Question 1 To 4 Have incomplete information that is you are not written what to do.
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Calculate the for the following conditions pH = 3.21 pOH = 13.34 2. Calculate the pH...
Calculate the [H_3O^+] for the following conditions a. pH = 3.21 b. pOH= 13.34 Calculate the pH of the following solutions: a. 3.7 times 10^-3 M HCl b. 8.6 times 10^-2 M HC_2H_3O_2 K_a = 1.74 times 10^-5 Calculate the pH of the following buffer a. 7.8 times 10^-2 M HC_2H_3O_2 and 8.6 times 10^-2 M NaC_2H_3O_2 A buffer is made from 3.7 times 10^-1 M HC_2H_3O_2 and 2.9 times 10^-1 M NaC_2H_3O_2 a. What is the pH? B. If...
3. A weak triprotic acid, H3Wa, has the following pKa's: pKal = 4. 75 p Ka2 = 7. 89 p Ka3 = 10.65 a. Calculate the pH of the resulting solution when 20.00 mLs of 0.200 M Hz Wa + 45.00 mLs of 0.200 M NaOH are mixed together. Please show all your work. b. Sketch an approximate titration curve for this titration. Show the general shape, and label the: axes equivalence points + who is present buffer regions +...
Question 2: A) Calculate the pH of the buffer that results from mixing 56.1 mL of a 0.406 M solution of HCHO2 and 11.9 mL of a 0.606 M solution of NaCHO2. The Ka value for HCHO2 is 1.8×10−4 B) Calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 300.0 mL of a buffer solution that is 0.225 M in HCHO2 and 0.280 M in KCHO2 C) Calculate the initial pH and the final pH...
this is the question here is the data EXP. 5 BUFFERS, TITRATION CURVES, AND INDICATORS LAB REPORT WORKSHEETS Solution D: 20.0 mL of 1:1 buffer + 5.00 ml NaOH. See the Buffers - Calculate the pH of a Buffer Solution after a Strong Base is added (MP4 file) Calculate the pH of the solution after mixing the buffer and base. An ICE table may be helpful. Use the pka of acetic acid (previously determined using the 1:1 buffer) in...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following data: Plot the data above in excel with pH values on the Y axis and the volume of NaOH added on the X axis Graphically determine the equivalence point and indicate the pH on the graph. b. 0.00 2.00 4.00 0.46 0.54 ii. 0.62 6.00 8.00 10.00 0.7 0.78 Show the following calculations on a separate sheet of paper: 0.87 12.00 0.96 1.07 14.00...
Using the literature/accepted value of Ka where needed, calculate the expected pH of the titration mixtire: a)before any NaOH has been added b)when 18.00 mL of NaOH has been added 10 - mL Table 1: Titration of acetic acid with 0.09458 mol L 1 NaOH(aq) (5.5 marks) Volume of acid sample:__25.00 Concentration of acid: 0.08887_mol L- Indicator methyl-red Colour change: dock pink to vellas yellow pH of color change: 6.62 Sharp or gradual change: Cadud Burette Cumulative Vol Burette Cumulativo...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CH3CH2COOH; Pka = 4.87) is titrated with 0.05 M NaOH. A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the location of the...
Calculate the pH of the solution after the addition of each of the given amounts of 0.0576 M HNO2 to a 50.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04 What is the pH of the solution after the addition of pH 0.00 mL HNO,? What is the pH of the solution after the addition of pH 7.41 mL HNO? What is the pH of the solution after the addition of a volume pH of HNO...
a) Calculate the pH of a 0.8M solution of HCOOH (Ka = 1.8 x 10-4) in 0.4M Li+ HCOO-. b) Calculate the pH of a solution of 0.4M NH4Cl and 0.5M NH3 (pKa NH4+ = 9.2). c) Calculate the pH of a titration of 100 mL 1.5M HCl when 75 mL 1.25M NaOH has been added. d) What volume of 1.25M NaOH must be added to 100 mL of 1.5M HCl to reach equivalence?
6. Using the literature accepted K value where needed, calculate the expected pH of the titra (a) initially, before any NaOH(aq) has been added (5 marka) ard, calculate the expected pH of the titration inixture [1,07 = 1 (7.413x10-6.0.1030 mol/l) = 8.738810-4 pH = -log 8.73880-4 = 3.058 (b) when 18.00 mL of NaOH(aq) has been added (8 marks) Chemistry 1051 Laboratory Experiment (e when 45.00 mL of NaOH(aq) has been added (3 marks) (d) at the equivalence point (5...