(Q1) What is the theoretical pH of 1.00M acetic acid (Ka = 1.8x10^-5)
What is the theoretical percent dissociation for Q1?
(Q2) What is the theoretical pH of 6.00M acetic acid (Ka = 1.8x10^-5)?
What is the theoretical percent dissociation for Q2?
(Q3) When 0.050 M HF solution has pH of 2.40, what is the percent dissociation?
(Q1) What is the theoretical pH of 1.00M acetic acid (Ka = 1.8x10^-5) What is the...
The Ka value for acetic acid, CH3COOH(aq), is 1.8x10^-5. Calculate the ph of a 2.80 M acetic acid solution. PH= Calculate the ph of the resulting solution when 3.00 mL of the 2.80 M acetic acid is diluted to make a 250.0 mL solution. PH= Answers are not 4.6 or 3.8
Consider that you have two solutions of acetic acid, Ka = 1.8x10-5, one solution that is 1.46 M and another solution that is 0.165 M. Compare the percent dissociation of acetic acid in these two solutions. What is the ratio of percent dissociation of the 1.46 M solution to the 0.165 M solution? (% dissocation of 1.46 M / % dissociation of 0.165 M) Enter your answer numerically to three significant figures.
An acetic acid solution (Ka= 1.8x10^-5) with an unknown concentration has a pH of 2.98 what is the concentration of the acidic acid solution?
Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8x10-5.
A weak acid acetic acid has a Ka of 1.8x10^-5 Calculate the pH of a solution made by dissolving 0.155 g of the sodium acetate (molarmass=82.034g/mol) in 30.0mL of water.
A "5% acidity" bottle of vinegar is approx. 0.875 M in acetic acid (Ka = 1.8x10^-5). a) Determine the approx. pH and percent ionization of acetic acid in this solution. b) Some health experts recommend adding 1 tablespoon (1 ounce) of vinegar to 1 cup of water (a total of 8 ounces). Calculate the approx. pH and percent ionization of acetic acid in this solution. c) How many mL of 0.10 M sodium acetate would be needed to make the...
The Ka value for acetic acid, CH3COOH(aq), is 1.8×10−5. Calculate the pH of a 2.40 M acetic acid solution. pH= Calculate the pH of the resulting solution when 2.50 mL of the 2.40 M acetic acid is diluted to make a 250.0 mL solution. pH=
What is the pH of a 0.358 M aqueous solution of acetic acid? Ka (CH3COOH) = 1.8x10^-5?
what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution with Ka=1.8x10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) = H3O + (aq) + CH3CO2-(aq)
A buffer solution is made by combining 1.00L of 0.350M Acetic Acid (Ka = 1.8x10-5) and 1.00L of 0.380M sodium acetate.What is the pH of the buffer after 5.00mL of 2.00M NaOH is added?