A solution is made by mixing exactly 500 mL of 0.182 M NaOH with exactly 500 mL of 0.100 M CH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8 × 10−5 [H+] × 10 M Enter your answer in scientific notation. [OH−] M [CH3COOH] × 10 M Enter your answer in scientific notation. [Na+] M [CH3COO−] M
A solution is made by mixing exactly 500 mL of 0.182 M NaOH with exactly 500...
A solution is made by mixing exactly 500 mL of 0.170 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8 × 10−5 [H+] ______M [OH−] ______M [CH3COOH] _______M [Na+] _______M [CH3COO−] ________M enter your answer in scientific notation.
A solution is made by mixing exactly 500 mL of 0.136 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8 × 10−5 [H+] [OH-] [CH3COOH] [Na+] [CH3COO-]
A solution is made by mixing exactly 500 mL of 0.196 M NaOH with exactly 500 mL 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+.
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
Question 12 1 pts Calculate the pH of a solution obtained by mixing 60.79 mL of 0.11 M CH3COOH with 12.47 mL of 0.12 M NaOH. (K,(CH3COOH) = 1.8 x 10-5) Enter your answer to 2 decimal places. For example, if your answer is pH = 12, enter 12.00
Calculate the pH of a solution made by mixing 100.0 mL of 0.874 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.
Consider a solution formed by mixing 41.0 mL of 0.100 M H2SO4, 76.0 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 26.0 mL of 0.100 M Ba(OH)2, and 12.0 mL of 0.150 M KOH. Calculate the pH of this solution. (Refer to this table of Ka values of common monoprotic acids.) (with the correct sig figs)
For a weak base (B), a 0.0100 M and a 0.100 M solution was made. Students obtained the following pH value for the solution. Fill in the table. Report all answers (except pH or pOH values) in scientific notation. 0.0100 M B 0.100 M B pOH 4.32 3.48 [OH-] [BH+] [B] (at equilibrium) Kb For the same solution fill out the following information: 0.0100 M B 0.100 M B pH (Do not...