Question

In: Chemistry

the acid-dissociation constant for benzoic acid is 6.3*10^-5. calculate the equilibrium constant concentration of h30+, C6H5COO-,...

the acid-dissociation constant for benzoic acid is 6.3*10^-5. calculate the equilibrium constant concentration of h30+, C6H5COO-, and C6h5COOH in the solution if the initial concentration of C6H5COOH is 0.050 M

Solutions

Expert Solution

                         C6H5COOH (aq) + H2O (l) ----> C6H5COO- (aq) + H3O+ (aq)

Initial                  0.05                       -                  0                0

change                  -x                         -                      +x                    +x

equilibrium        0.05 - x                      -                       x                     x

The acid dissociation constant, Ka is given by:

Assuming x to be very small compared to 0.05, we get:

6.3 x 10-5 = x2/0.05

solving for x, we get:

x = 0.00177 M

Therefore equilibrium concentrations are:

[H3O+] = x = 0.00177 M

[C6H5COO-] = x = 0.00177 M

[C6H5COOH] = 0.05 - x = 0.05 - 0.00177 = 0.0482 M


Related Solutions

The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. A. Calculate the equilibrium concentration of H3O+...
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. A. Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 5.1×10−2M B. Calculate the equilibrium concentration of C6H5COO− in the solution if the initial concentration of C6H5COOH is 5.1×10−2 M . C. Calculate the equilibrium concentration of C6H5COOH in the solution if the initial concentration of C6H5COOH is 5.1×10−2 M .
Calculate the percent dissociation of 0.40 M benzoic acid, C6H5COOH. (Ka = 6.3 x 10^-5) ___%?
Calculate the percent dissociation of 0.40 M benzoic acid, C6H5COOH. (Ka = 6.3 x 10^-5) ___%?
1) The acid-dissociation constant for benzic acid (C6H5COOH) is 6.3 x 10^-5. Calculate the concentrations of...
1) The acid-dissociation constant for benzic acid (C6H5COOH) is 6.3 x 10^-5. Calculate the concentrations of H3O+, C6H5COO-, and C6H5COOH in the solution if the initial concentration of C6H5COOH is 0.050 M. 2) Citric acid, which is present in citrus fruit, is a triprotic acid. (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make approximations or assumptions in completing your calculations? (c) Is the concentration of citrate ion (C6H5O7^3-) equal to,...
The equilibrium constant (Ka) for benzoic acid is 6.46 x 10^-5. Calculate the ratio of benzoic...
The equilibrium constant (Ka) for benzoic acid is 6.46 x 10^-5. Calculate the ratio of benzoic acid to benzoate ion in solution pH=2.00. Then calculate the same ratio at pH=4.00.
Benzoic acid is a weak monoprotic acid occurring in most of berries. The acid dissociation constant...
Benzoic acid is a weak monoprotic acid occurring in most of berries. The acid dissociation constant of benzoic acid is 6.3 x 10-5. Find pH and percent of dissociation of 0.001 M solution of benzoic acid.
Calculate the hydroxide ion concentration in a 0.0500 M NaOCl solution. The acid dissociation constant for...
Calculate the hydroxide ion concentration in a 0.0500 M NaOCl solution. The acid dissociation constant for HOCl is 3.0 x 10-8.
Titrate 40.0 mL of 0.0350 M benzoic acid (C6H5COOH, Ka = 6.3 × 10–5) with 0.0700...
Titrate 40.0 mL of 0.0350 M benzoic acid (C6H5COOH, Ka = 6.3 × 10–5) with 0.0700 M NaOH Calculate the pH in the solution after addition of 25.0 mL of 0.0700 M NaOH. a) 2.269 b) 8.284 c) 9.845 d) 11.731 e) 5.628
Calculate the apparent solubility of benzoic acid at pH 5. Benzoic acid is a weak acid,...
Calculate the apparent solubility of benzoic acid at pH 5. Benzoic acid is a weak acid, with pKa = 4.2 and solubility of nonionized species S0 = 0.028 mol/L. Please show steps
Calculate the pH of a 0.01 M solution of sodium benzoate. A: Dissociation constant of benzoic...
Calculate the pH of a 0.01 M solution of sodium benzoate. A: Dissociation constant of benzoic acid. B: Calculate the hydrolysis constant of sodium benzoate. C: Calculate the pH of the 0.01 M solution.
The Ka of benzoic acid is 6.5 x 10 ^(-5) a) Calculate the pH of a...
The Ka of benzoic acid is 6.5 x 10 ^(-5) a) Calculate the pH of a 40.00 mL, 0.1 M benzoic acid buffer solution after the addition of 20.00 mL of a 0.1M NaOH b) Calculate the pH of a 40.00 mL, 0.1 M benzoic acid buffer solution after the addition of 50.00 mL of a 0.1M NaOH REDOX TITRATION 2) Express the reactions for potassium permanganate titration with sodium oxalate: Hint: include the 2 half-reactions. 3) What is the...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT