6.1.3 revision guide carboxylic acids and esters
... withdraw electron density from the COO- ion, making it less negative and more stable. This make the acid more strong. ...
... withdraw electron density from the COO- ion, making it less negative and more stable. This make the acid more strong. ...
Acid Base PPT - mvhs
... The pH Scale The pH of a solution is defined as the negative of the common logarithm of the hydronium ion concentration. pH= -log [H3O+] The pOH of a solution is defined as the negative of the common logarithm of the hydroxide ion concentration. ...
... The pH Scale The pH of a solution is defined as the negative of the common logarithm of the hydronium ion concentration. pH= -log [H3O+] The pOH of a solution is defined as the negative of the common logarithm of the hydroxide ion concentration. ...
Ka or Kb - RangerCalculus
... EQUILIBRIUM REVIEW #2 (Ka/Kb) Ka or Kb Here are some things in common with most Ka/Kb problems. 1. Many of them will ask for you to determine pH or pOH. To do this, you obviously need to know [H+] or [OH-]. If you have a strong acid or strong base, you can determine [H+] or [OH-] directly from the a ...
... EQUILIBRIUM REVIEW #2 (Ka/Kb) Ka or Kb Here are some things in common with most Ka/Kb problems. 1. Many of them will ask for you to determine pH or pOH. To do this, you obviously need to know [H+] or [OH-]. If you have a strong acid or strong base, you can determine [H+] or [OH-] directly from the a ...
1 - Test Bank
... A) CH3CH2OH can be a Bronsted-Lowry acid. B) CH3CH2NH2 can be a Bronsted-Lowry base. C) CH3CH2OH can be a Lewis base. D) CH3CH2OH can be a Bronsted-Lowry acid, and CH3CH2NH2 can be a BronstedLowry base. E) CH3CH2OH can be a Bronsted-Lowry acid, CH3CH2NH2 can be a Bronsted-Lowry base, and CH3CH2OH ca ...
... A) CH3CH2OH can be a Bronsted-Lowry acid. B) CH3CH2NH2 can be a Bronsted-Lowry base. C) CH3CH2OH can be a Lewis base. D) CH3CH2OH can be a Bronsted-Lowry acid, and CH3CH2NH2 can be a BronstedLowry base. E) CH3CH2OH can be a Bronsted-Lowry acid, CH3CH2NH2 can be a Bronsted-Lowry base, and CH3CH2OH ca ...
Chapter 19 Summary - McGraw Hill Higher Education
... (a) 2-Hydroxypropanoic acid (better known as lactic acid, it is found in sour milk and is formed in the muscles during exercise) (b) 2-Hydroxy-2-phenylethanoic acid (also known as mandelic acid, it is obtained from plums, peaches, and other fruits) (c) Tetradecanoic acid (also known as myristic acid ...
... (a) 2-Hydroxypropanoic acid (better known as lactic acid, it is found in sour milk and is formed in the muscles during exercise) (b) 2-Hydroxy-2-phenylethanoic acid (also known as mandelic acid, it is obtained from plums, peaches, and other fruits) (c) Tetradecanoic acid (also known as myristic acid ...
The acidic environment – Acids
... 8. Round off the figures you see to an appropriate number of significant figures, e.g. because 0.0020 is to two significant figures, the pH answer should be given to two significant figures as 2.7. You are also expected to be able to work out [H+] if you are given pH. You will need to use a key mark ...
... 8. Round off the figures you see to an appropriate number of significant figures, e.g. because 0.0020 is to two significant figures, the pH answer should be given to two significant figures as 2.7. You are also expected to be able to work out [H+] if you are given pH. You will need to use a key mark ...
Chapter 11 Carboxylic Anhydrides, Esters, and Amides
... Anhydrides react with alcohols and phenols to give an ester and a carboxylic acid. ...
... Anhydrides react with alcohols and phenols to give an ester and a carboxylic acid. ...
u11_tqs
... 46. Strong acids ionize completely, while weak acids ionize only slightly in aqueous solution. 47. Strong acids have large Ka values; weak acids have small Ka values. 48. Strong bases dissociate into what two things, in aqueous solution? metal ions and hydroxide (i.e., OH–) ions 49. The smaller the ...
... 46. Strong acids ionize completely, while weak acids ionize only slightly in aqueous solution. 47. Strong acids have large Ka values; weak acids have small Ka values. 48. Strong bases dissociate into what two things, in aqueous solution? metal ions and hydroxide (i.e., OH–) ions 49. The smaller the ...
Acids, bases and ions in aqueous solution
... If a pure liquid partially dissociates into ions, it is selfionizing. Water itself is ionized to a very small extent (equation below) and the value of the self-ionization constant, Kw , shows that the equilibrium lies well to the left-hand side The self-ionization in equation 6.1 is also calle ...
... If a pure liquid partially dissociates into ions, it is selfionizing. Water itself is ionized to a very small extent (equation below) and the value of the self-ionization constant, Kw , shows that the equilibrium lies well to the left-hand side The self-ionization in equation 6.1 is also calle ...
