For the system
HC6H5O + C4H2O2^- ----> C6H5O^- + HC4H7O2
the position of the equilibrium lies to the left. Which is the strongest acid in the system?
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For the system HC6H5O + C4H2O2^- ----> C6H5O^- + HC4H7O2 the position of the equilibrium lies...
7. Label the acid and the base. Indicate whether the equilibrium lies to the left or the right. Using curved arrows, show the flow of electrons that explain the formation of the favored product - Hoco + HCC pH • NHỊ DK, 4.7 ® NH. 2 DK, = 9 H-CI - CH, OH C b. PK, -7 - CH,OH, PK,- -2.5 HẠC-CCH N - HỌC-C=C c. PK, 26 + NH4 PK, = 36
The acetic acid/acetate buffer system is a common buffer used in the laboratory. Write the equilibrium equation for the acetic acid/acetate buffer system. The formula of acetic acid is CH,CO,H. equilibrium equation: Which way does the equilibrium shift if more H,O is added? The equilibrium will not change. The equilibrium will shift to the left. The equilibrium will shift to the right. Which way does the equilibrium shift if more OH” is added? The equilibrium will shift to the right...
I answered the first 2, I just need the explanation for 16, thank you. Use this information for the next 3 questions: HCN (K, = 6.2 x 10:10) HCHO2 (K, = 1.7 x 10^^) HOCI (K. = 3.5 x 10%) HC,H,O2 (K, = 1.8 x 105) 14. A 0.10 M solution of which of the above acids will have the lowest pH? a. HCN) b. HCHO, C. HOCI d. HC,H,02 e. All will have the same pH 15. From the...
QUESTION 4 the concentration The position of the equilibrium for a system where K = 8.4 x 10-can be described as being favored to of products is relatively_ the right; large the right; small the left; large the left; small neither direction, large
16. The only factor that changes the equilibrium constant of a chemical reaction is: A) pressure B) concentration C) volume D) temperature 17. Determine the effect of increased pressure on the system in the following equilibrium: C(graphite)+S2(g) CS2 (g) A) The equilibrium position SHIFT to the right B) The equilibrium position SHIFT to the left C) does not change the position of equilibrium D) The Le Chatelet principle does not apply to the system. 18. If the acetic acid dissociation...
Pls help me with questions 2,4,5 pls 1. Write the structure of The conjugate acid of Hz0; the conjugate base of H20 b. a. The conjugate base of CH3CH2Co2H c. The conjugate base of CH3CH2CH2NH3 d. The conjugate acid of NaHSO3 2. Complete the following acid-base reactions. Label each acid and base and determine whether the equilibrium in the reaction lies to the right or left. CHyCH2 b. CH,CH,СНго" .H,SO NH, H2O CH,OH + 3. Rank the following in order...
9. Which of the following is not a Lewis 13. A carbocation is acid. A) BF B) NaF C) AICl D) FeBr E) ZnCl2 A) a carbon with a negative charge B) a carbon with a positive charge C) a carbon with an unpaired electron D) a carbon with complete octet E) a carbon with five hydrogens 14. Consider the following equilibrium: 10. In which of these Lewis structures would iodine be assigned a formal charge of +2? Which of...
Question 1 8 pts CH,0 Hoc LCH, CH,OH M, EH pka: CH2OH=16, (CH3)2CO=20 What is the strongest acid? Which way will the equilibrium shift? O CH3OH, towards left O CH3COCH3, towards right O CH3OH, towards right O CH3COCH3, towards left
Question 15 1 pts Indicate the position of the equilibrium for the following acid-base reaction: :0 - + :0: F 0-4 Left No preference Right Not enough information
Question 10 Which of the following statements is FALSE? Resonance forms must obey normal valency rules. Resonance is a fast equilibrium between two species. Resonance forms represent the extremes of something that really exists in between. Resonance forms differ in their arrangement of electrons only. Question 9 What is the formal charge of the nitrogen in the molecule shown below? N-H O-1 O-2 O +1 Question 8 2 pts Consider the following acid base reaction: OH CH,00 CH3OH pka =...