Are the reactants or products favored at equilibrium in each reaction?
a.
b.
c.
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General, Organic, & Biological Chemistry
- Ka for acetic acid at 25.0C is 1754 105. At 55.0C, Ka is 1.625 105. What are H and S for the ionization of acetic acid?arrow_forwardMost naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forwardCl2(g) + H2O(l)-> Cl–(aq) + ClO-(aq) + 2H+(aq) The addition of which substance would move the above equilibrium to the right and why? A. hydrogen ions B. hydrochloric acid C. sodium chloride D. sodium hydroxidearrow_forward
- Pmpletion Status: QUESTION 8 What is the [ H+1]in a 0.0001 M solution of HCl? O a. 1 X 10-14 M Ob.1X 10 10 M OCIX 10-4M O d. 1 X 10-7 M QUESTION 9 Which K value indicates the greatest concentration of reactants at equilibrium? eq O a. 6.7 X 105 O b. 3.2 X 109 O c.1.4 X 10-3 O d. 3,2 x 107 d. 3.2 X 10-7 QUESTION 10 Hydrocyanic acid, HCN, is a weak acid whose K value is 4.0 X 10 10, What is the pH of a 0.1 M solution of HCN? a a. 1.0 O b. 5.2 O c. 9.4 O d. 10. QUESTION 11 Save All Answers Close Winc Click Save and Submit to save and submit. Click Save All Answers to save all answers. Search the web and Windowsarrow_forwardYou are given the following information. acid Ка HF 7.2X10-4 HC2H302 1.8×10-5 HCIO 3.5X10-8 HCN 4.0X10-10 Determine the equilibrium constant for each of the following reactions and indicate which arrow would be more appropriate. (Hint: Reactions that produce less than 0.1% of products and reactions that retain less than 0.1% of reactants are not considered to be "equilibrium reactions"). (a) HC2H302 + F C2H302 K = 0 0.025 + HF (b) HCN + CIO - CN + HCIO K = 40 0.010 (c) HCIO + F - CIO + HF K = 40 87.5 lo+ (d) HF + CN + HCN K = 00 1.14e-2arrow_forwardWhen the following equation is at equilibrium, A+B⇌C+D A. The forward and reverse reaction has stopped B. Neither the forward nor reverse reaction has stopped C.The concentrations of A and B must be equal to C and D D. Only the forward reaction has stoppedarrow_forward
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