Synthesis of n-Butyl Acetate via Esterification
... bumping. As an option, you might hold a thermometer just above the boiling liquid and note a temperature of about 91°C. Remove the thermometer and allow the reaction mixture to reflux in such a manner that the vapors condense about one-third of the way up the empty distilling column, which is functi ...
... bumping. As an option, you might hold a thermometer just above the boiling liquid and note a temperature of about 91°C. Remove the thermometer and allow the reaction mixture to reflux in such a manner that the vapors condense about one-third of the way up the empty distilling column, which is functi ...
Supplement AP Chemistry –
... obtain a buffer solution that has a pH of 7.49? Assume that the addition of solid NaOH results in a negligible change in volume. (e) Household bleach is made by dissolving chlorine gas in water, as represented below. Cl2 (g) + H2O H+ + Cl- + HOCl Calculate the pH of such a solution if the concentr ...
... obtain a buffer solution that has a pH of 7.49? Assume that the addition of solid NaOH results in a negligible change in volume. (e) Household bleach is made by dissolving chlorine gas in water, as represented below. Cl2 (g) + H2O H+ + Cl- + HOCl Calculate the pH of such a solution if the concentr ...
Analysing Acids and Bases
... Figure 4.4 pH curves showing change of pH during a titration of a a strong base with a strong acid, and b a weak base with a strong acid. Phenolphthalein, which changes colour in the pH range 8.2–10, gives a sharp end point in a but a broad end point in b. Methyl orange, which changes colour between ...
... Figure 4.4 pH curves showing change of pH during a titration of a a strong base with a strong acid, and b a weak base with a strong acid. Phenolphthalein, which changes colour in the pH range 8.2–10, gives a sharp end point in a but a broad end point in b. Methyl orange, which changes colour between ...
Chapter 11 Carboxylic Anhydrides, Esters, and Amides
... Anhydrides react with alcohols and phenols to give an ester and a carboxylic acid. ...
... Anhydrides react with alcohols and phenols to give an ester and a carboxylic acid. ...
Aspirin - Community Colleges of Spokane
... The functional groups you will study in this experiment are: (1) alcohols and phenols, (2) carboxylic acids, (3) esters, and (4) anhydrides. Alcohols are compounds that contain at least one hydroxyl group (-OH) attached directly to a carbon. Phenols are similar to alcohols, but the hydroxyl group is ...
... The functional groups you will study in this experiment are: (1) alcohols and phenols, (2) carboxylic acids, (3) esters, and (4) anhydrides. Alcohols are compounds that contain at least one hydroxyl group (-OH) attached directly to a carbon. Phenols are similar to alcohols, but the hydroxyl group is ...
Chem. 31 * 9/15 Lecture
... – Ka = [H+][A-]/[HA] = x2/(2.0 x 10-4 – x) x = 1.2 x 10-4 M (using quadratic equation) Note: sometimes (but not in this case), a 2nd assumption can be made that x << 2.0 x 10-4 to avoid needing to use the quadratic equation [H+] = [A-] = 1.2 x 10-4 M; pH = 3.92 [HA] = 2.0 x 10-4 – 1.2 x 10-4 = 8 x 1 ...
... – Ka = [H+][A-]/[HA] = x2/(2.0 x 10-4 – x) x = 1.2 x 10-4 M (using quadratic equation) Note: sometimes (but not in this case), a 2nd assumption can be made that x << 2.0 x 10-4 to avoid needing to use the quadratic equation [H+] = [A-] = 1.2 x 10-4 M; pH = 3.92 [HA] = 2.0 x 10-4 – 1.2 x 10-4 = 8 x 1 ...
chm238f02.pracexam2.ans
... (c) If we used only pure (fuming) sulfuric acid, what would be the product(s)? mostly sulfonation of Cl benzene, both o and p, because SO3H+ becomes the superelectrophile and there is not as much protons for the dehydration of nitric acid. (d) Chlorine is o,p directing group but chlorobenzene is slo ...
... (c) If we used only pure (fuming) sulfuric acid, what would be the product(s)? mostly sulfonation of Cl benzene, both o and p, because SO3H+ becomes the superelectrophile and there is not as much protons for the dehydration of nitric acid. (d) Chlorine is o,p directing group but chlorobenzene is slo ...
Computational Docking Experiments to Find a Ligand that Will Bind
... kcal/mol and is positioned significantly different than the original ligand (Fig. 4D). However, the Carboxylic Acid #8 (derivative) has a significantly higher affinity value (-6.7 kcal/mol) than the allopurinol and is positioned just slightly different from the original ligand. This suggests that Ca ...
... kcal/mol and is positioned significantly different than the original ligand (Fig. 4D). However, the Carboxylic Acid #8 (derivative) has a significantly higher affinity value (-6.7 kcal/mol) than the allopurinol and is positioned just slightly different from the original ligand. This suggests that Ca ...
The "pH Factor"
... broken down, it leaves certain chemical and metallic residues, a noncombustible "ash" which, when combined with our body fluids, yields either acid or alkali potentials of pH. Certain foods are "acidforming" in nature, whereas others are known to be "alkali-forming." Which Foods Are "Acid-Forming" A ...
