide reacts with the silver.(1% ethanolic silver nitrate solution) Explain why this is wrong and the actual role of the Ag+ ion as a Lewis acid