Consider a buffer composed of aqueous HA and A- . The Ka for HA is 3.7 x 10-9 . Which of the following combinations of reagents will produce an HA / A- buffer with pH 8.13? A. 0.80 mol of HA and 0.40 mol of A - B. 0.80 mol of HCl and 1.20 mol of A - C. none of these D. 1.20 mol of HA and 0.40 mol of NaOH E. all of these
Consider a buffer composed of aqueous HA and A- . The Ka for HA is 3.7...
Consider a buffer composed of aqueous HA and A.The Ka for HA is 3.7 x 109. The concentration of HA (aq) and A (aq) would be equal in a buffer solution with a pH equal to O A. 9.28 B. 7.00 C. 6.63 OD. 4.75 E.8.43 Reset Selection
Ka for NH4^+ ion is 5.6x10^-10 at 25 oC. Which of the following combinations of reagents will produce a buffer with pH=8.85 ? a) 1 mol NH4Cl and .4 mol NH3 b) 1.4 mol NH4Cl and .4 mol NaOH c) 1 mol HCl and 1.4 mol NH3 d) all of these e) none of these
QUESTION 3 What is the pH of a buffer solution composed of HA and A (Ka = 1.38 x 10-4) under these conditions: concentration of HA = 0.62, concentration of A = 0.65
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.45×10–8), and the conjugate base, A–, after 2.71 mL of 0.135 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.7 M and [A–]=0.37 M. Enter your value to two (2) decimal places.
What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.58×10–5), and the conjugate base, A–, after 1.83 mL of 0.094 M HCl solution is added. The initial concentrations of the 133 mL buffer solution are [HA]=0.38 M and [A–]=0.67 M. Enter your value to two (2) decimal places.
1. Determine the pH of a buffer solution prepared by mixing 25.3mL of 0.35M HA (Ka= 1.6x10-5) with 15.3mL of 0.45M NaA. 2.100 mL of buffer solution that is 0.15M HA (Ka= 6.8x10-5) and 0.20M NaA is mixed with 17.3mL of 0.25M HCl. What is the pH of the resulting solution? 3. Calculate the pH of a solution made by mixing 75.0mL of 0.15M HA (Ka= 2.5x10-5) with 7.5mL of 0.75M NaOH 4. 100 mL of buffer solution that is...
1.What is the pH at which a buffer composed of NH3 and NH4+ would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15. 2. Consider a 1.0 L buffer containing 0.119 mol L-1 HF and 0.081 mol L-1 F-. What is the pH of the solution after adding 5.7 x 10-3 mol of NaOH? Express your answer to 2 decimal places....
Consider two buffer solutions. Buffer 1 consists of 0.50 M HA and 0.25 M KA, and Buffer 2 is made from 0.050 M HA and 0.050 M NaA. How do the pHs of these buffer solutions compare? Select one or more: a. The pH of Buffer 1 is twice the pH of Buffer 2. b. The pH of Buffer 1 is half the pH of Buffer 2. c. The pH of Buffer 1 is equal to the pH of Buffer...
Question 1 : HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M. Question 2 : We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA. Question 3 : We place 0.661 mol of a weak acid, HA,...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...