Needing help answering these two questions. Thank you
Needing help answering these two questions. Thank you What will happen to the reaction equilibrium if...
Calculate the pH of the solution obtained by titrating 40 ml of 0.35 M HNO2(aq) with 0.4 M NaOH(aq) to the equivalence point. Take Ka= 4.6x10^M.
Calculate the pH of the solution obtained by titrating 40 ml of 0.35 M HNO3(aq) with 0.4 M NaOH(aq) to the equivalence point. Take K = 4.6x10^M.
Need help on questions 1-3
Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H3O+ + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) > 2 HI(g)
7. Calculate the pH of the solution obtained by titrating 50.0 mL of 0.100 M HNO2(aq) with 0.150 M NaOH(aq) to the equivalence point. Take Ka = 5.6 x 10 - M for HNO2(aq).
Need help with these 2 questions.
What will happen if we increase the temperature in the reaction vessel? CHA(g) + 2 O2(g) + CO2(g) + 2 H2O(g) + A Calculate the pH of a solution that is 0.025 M in HNO2(aq) and 0.25 M in! NaNO2(aq)). K of the acid is 4.6 x 104.
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) --------> H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
9. The equilibrium constant for the reaction H2(g) + I2(g)
2HI(g) has a value of 54.6 at 699K. What are
the equilibrium concentrations of H2, I2, and HI if the
initial concentrations at this temperature are 0.0800M
H2 and 0.0700 M I2.
10. Find the pH and pOH of a solution prepared by dissolving
9.85 grams of NaOH into a total aqueous solution
volume of 75.0 ml.
11. Using the data in Appendix B of your text, calculate the
values...
1.At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) (CH3)2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature? A. The forward reaction will proceed in order to reestablish equilibrium. B. The reverse reaction will proceed in order to reestablish equilibrium. C. No change occurs. D. The equilibrium constant will increase. E. The equilibrium constant will decrease. 2. The following reaction is...
5. The equilibrium concentrations of the reacting species in the reaction below are CO)-0.50M: [Hs)-0.45M: [CO2]-0.86M and (H20] 0.40 M a calculate Ka for the reaction at 5000 b, if we decrease the CO, concentration to 0.5M; what will the concentrations of all the gases be when equilibrium is reestablished? c. what is the Kp of this system? CO2 (g) + H2 (g) ←→CO (g) + H,O(g) 6. You are conducting a titration of 22 ml ofo.1 M HCI with...