Question 6 (2 points) A 1.00-L of a buffer contains 0.316 M CH3COOH(aq) and 0.315 M...
Question 8 (2 points) A 1.00-L of a buffer contains 0.076 M CH3COOH(aq) and 0.214 M CH3COONa(aq); Kalacetic acid) - 1.8 x 10-5. Calculate the pH after the addition of 0.003 moles HCI. Provide your answer to two places after the decimal.
Calculate the pH of 1.00 L of the buffer 1.05 M CH3COONa/0.96 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: 4.786 (b) pH after addition of 0.065 mol NaOH: (c) pH after further addition of 0.144 mol HCI:
please solve and show work! A buffer contains 0.50 M CH3COOH (acetic acid) and 0.50 M CH3COONa (sodium acetate). The pH of the buffer is 4.74. What is the pH after 0.10 mol of HCI is added to 1.00 liter of this buffer? A.5.57 B.4.74 C.4.38 D. 4.92 E.4.57
Calculate the pH of 1.00 L of the buffer 1.04 M CH3COONa/1.10 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.045 mol NaOH: (c) pH after further addition of 0.145 mol HCl:
Calculate the pH of 1.00 L of the buffer 1.03 M CH3COONa/0.97 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.080 mol NaOH: (c) pH after further addition of 0.144 mol HCl:
7. Calculate the mass of sodium acetate (CH3COONa) that must be added to 1.00 L 0.450 M acetic acid (CH3COOH), Ka = 1.8 x 10 ) to form a pH = 5.00 buffer. Ka = 1.8 x 109.
calculate the ph of a buffer solution that contains 1.5 M acetic acid (CH3COOH) and 0.3 M sodium acetate (CH3COONa) [Ka=1.8x10-5 for acetic acid]
(Please show work) A 100.0 mLbuffer solution is 0.250 M in acetic acid (CH3COOH) and 0.250 M in sodium acetate (CH3COONa). [Acetic Acid (CH3COOH) Ka = 1.8 x 10-5] a)What is the pH of this buffer solution? b)What is the pH after addition of 0.0050 mol of HCl? c)What is the pH after addition of 0.0050 mol of NaOH?
1. Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the...
A buffer formed from 20.0 mL of 0.120 M Acetic acid (CH3COOH) (pKa = 4.74) and 12.0 mL of 0.200 M sodium acetate (CH3COONa). What is the pH of this buffer after addition of 0.0001 mol of HCl?