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 2.
d. The pH of Buffer 1 is 0.3 lower than the pH of Buffer 2.
e. Cannot be determined without the Ka values.
Ka will remain constant for a particular acid despite a change in concentration (all other conditions, such as temperature, held constant).
So in given buffers, both has same acid so Ka value will be same so pKa value will also be same because pKa = log Ka
By using Henderson-Hasselbalch Equation
You can calculate the pH of buffers and compare them.
Consider two buffer solutions. Buffer 1 consists of 0.50 M HA and 0.25 M KA, and...
1.) You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.050 M HOAc and 0.050 M NaOAc. How do the pHs of the buffered solutions compare? (Note: Ac– = acetate ion, CH3COO–). A. The pH of buffered solution 1 is greater than that of buffered solution 2. B. None of the answers are correct C. The pH of buffered solution 1 is equal to that of...
A buffer containing 0.50 M of an acid (HA) and 0.10 M of its conjugate base (A–) has a pH of 10.30. Which of the following solutions will make a buffer with a pH of 11.30? A. A solution with [HA] = 0.25 M and [A–] = 0.10 M. B. A solution with [HA] = 0.50 M and [A–] = 0.50 M. C. A solution with [HA] = 0.10 M and [A–] = 0.50 M. D. A solution with [HA]...
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...
1.00 L buffer made with 0.50 M generic acid HA and its conjugate salt 0.75 M NaA has a pka of 8.599 If you add 45.0 ml of 0.446 M NaOH, what is the new pH? Answer to 3 decimal places. (Your scratch paper must show work to receive partial credit)
Which of these solutions would be the best choice for a pH 11.00 buffer? Ka Acid HA HB 7.59 x 10-4 1.26 x 10-6 7.94 x 10-9 1.32 x 10-11 HC HD O 1.0 MHC and 1.0 M NaC They are all equally good 1.0 M HD and 1.0 M NaD O 1.0 MHA and 1.0 M NaA 1.0 MHB and 1.0 M NaB
Consider the following solutions: Solution 1: 0.100 L of 0.25 M NaCH3CO2 + 0.050 L of 0.25 M HCl Solution 2: 0.100 L of 0.25 M HCH3CO2 + 0.050 L of 0.25 M NaOH 1. How many moles of acid does it take to change the pH of the original Solution 1 by 0.30 pH units? 2. How many moles of acid does it take to change the pH of the original Solution 2 by 0.30 pH units?
1. Calculate pH and % ionization of 0.25 M Naco (Ka (HCO2H) 1.8 x 10") 2- Calculate the pH of: a) 0.35 M HNO b) 0.15 M Sr(O)2 c) 0.08 M Ba(CIO4)2 3- Calculate the pH of 0.375 L buffer solution made of a 0.18 M Acetic acid HC2H:02(Ka 1.8x 10) and a 0.134 M Potassium acetate KC2Hs02 (do not use more than 3 digits beyond the decimal point) a) before adding anything b) after adding 0.010 mol Ba(OH)2 c)...
1. Consider a 0.475 M NaA(aq) solution in which HA(aq) has a Ka of 1.950E-03 at 25°C. a. Identify the major species present in the NaA(aq) solution. Major species: b. Calculate the Kb of the conjugate base, A (aq). Kb = c. Calculate the pH of a 0.475M NaA(aq) solution.
28. A 0.50 L buffer solution is 0.20 M in HF and 0.40 M in NaF. The Ka for HF is 1.5 x 10*. Show all work for full credit. (a) Calculate the pH of the solution after the addition of 0.025 moles of solid KOH. (3 pts) (b) Calculate the pH of the solution after the addition of 0.050 moles of HCI. (3 pts)
Consider the following solutions: Solution 1: 0.100 L of 0.25 M NaCH3CO2 + 0.050 L of 0.25 M HCI Solution 2: 0.100 L of 0.25 M HCH3CO2 + 0.050 L of 0.25 M NaOH What is the pH of Solution 1 after adding 4.2 mmol of strong base? The number of significant digits is set to 3; the tolerance is +/-1.0% LINK TO TEXT What is the pH of Solution 2 after adding 4.2 mmol of strong base? The number...