Show your work for full credit. What would the pH of the solution be if 6.00...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
Write legibly. Show your work for full credit. All calculations should be performed for an aqueous solution at a temperature of 25 °C. 1. Calculate the pH after the addition of 0.00, 10.00, 25.00, 40.00, 45.00 ,50.00, 51.00, 55.00, 60.00, and 70.00 mL of 0.1000 M of HCl in the titration of 50.00 mL of 0.1000 M NaOH.. 2. Make a graph of pH versus the volume of HCl added. (Use Excel Spread Sheet)
Please record your answers directly onto these pages. Show all work for full credit. 1. A buffer solution is prepared by adding 60.00 mLs of 0.345 M NaH3EDTA and 65.00 ml.s of 0.350 M Na2H2EDTA. (The fully protonated acid is HAEDTA, a tetraprotic acid) a. Give the NIE associated with each K. Kal = 1.02 x 10-2 Kay= 2.14 x 10-3 Ka3 -6.92 x 10-7 K4 = 5.50 x 10-11 b. Calculate the pH of this buffer solution. c. Calculate...
1. What is the pH of a hypoiodous acid/sodium hypoiodite buffer in which the concentration of the weak acid component is 0.129 M and the concentration of the conjugate base is 0.102 M?Ka=2.3E-11. 2. The pH of a hypoiodous acid/sodium hypoiodite buffer in which the concentration of the weak acid component is 0.140 M and the concentration of the conjugate base is 0.070 M is 10.34. Suppose 0.128 g of solid NaOH are added to 100 mL of this buffer...
25. If 10.00 mL of 0.200 M HCl is added to 30.0 mL of 0.0500 M NaOH, what is the solution? Show all work for full credit. (6 pts)
(a) What is the pH of a solution that contains 0.100 M HClO and 0.300 M KClO? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH?
irmat Arrange View Share Window Help Extra Credit Question-Lab 8-Studying pH of weak and strong acids, salt and buff T T Insert Table Chart Text Shape Media Comment 25% Zoom Lab 8: Studying the pH of Strong Acid, Weak Acid, Salt and Buffer Solutions. What would the pH of a solution that contains 25.1 mL of 0.50 M ammonia? What would the pH be if 2.78 mL of 0.0471 M HC) was added to the ammonia solution? Show all work...
15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing 1.0 mmol CH3COOH and 1.0 mmol CH3COO-. What is the new solution pH? (show work) a) 11.89 b) 2.11 c) 7.87 d) can't tell/need more info.
Pre-Lab Calculating pH and Buffer Capacity (You must show work for credit) Name: 1. Calculate the volume of glacial acetic acid (17.6 M) and mass of sodium acetate (mm 82.03) required to make 102 ml of 0.20 M buffer at pH 4.85. The Ka of acetic acid is 1.4 x10. (this question is challenging, use the background section and your book for help). 2. Consult the table of Ka values in the back of your textbook and suggest acid/conjugate base...
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.