Calculate the pka and ka given the pH. Please show ALL steps measured pH = cal, pKa = q. I 0 pH1 after 5 drops of NaOH-14- pH after 5 drops of HCl = gng BE SURE TO GET T 3) Buffer System with 2 ml acid + 20 ml conjugate base [B]/ [HB] = 10 BE SURE TO GET THIS CORRECT!! (use "H+H" Eq. above to calculate pKa) measured pH- 450 pH after addition of XS NaOH-10.00 dition of...
Properties of Buffers Lab. I need help with problems 7 & 8. They’re pretty similar, but I’m confused on whether I’m doing them right. I need to calculate the moles of HCl and NaOH and then somehow insert them into the log fraction in the Henderson Hasselbach formula, is that right? Procedure (values are needed in procedure): Measured values during lab that I’ll be comparing #6/7/8 to: Questions I need help with: Part B Procedures: 1. Weigh about 3.5g of...
Hello, I will try this again I am trying to prepare a buffer from a solution of a weak acid. This is for part D. of Experiment 25 - Ph Measurements - buffers and their properties I am to be give an 0.50 M solution of weak acid with a given pKa, and I will preparre a buffer of a desired pH measurement (choose any pH) I must first dilute the acid solution to 0.10 M by adding 10 ml...
PART C. Properties of Buffers Buffer system selected_HCO -(0,2- Weak acid name _ NaC,H,O, pH of buffer 4.68 (H') = 2.09 XIOK 2.09x10 pH of diluted buffer 4.13 [H") = 1.8x10K - 1.8x10-5 pH after addition of five drops of NaOH 4.76 pH after addition of five drops of HCI - 4.69 pH of buffer in which (HA) = 0.10 5.66 K.- 2.188x106 pH after addition of excess NaOH 11.53 (2.188x10-6) (0.00) pH of distilled water 8.22 10.09) pH after...
i need help explaining this, explain the results. discuss the change in pH for water and contrast it to the change in pH of the buffer system thanks General Chemistry II Laboratory Manual After addition: H,O 82PH 4 656 pH 7 8.1 pH 10 o Explain the results. Discuss the change in pH for water and contrast it to the change in pH of the buffer systems Acid Addition Base Addition 3. Buffer Preparation Assigned buffer pH S.5 L a....
I need help with the problem in the last photo.. I thought I’d post my lab explanation and data if that helps you get a better understanding, but it’s just the question at the end. I know I need to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log( [acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how do I find the concentrations to put in the log fraction? Thanks, in advance! Learning Objectives: 1....
I am needing help to solve this table. specifically the step 4 portion. My 2 compounds that I'm using for this experiment are 0.1 M NaHCO3 (acid) and 0.1 M Na2CO3. im having issues finding the concentration and pKa of everything. thank you! Step 1 hydrogen carbonate/carbonate (HCO3/003-) [NaHCO₃ and Nagco ₂] Initial Buffer: Pour 10 mL of the acid component of your buffer into a 50-ml beaker. Add 10 mL of the conjugate base of your buffer, and mix....
c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml of this buffer. For full creds, show your work in detail. (4) aj Calculate the pH if 9.5 mL of 10.0 M NaOH (ag) is added to 200.0 mL ofa freshly prepared solution of this buffer. For full credit, show your work in detail (4) e) You should see from the calculations that this buffer is better able to buffer against added acid than...
How do you find the degree of ionization of the solutions when accounting for the dillution effect of adding 10 mL of water? Also for the second page, how do you calculate pH with a buffer using the Henderson-Hasselbalch equation? Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for the dilution effect of adding 10.0 mL of water, and use MV1 = M2V2 Degree of lonization of solution 2...