... broken down, it leaves certain chemical and metallic residues, a noncombustible "ash" which, when combined with our body fluids, yields either acid or alkali potentials of pH. Certain foods are "acidforming" in nature, whereas others are known to be "alkali-forming." Which Foods Are "Acid-Forming" A ...
1-13 acids esters fats
... This reaction has a double arrow. The reason is that organic acids are weak acids and form an equilibrium in a solution. Only a small percentage of the acids give up their hydrogen. Once the equilibrium has been reached the concentration of acid, hydrogen ion and anion remain constant. In the above ...
... This reaction has a double arrow. The reason is that organic acids are weak acids and form an equilibrium in a solution. Only a small percentage of the acids give up their hydrogen. Once the equilibrium has been reached the concentration of acid, hydrogen ion and anion remain constant. In the above ...
Synthesis of Benzene Derivatives: Electrophilic Aromatic Substitution
... Fuming sulfuric acid (8% SO3 in concentrated H2SO4) reacts with benzene to form benzenesulfonic acid. ...
... Fuming sulfuric acid (8% SO3 in concentrated H2SO4) reacts with benzene to form benzenesulfonic acid. ...
Chemistry Honors: Lesson 6 Acids and Bases Definitions 1
... HA + H2O <===> H3O+ + AThe acid dissociation constant, Ka, is a measure of the how much the acid dissociates. Ka = [H30+][A-]/[HA] Similarly, a weak monovalent base, BOH, dissociates to give B+ and OH-. The base dissociation constant, Kb, is a measure of the degree that the base dissociates. Kb = [B ...
... HA + H2O <===> H3O+ + AThe acid dissociation constant, Ka, is a measure of the how much the acid dissociates. Ka = [H30+][A-]/[HA] Similarly, a weak monovalent base, BOH, dissociates to give B+ and OH-. The base dissociation constant, Kb, is a measure of the degree that the base dissociates. Kb = [B ...
Assistance Lecturer Amjad Ahmed Jumaa Arrhenius theory of acids
... If the correct amounts of acids and bases are mixed together, the original properties of the acid and bases are lost. The reaction product has a taste that is salty sour or bitter. A salt and water were formed when an acid neutralizes a base. For example: H2SO4 (aq) + 2KOH (aq) → ...
... If the correct amounts of acids and bases are mixed together, the original properties of the acid and bases are lost. The reaction product has a taste that is salty sour or bitter. A salt and water were formed when an acid neutralizes a base. For example: H2SO4 (aq) + 2KOH (aq) → ...
Tutorial 6 Writing Chemical Formulas for Molecular Compounds and
... • Ionic compounds form when metals transfer valence electrons to nonmetals forming cations and anions, respectively. The ratio of cations to anions is always expressed in the simplest whole number ratio k ...
... • Ionic compounds form when metals transfer valence electrons to nonmetals forming cations and anions, respectively. The ratio of cations to anions is always expressed in the simplest whole number ratio k ...
Chapter 2: Aqueous Soln` H
... Representation of the transport of CO2 from the tissues to the blood with delivery of O2 to the tissues. The opposite process occurs when O2 is taken up from the alveoli of the lungs and the CO2 is expelled. All of the processes of the transport of CO2 and O2 are not shown such as the formation and ...
... Representation of the transport of CO2 from the tissues to the blood with delivery of O2 to the tissues. The opposite process occurs when O2 is taken up from the alveoli of the lungs and the CO2 is expelled. All of the processes of the transport of CO2 and O2 are not shown such as the formation and ...
Sulfuric acid
Sulfuric acid (alternative spelling sulphuric acid) is a highly corrosive strong mineral acid with the molecular formula H2SO4 and molecular weight 98.079 g/mol. It is a pungent-ethereal, colorless to slightly yellow viscous liquid which is soluble in water at all concentrations. Sometimes, it is dyed dark brown during production to alert people to its hazards. The historical name of this acid is oil of vitriol.Sulfuric acid is a diprotic acid and shows different properties depending upon its concentration. Its corrosiveness on other materials, like metals, living tissues or even stones, can be mainly ascribed to its strong acidic nature and, if concentrated, strong dehydrating and oxidizing properties. Sulfuric acid at a high concentration can cause very serious damage upon contact, since not only does it cause chemical burns via hydrolysis, but also secondary thermal burns through dehydration. It can lead to permanent blindness if splashed onto eyes and irreversible damage if swallowed. Accordingly, safety precautions should be strictly observed when handling it. Moreover, it is hygroscopic, readily absorbing water vapour from the air.Sulfuric acid has a wide range of applications including domestic acidic drain cleaner, electrolyte in lead-acid batteries and various cleaning agents. It is also a central substance in the chemical industry. Principal uses include mineral processing, fertilizer manufacturing, oil refining, wastewater processing, and chemical synthesis. It is widely produced with different methods, such as contact process, wet sulfuric acid process and some other methods.