4. (12 pts) A buffer is created by mixing 50.0 mL of 0.50 M C6H5N and...
3) Calculate the pH of a solution by mixing 50.0 mL of 0.200 M Na2HPO4 with 20.0 mL 0.0400 M NaH2PO4. (Hint: Buffer solution. Use Henderson-Hasselbalch equation) H3PO4 5 H+ + H2PO4 pkı = 2.1 H2PO4 5 H+ + HPO42- pK2 = 7.2 HPO42- 5 H+ PO43- pK3 = 12.3
A buffer is prepared by combining 80.0 mL of 0.50M HClO and 40.0 mL of 1.0M NaClO. The Ka of hypochlourous acid is 3.5X10-8. a.) if one adds 0.080 mol of solid KOH to the solution, what will be the new pH? assume no change in volume. b.) If instead, one adds 20.0 mL of 1.0 M HCl to the orginal buffer, what will be the new pH?
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHCO Na. Record this pH in Part II data sheet, Beaker #1 & N2 for Theoretical Initial pH. K for CHCOH = 1.8 x 10 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCL Record in Part Il data sheet, for Theoretical Final pH...
A buffer can be formed from the combination of A) 50.0 mL of 0.50 M HNO3 and 50.0 mL of 0.25 M KNO3. B) 50.0 mL of 0.50 M HNO3 and 50.0 mL of 0.50 mL of KNO2. C) 50.0 mL of 0.50 M HNO3 and 25.0 mL of 0.25 M KNO3 D) 50.0 mL of 0.50 M HNO3 and 25.0 mL of 0.75 M KNO2. E) 50.0 mL of 0.50 M HNO3 and 50.0 mL of 0.50 M KNO2.
Calculate the pH of the buffer created when 10.00 mL of 0.300 M HBr is added to 40.00 mL of 0.200 M methylamine at 25 degrees Celsius. (CH3NH2 Kb = 4.4x10^-4). Show all relevant chemical equations. (Answer is pH=10.87)
Help: what is the pH after mixing If 50.0 mL of 0.100 M NaOH(a) is added to this buffer solutn then what is the final pH? Situation: Consider a buffer system / solution composed of 100.0 mL 0.100 M hydrochloric acid mixed with 300.0 mL of 0.150 M sodium acetate at 298 K.
3. pH OF BUFFERS Calculate the pH of a buffer prepared by mixing 50.0 mL of 0.10 M acetic acid and 35.0 mL of 0.10 M sodium acetate. intermediate value Final value pH of buffer (15) 2
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0 mL of a 0.50 M NaHCO3 solution in a test tube. The pH of this buffer was found to be 10.20. After 2.0 mL of 1.0 M HCl solution is added to this buffer solution, the pH is measured to be 9.95. What is the buffering capacity with respect to a strong acid, βa, of this buffer solution, in units of mol/L per pH unit?...
HEPES is a commonly used biochemical buffer with a pKa 7.5 at 25 °C. Please answer the questions below on the use of HEPES as a buffer. Use the Henderson-Hasselbalch equation. a) What is the pH of a solution prepared by combining 100.0 mL of 0.50 M protonated HEPES with 50.0 mL of 0.20 M HEPES base and diluting to a final volume of 1.00 L? b) You add 20 mL of 1.0 M NaOH to the solution prepared in...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M acetic acid/sodium acetate buffer 50.0 mL 0.10 M acetic acid/sodium acetate buffer + 1.0 mL 1.0 M HCl 50.0 mL 0.10...