The ionization reaction of acetic acid in water is
CH3COOH + H2O <=> CH3COO- + H3O+
Initial Conc: 0.1 0 0
At Equilibrium: 0.1 - x x x
We know Ka= 1.8 x 10 ^ -5 for acetic acid
so
Ka= [CH3COO-]*[H3O+]/[CH3COOH]
1.8 x 10 ^ -5 = x^2/(0.1-x)
On solving this equation we get
x = 0.0013 => [H+]
so pH = -log([H+]) = 2.88
8. Write the reaction of acetic acid in water and calculate the pH of a 0.100...
100mL of 0.100 M NaOH is added to 250mL of 0.100 M acetic acid, and water is added to gove a final volume of 1 L. What is the pH of the final solution? The Ka for acetic acid is 1.74 x 10^-5 M.
a) Write the dissociation reaction and corresponding K, expression for CH3NHs in water 8. b) Write the reaction with water and corresponding Ko expression for aniline (CGHsNH2) 9 A typical sample of vinegar has pH of 3.0. Assuming the vinegar in only an aqueous solution of acetic acid (Ka 1.8 x 105), calculate the concentration of acetic acid in vinegar? 10. Calculate the pH of a solution that contains 1.0 M HF (K-7.2x10) and 1.0 M CHsOH (K-1.6x1010). Calculate the...
Part B: pH vs Concentration of Acetic Acid a) Write a chemical equation that shows what happens when acetic acid is dissolved in water. Be sure to use a double arrow since this is a weak acid) b) Using the measured pH in Part B, calculate the concentrations of all species in the reaction. When finished, enter the results into a table like the following: Concentration pH [H,o ] 2.H7 2. 86 3.18 Acetic Acid [C,H,o2 1 [HC2H 021 1.00...
What is the pH of a solution that is 0.100 M in acetic acid and 0.150 M in sodium acetate? pKa of acetic acid = 4.76 A. 6.26 B. 4.58 C. 2.94 D. 4.94
1. Calculate the pKs of acetic acid. Please write out the entire calculation. 2. Calculate the pH of a 0.100 M acetic acid, 0.500 M sodium acetate buffer solution. You do not need to check any simplifying approximations made. 3. Calculate the pKa of the ammonium ion. Please write out the entire calculation. 4. Calculate the pH of a 0.200 M ammonia, 0.400 M ammonium chloride buffer solution. You do not need to check any simplifying approximations made.
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:
A) Calculate the pH of an acetic acid solution. The concentration of acetic acid is 1.0696M and the pKa of acetic acid = 4.75. B) Calculate the pH of a sodium acetate solution of concentration 1.0401M. C) Calculate the pH of a solution made of 100 mL each of the two above solutions (200 mL total) D) Calculate the pH of a solution made of 40 mL of the solution in part C + 160 mL water (200 mL total)...
A solution containing 50.00 mL of 0.100 M of acetic acid is titrated with 0.100 M of a strong base KOH. Calculate the pH of the solution before the base is added. Ka = 18x10-5 OAZO OB 10 OC 29 00.25
Name 1 (25 pts) Consider the titration of 50 mL of 0.100 M acetic acid (CH-COOH, K. -1.8 x 10) 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: