Homework Answers
Due to complete dissociation
of strong acids (HCl,HBr,HNO3) int solution the concentration of
hydronium ions in the water is equal to the total concentration of
the acid.
So ka is not calculated for strong acid.instead of ka pka is used.
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1.) A key component of understanding weak acids is their K, values which are just equilibrium...
3. Consider the following weak acids and their K, values, calculate the pK, for each acid....
3. Consider the following weak acids and their K, values, calculate the pK, for each acid. HC,H,O, - Acetic acid K. = 1.8 x 105 PK,= H,PO, - Phosphoric acid K = 7.1 x 10 PK, HCIO - Hypochlorous acid K = 3.5 x 10 pk = You want to prepare buffers at pH 2.8, 4.5 and 7.5. Which weak acid-conjugate base buffer system is the best choice for each pH from the acids listed? Write the reaction and indicate...
Consider the following list of K, values for various weak acids HNO, 14.6 x 10- 40...
Consider the following list of K, values for various weak acids HNO, 14.6 x 10- 40 HCIO 12.95 x 10-8 HCIO 1.12 x 10- 2 NH, 5.6 x 10-10 HSCN 1.0 x 104. HE 3.5 x 10- 4 HNHOH 11 x 10-6 CHO H 1.8 x 105 W Which of the following species below is the most basic? 2,4-Dichlorophenoxyacetic acid (ca) is a common heriode that is used to treat broad leaf weeds it is also one of two herbicides...
30 QUESTIONS FOR WEAK ACIDS & BASES EXP. 1. Examine the data for acetic acid and...
30 QUESTIONS FOR WEAK ACIDS & BASES EXP. 1. Examine the data for acetic acid and discuss the effects of dilution on the percent dissociation of this weak acid. a. What immediate effect did dilution have on Q? b. Did K change? Should it have changed? Why or why not? c. Which way did any changes cause the equilibrium to shift? Why? d. How did the shift affect the percent dissociation? Should the effects of dilution on % dissociation for...
Homework Question 8.16 Determine (or estimate) the pKa of an acid with an acidity constant K= 1 x 10^-6. Values in Ta...
Homework
Question 8.16 Determine (or
estimate) the pKa of an acid with an acidity constant K= 1 x 10^-6.
Values in Table 9.3 may be helpful.
Homework Question 8.16 Unanswered Determine (or estimate) the pKaof an acid with an acidity constant Ka=1x10-6. Values in Table 9.3 may be helpful. Type your response Table 8.3 Acidity Constants of Some Bronsted-Lowry Acids Acid, HA K pk Strong acids hydrolodic 2010 hydobromic acid hydrochloric acid sulfuric acid HUSO HIND nitric acid Weak acids...
For which of the following Keg values does the equilibrium lie to the left? a) Keo...
For which of the following Keg values does the equilibrium lie to the left? a) Keo = 1 x 10-33 b) Keg = 1 x 1028 c) Keq = 1 x 10-12 d) Keo = 1 x 102 e) no correct response 34 Which of the following weak acids is the weakest? a) Ks = 1.75 x 10-5 b) K, = 1 42 x 10-7 c) K; = 6.28 x 10-6 dj k, = 23 x 10-1 e) Ka =...
Chemistry 202 Worksheet -Equilibrium Worksheet Grade: Name: K,= POP" Key concepts 1. Equilibrium is the state...
Chemistry 202 Worksheet -Equilibrium Worksheet Grade: Name: K,= POP" Key concepts 1. Equilibrium is the state at which the concentrations of the reactants and products remain constant over time. Equilibrium is often defined in terms of Ke or Kp, the equilibrium constants in terms of concentration or partial pressure, respectively. For aA + bB - C + dD: [C]*[D]" [A]"[B]" The two constants are related to each other for a given reaction by: K = K (RT).. (Use R =...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants Periodic Table Percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid HA: A certain weak acid, HA, has a Ka value of 4.7x10-7 Percent ionization=1 _HA ionized HA initial x 100% Part A Percent ionization increases with increasing K. Strong acids, for which K, is very large,...
late for class please just help with these dont have time to make more posts 4....
late for class please just
help with these dont have time to make more posts
4. The equilibrium constant values for a number of reactions are listed below. Indicate whether the products or reactants are favored. Reaction Which side is favored? NH3(aq) + H2O(l) 5 NH4+ (aq) + OH(aq) K = 5.0 x 1012 2 HBr 5 2 Hz Brz K = 5.8 x 10-18 CH3CH(OH)COOH(aq) = CH3CH(OH)COO"(aq) + H+(aq) K= 1.4 x 10-4 5. Hydrogen chloride can be made...
please correct Question 1 (1 point) Saved Certain acids are defined as weak acids which means...
please correct
Question 1 (1 point) Saved Certain acids are defined as weak acids which means that a small percentage of acid molecules ionize in water. True False Question 2 (1 point) Saved Strong acids, like Hydrochloric acid, completely ionize in water. True False Question 3 (1 point) Saved The equivalence point of titration is also known as the stoichiometric point or end point. True False Question 4 (1 point) Saved Phenolphthalein is a pH indicator which turns bright pink...
please show work 11. Consider the K, values for the following acids: Cyanic acid, HOCN, 3.5...
please show work
11. Consider the K, values for the following acids: Cyanic acid, HOCN, 3.5 x 104 Formic acid, HCHO2, 1.7 x 104 Lactic acid, HC,H,O3, 1.3 x 104 Propionic acid, HC,H,02, 1.3 x 10- Benzoic acid, HC,H,02, 6.3 x 10-5 Given initially equimolar soutions of each weak acid, which solution will have the highest hydronium ion concentration once equilibrium is established? A) cyanic acid B) benzoic acid C) lactic acid D) formic acid E) propionic acid
3. Consider the following weak acids and their K, values, calculate the pK, for each acid. HC,H,O, - Acetic acid K. = 1.8 x 105 PK,= H,PO, - Phosphoric acid K = 7.1 x 10 PK, HCIO - Hypochlorous acid K = 3.5 x 10 pk = You want to prepare buffers at pH 2.8, 4.5 and 7.5. Which weak acid-conjugate base buffer system is the best choice for each pH from the acids listed? Write the reaction and indicate...
Consider the following list of K, values for various weak acids HNO, 14.6 x 10- 40 HCIO 12.95 x 10-8 HCIO 1.12 x 10- 2 NH, 5.6 x 10-10 HSCN 1.0 x 104. HE 3.5 x 10- 4 HNHOH 11 x 10-6 CHO H 1.8 x 105 W Which of the following species below is the most basic? 2,4-Dichlorophenoxyacetic acid (ca) is a common heriode that is used to treat broad leaf weeds it is also one of two herbicides...
30 QUESTIONS FOR WEAK ACIDS & BASES EXP. 1. Examine the data for acetic acid and discuss the effects of dilution on the percent dissociation of this weak acid. a. What immediate effect did dilution have on Q? b. Did K change? Should it have changed? Why or why not? c. Which way did any changes cause the equilibrium to shift? Why? d. How did the shift affect the percent dissociation? Should the effects of dilution on % dissociation for...
Homework
Question 8.16 Determine (or
estimate) the pKa of an acid with an acidity constant K= 1 x 10^-6.
Values in Table 9.3 may be helpful.
Homework Question 8.16 Unanswered Determine (or estimate) the pKaof an acid with an acidity constant Ka=1x10-6. Values in Table 9.3 may be helpful. Type your response Table 8.3 Acidity Constants of Some Bronsted-Lowry Acids Acid, HA K pk Strong acids hydrolodic 2010 hydobromic acid hydrochloric acid sulfuric acid HUSO HIND nitric acid Weak acids...
For which of the following Keg values does the equilibrium lie to the left? a) Keo = 1 x 10-33 b) Keg = 1 x 1028 c) Keq = 1 x 10-12 d) Keo = 1 x 102 e) no correct response 34 Which of the following weak acids is the weakest? a) Ks = 1.75 x 10-5 b) K, = 1 42 x 10-7 c) K; = 6.28 x 10-6 dj k, = 23 x 10-1 e) Ka =...
Chemistry 202 Worksheet -Equilibrium Worksheet Grade: Name: K,= POP" Key concepts 1. Equilibrium is the state at which the concentrations of the reactants and products remain constant over time. Equilibrium is often defined in terms of Ke or Kp, the equilibrium constants in terms of concentration or partial pressure, respectively. For aA + bB - C + dD: [C]*[D]" [A]"[B]" The two constants are related to each other for a given reaction by: K = K (RT).. (Use R =...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants Periodic Table Percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid HA: A certain weak acid, HA, has a Ka value of 4.7x10-7 Percent ionization=1 _HA ionized HA initial x 100% Part A Percent ionization increases with increasing K. Strong acids, for which K, is very large,...
late for class please just
help with these dont have time to make more posts
4. The equilibrium constant values for a number of reactions are listed below. Indicate whether the products or reactants are favored. Reaction Which side is favored? NH3(aq) + H2O(l) 5 NH4+ (aq) + OH(aq) K = 5.0 x 1012 2 HBr 5 2 Hz Brz K = 5.8 x 10-18 CH3CH(OH)COOH(aq) = CH3CH(OH)COO"(aq) + H+(aq) K= 1.4 x 10-4 5. Hydrogen chloride can be made...
please correct
Question 1 (1 point) Saved Certain acids are defined as weak acids which means that a small percentage of acid molecules ionize in water. True False Question 2 (1 point) Saved Strong acids, like Hydrochloric acid, completely ionize in water. True False Question 3 (1 point) Saved The equivalence point of titration is also known as the stoichiometric point or end point. True False Question 4 (1 point) Saved Phenolphthalein is a pH indicator which turns bright pink...
please show work
11. Consider the K, values for the following acids: Cyanic acid, HOCN, 3.5 x 104 Formic acid, HCHO2, 1.7 x 104 Lactic acid, HC,H,O3, 1.3 x 104 Propionic acid, HC,H,02, 1.3 x 10- Benzoic acid, HC,H,02, 6.3 x 10-5 Given initially equimolar soutions of each weak acid, which solution will have the highest hydronium ion concentration once equilibrium is established? A) cyanic acid B) benzoic acid C) lactic acid D) formic acid E) propionic acid
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