A "5% acidity" bottle of vinegar is approx. 0.875 M in acetic acid (Ka = 1.8x10^-5)....
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 pH of the solution in part b equal to the pKa of acetic acid? Note: 1 cup is approx. 236.6 mL.
d) What would be the pH of the solution in part c after adding 1.0 mL of 0.10M NaOH?
Please show all work!! Thank you!!
Homework Answers
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A "5% acidity" bottle of vinegar is approx. 0.875 M in
acetic acid (Ka = 1.8x10^-5)....
Vinegar is a solution of acetic acid in water. If a 325 mL bottle of distilled...
Vinegar is a solution of acetic acid in water. If a 325 mL bottle of distilled vinegar contains 18.3 mL of acetic acid, what is the volume percent (v/v) of the solution?
Vinegar is a solution of acetic acid in water. If a 145 mL bottle of distilled...
Vinegar is a solution of acetic acid in water. If a 145 mL bottle of distilled vinegar contains 34.2 mL of acetic acid, what is the volume percent (v/v) of the solution? Express your answer to three significant figures.
The Ka value for acetic acid, CH3COOH(aq), is 1.8x10^-5. Calculate the ph of a 2.80 M...
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
A weak acid acetic acid has a Ka of 1.8x10^-5 Calculate the pH of a solution...
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.
(Q1) What is the theoretical pH of 1.00M acetic acid (Ka = 1.8x10^-5) What is the...
(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?
4. Mr. Burnes bought a bottle of vinegar and wondered how concentrated the acetic acid (CH-COOH;...
4. Mr. Burnes bought a bottle of vinegar and wondered how concentrated the acetic acid (CH-COOH; mm = 60.05 g/mol) was inside. He titrated it with 0.00182 M NaOH that he found in a general chemistry laboratory. It took 9.90 mL of NaOH to reach the equivalence point. See titration curve on next page. A. What is the concentration of acetic acid if 23.7 mL of vinegar was used for the titration? B. Mr. Burnes bought the economy size bottle...
Acetic acid has a pKa of 4.74. A stock solution of 1.0 M acetic acid is...
Acetic acid has a pKa of 4.74. A stock solution of 1.0 M acetic acid is available. A stock solution of 2.0 M potassium acetate is available. Show all the calculations and explain how to make 560.0 mL of 250. mM acetate buffer that has a pH = 5.0. (Hint: first make a 250 mM potassium acetate solution and a 250 mM acetic acid solution. Then determine how much of each to use.). pH = pKa + log {[acetate]/[acetic acid]}
The ionization energy of Acetic acid is 1.8x10^-5. Calculate the pH for each of the following...
The ionization energy of Acetic acid is 1.8x10^-5. Calculate the pH for each of the following points in the titration of 100.0 mL of .210 M acetic acid with .300M NaOH A. Calculate the initial pH (no NaOH added) B. Calculate the pH after the addition of 41.0 ml of NaOH. C. Calculate the pH after the addition of 100.0 mL of NaOH. Please show work to help me understand. Thanks.
2.) Vinegar is an aqueous solution (homogenous mixture) of acetic acid and water laqueous aqua" -...
2.) Vinegar is an aqueous solution (homogenous mixture) of acetic acid and water laqueous aqua" - Latin for water). To simplify the calculations let us assume that all of the acetic acid in the vinegar reacts and there is some left over "excess" baking soda. The vinegar solution is a 5% acetic acid solution. If you look at the bottle of vinegar somewhere on there it probably says "5% acidity" or similar notation. Let us estimate that about 25.0 g...
Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8x10-5.
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4. Mr. Burnes bought a bottle of vinegar and wondered how concentrated the acetic acid (CH-COOH; mm = 60.05 g/mol) was inside. He titrated it with 0.00182 M NaOH that he found in a general chemistry laboratory. It took 9.90 mL of NaOH to reach the equivalence point. See titration curve on next page. A. What is the concentration of acetic acid if 23.7 mL of vinegar was used for the titration? B. Mr. Burnes bought the economy size bottle...
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