Homework Answers
Acetic acid when ionized would lose an electron (according to Bronsted-Lowry acid-base theory, acids are proton donors) and water would act as a base and gain a proton.
In ionization reactions, a polar species becomes charged when in presence of a polar solvent.
The ionization reaction for acetic acid would be as follows:
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Consider the weak acid, CH3CO2H, acetic acid. Provide its ionization reaction:
Can someone show me how to do this? The weak acid of vinegar, acetic acid, has...
Can someone show me how to do this? The weak acid of vinegar, acetic acid, has a pKa value of 4.8. Determine the ratio of the acid form to the base form(i.e., determine [HA)/[A-]) at pH 6.0.
W THE PENCERO .99 37. Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l) = CH3CO2...
W THE PENCERO .99 37. Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l) = CH3CO2 (aq)+H30 (aq) where K=1.8x10-5 Which two bases are competing for the proton? Which is the stronger base? Why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. 38. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak...
. Calculate the ionization constant for a weak acid, acetic acid (CH3COOH), that is 1.60% ionized...
. Calculate the ionization constant for a weak acid, acetic acid (CH3COOH), that is 1.60% ionized in 0.0950 M solution. (Use the ICE table for the dissociation equation) (K. = 1.8 x 10-5 for the acetic acid)
For the acetic acid dimerization reaction: 2CH3CO2H --> (CH3CO2H)2 estimate the value of Delta H and...
For the acetic acid dimerization reaction: 2CH3CO2H --> (CH3CO2H)2 estimate the value of Delta H and the sign of Delta S
Acetic acid, CH3CO2H, is the solute that gives vinegar its characteristic odor and sour taste. (Ka...
Acetic acid, CH3CO2H, is the solute that gives vinegar its characteristic odor and sour taste. (Ka was not given in this question) Part A: Calculate the pH in 0.840 M CH3CO2H. Part B: Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 0.840 M CH3CO2H. Part C: Calculate the pH in 0.139 M CH3CO2H. Part D: Calculate the concentrations of all species present (H3O+, CH3CO2−, CH3CO2H, and OH−) in 0.139 M CH3CO2H.
determination of the molar mass and ionization constatant of a weak, monoprotoc acid. ( Lab 8)...
determination of the molar mass and ionization constatant of a
weak, monoprotoc acid. ( Lab 8)
I need help with the rest of the table.
Instructor Name EXPERIMENTS DETERMINATION OF THE MOLAR MASS AND IONIZATION CONSTANT OF A WEAK, MONOPROTIC ACID Report Sheet B. TITRATION OF ACETIC ACID Trial 1 Trial 2 Trial 3 Acetic acid/L solution Volume of acetic acid (mL) Initial buret volume (ml) 3g/L 30 ml 30mL 30mL OmL OmL OML T 14mL 16ML | 15mL |...
Can someone help me? Did I do these two correctly? 1. Consider the reaction: conjugati bile...
Can someone help me? Did I do these two correctly?
1. Consider the reaction: conjugati bile acid base conjugale conjugate acid HNO3(aq) + H2O(1)=H30*(aq) + NO2 (aq). Label the species that is a acid/base and conjugate acid/base. 2. The pH of a solution at 25°C in which [OH) = 3.7 x 10 Mis: 10-14 3.7x10-6 -2.70 x10 20 M Pt--log C++] = 19.6 unter until the pH of the solution is 11.50. The
Can someone help me deduce the oxydation numbers? This is the answer : In this reaction,...
Can someone help me deduce the oxydation numbers? This is the answer : In this reaction, the oxidation number of the carbon atom bonded to the oxygen changes from 1 in propanal to 3 in propanoic acid. Propanal is therefore oxidized to propanoic acid. The KMnO4 is reduced in this reaction. But I got +2 for the oxydation number of the carbon in the ractants and +4 for the carbon in the products... please help!
please help me with these questions! At a concentration of 1 M, the weak acid HNO,...
please help me with these questions!
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
The ionization energy of Acetic acid is 1.8x10^-5. Calculate the pH for each of the following...
The ionization energy of Acetic acid is 1.8x10^-5. Calculate the pH for each of the following points in the titration of 100.0 mL of .210 M acetic acid with .300M NaOH A. Calculate the initial pH (no NaOH added) B. Calculate the pH after the addition of 41.0 ml of NaOH. C. Calculate the pH after the addition of 100.0 mL of NaOH. Please show work to help me understand. Thanks.
W THE PENCERO .99 37. Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l) = CH3CO2 (aq)+H30 (aq) where K=1.8x10-5 Which two bases are competing for the proton? Which is the stronger base? Why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. 38. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak...
. Calculate the ionization constant for a weak acid, acetic acid (CH3COOH), that is 1.60% ionized in 0.0950 M solution. (Use the ICE table for the dissociation equation) (K. = 1.8 x 10-5 for the acetic acid)
determination of the molar mass and ionization constatant of a
weak, monoprotoc acid. ( Lab 8)
I need help with the rest of the table.
Instructor Name EXPERIMENTS DETERMINATION OF THE MOLAR MASS AND IONIZATION CONSTANT OF A WEAK, MONOPROTIC ACID Report Sheet B. TITRATION OF ACETIC ACID Trial 1 Trial 2 Trial 3 Acetic acid/L solution Volume of acetic acid (mL) Initial buret volume (ml) 3g/L 30 ml 30mL 30mL OmL OmL OML T 14mL 16ML | 15mL |...
Can someone help me? Did I do these two correctly?
1. Consider the reaction: conjugati bile acid base conjugale conjugate acid HNO3(aq) + H2O(1)=H30*(aq) + NO2 (aq). Label the species that is a acid/base and conjugate acid/base. 2. The pH of a solution at 25°C in which [OH) = 3.7 x 10 Mis: 10-14 3.7x10-6 -2.70 x10 20 M Pt--log C++] = 19.6 unter until the pH of the solution is 11.50. The
please help me with these questions!
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
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