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 0.136 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 0.182 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 0.196 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]
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
Calculate the pH of a solution when 100.0 mL of a 0.100 M solution of acetic acid (CH3COOH), which has a Ka value of 1.8 × 10–5, is titrated with 110 mLs of a 0.10 M NaOH solution.
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
Calculate the pH of a solution made by mixing 100.0 mL of 0.355 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10–5) Select one: a. 9.66 b. 8.85 c. 4.34 d. 9.26
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)