Just give me the answers 14) A0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pHi of 5.35. The value of Kg for HA is A) 14 10-10 B) 7.1 10-9 E) 33 104 918-10-5 D) 3.0 10-5 15) The Kg for HON is 49-10-10, What is the value of Kb for CN-? A) 49-10-24 B) 20 10-5 D) 4.9-104 9 4.0 10-6 E) 2.0 109 16) Caleulate the pOH of a 0.0827 M aqueous...
Just give me the answers 7) The reaction below is exothermic 2502 (8) + 02 (8) 2503 (8) will result in an increase in the number of moles of SO3 (8) in Le Chatelier's Principle predicts that the reaction container. A) increasing the volume of the container B) increasing the pressure C) increasing the temperature D) decreasing the pressure E) removing some oxygen 2B. For this reaction the value of the equilibriur 8) Shown below is a concentration vs. time...
Just give me the answers 2502 (8) + 026) = 2503 (8) will result in an increase in the number of moles of SO3 (s) in Le Chatelier's Principle predicts that the reaction container. A) increasing the volume of the container B) increasing the pressure C) increasing the temperature D) decreasing the pressure E) removing some oxygen 8) Shown below is a concentration vs. time plot for the reaction A constant is 2B. For this reaction the value of the...
I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer, will not produce a pH o 9.00" 1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...
Just give me the answers 7) The reaction below is exothermic 2502 (8) + 02 (8) 2003 (8) will result in an increase in the number of moles of SO3 (8) in Le Chatelier's Principle predicts that the reaction container. A) increasing the volume of the container B) increasing the pressure C) increasing the temperature D) decreasing the pressure E) removing some oxygen 2B. For this reaction the value of the equilibriur 8) Shown below is a concentration vs. time...
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka value for CH3CO2H is 1.80 × 10-5. What is the ratio of the concentration of CH3CO2H to CH3CO2-? [CH3CO2H]/[ CH3CO2-] = _________ B) What is the pH change when 29.6 mL of 0.117 M NaOH is added to 95.4 mL of a buffer solution consisting of 0.123 M NH3 and 0.179 M NH4Cl (Ka for ammonium ion is 5.6x10^-10.) pH change =_______
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VaoH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
What is the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH3CO2H and 0.100 M NaCH3CO2? The Ka for acetic acid is 1.80E-5 Enter your answerwith two decimal places and without units.
A buffer solution is made from 0.235 M in HC2H3O2 and 0.265 M NaC2H3O2 (the Ka of acetic acid is 1.79 x 10-5). a. Determine the pH of the buffer solution b. What is the pH of the buffer solution when a 0.100 M HCl solution is added? c. What is the pH of the buffer solution when a 0.125 M NaOH solution is added?
10. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? A) CHCO02Na / CH3COOH (Ka 1.8 x 10) NH3/NH4CI (K-5.6 x 10-10) в) NaOCl/HOCI (K= 3.2 x 10-) C) NaNO2 / HNO2 (Ka= 4.5 x 104) D) NaCl/HCI E)