1) Find the pH of 0.200 M HF acid solution
2) Find the pH of a and [H3O+] of 0.100 M benzoic acid solution
Explain how you got answer!
.HF + H2O <==> H3O+
+ F-
Initial . . . . . .0.2 . . . . . . . . . . . . .0 . . . . . 0
Change . . . . .-x . . . . . . . . . . . . .x . . . . . x
At Equil. . .0.2-x . . . . . . . . . . . . .x . . . . ..x
Ka = [H3O+][F-] / [HF] = (x)(x) / (0.20-x) = 6.8 x 10^-4. . .the -x
term will be small compared to 0.20 so we delete it.
x^2 / 0.20 = 6.8 x 10^-4
x^2 = 1.4 x 10^-4
x = 1.2 x 10^-2 = [H3O+]
pH = -log [H3O+] = -log (1.2 x 10^-2) = 1.93
2)
Find the pH of a 0.200 M HNO2 solution. -Remember that this is a weak acid. HNO2 (aq) + H2O (l) = H3O+ (aq) + NO2- (aq)
Benzoic acid (C6H5COOH), a commonly used food preservative, is a weak acid. A 0.200 M aqueous solution of benzoic acid has a pH of 2.44. Determine the concentration of H3O+in solution.
1. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the [H3O+] in the solution. 2. Suppose you have a 0.100 M solution of a weak acid that has a pH of 2.07. Calculate the Ka for this acid. *Report your answer to 2 significant figures.
If a buffer solution is 0.300 M in a weak base (K5 = 2.7 x 10 ) and 0.400 M in its conjugate acid, what is the pH? pH = You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK-4.20) and 0.200 M sodium benzoate How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: Amt ml. sodium benzoate: 1 ml
Determine the [H3O*1 and pH of a 0.200 M formic acid (HCHO2) solution. The Ka of formic acid at 25 °C is 1.8 X 10. (1 point)
You have solutions of 0.200 M HF and 0.200 M KF (Ka for HF = 7.2 × 10–4). A buffer of pH 3.00 is needed. What volumes of HNO2 and KNO2 are required to make 1 L of buffered solution? I am really confused about how to do every step of this. Please write it out and explain EVERYTHING. Thank you
Find the pH of a 0.200 M HNO2 solution. - Remember that this is a weak acid. HNO2 (aq) + H2O(l) = H3O+ (aq) + NO; (aq) O pH = 3.45 O pH = 7.05 O pH = 15.5 O pH = 2.02 O pH = 0.45 0 pH = -2.14
Calculate the pH of a solution that is 0.100 M in hydrofluoric acid (HF) and 0.100 M in sodium fluoride (NaF). Ka of hydrofluoric acid is 6.3 x 10-4
#15.64 1) Determine the [H3O+] of a 0.200 M solution of formic acid. (express with 2 sig figs) 2) Determine pH of this solution of formic acid. (express to two decimal places)
a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of benzoic acid C6H5CO2H and 0.100 M sodium benzoate NaC6H5CO2. Ka = 6.3 x 10-5. b) Calculate the pH after .10 mL of 1.00 M H+ has been added. c) Calculate the pH after 10 mL of 1.00 M OH- has been added.