1a. Write out the reaction for acetic acid (CH3COOH) and water. 1b. Calculate the pH of a 0.15 M solution of acetic acid, which has a K₂ of 1.8 x 10-5 1c. What would happen to the pH of the solution if you added some sodium acetate (NaCH3COO) to it? Why? (Hint: NaCH3COO contains the conjugate base of CH3COOH) Describe how the acetate ion would interact with the reaction of acetic acid in water that you wrote in part A. 1d. If it was 0.10 M sodium acetate that was added in part C, what would be the new pH value?

1a. Write out the reaction for acetic acid (CH3COOH) and water. 1b. Calculate the pH of a 0.15 M solution of acetic acid, which has a K₂ of 1.8 x 10-5 1c. What would happen to the pH of the solution if you added some sodium acetate (NaCH3COO) to it? Why? (Hint: NaCH3COO contains the conjugate base of CH3COOH) Describe how the acetate ion would interact with the reaction of acetic acid in water that you wrote in part A. 1d. If it was 0.10 M sodium acetate that was added in part C, what would be the new pH value?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 108QAP

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Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
fill in the blanks please In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.101. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =_______ While, in the same laboratory, another general chemistry student measured the pH of a 0.590 M aqueous solution of hypochlorous acid to be 3.856. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =__________
1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?
propionic acid, ?a=1.34×10−5,Ka=1.34×10−5, 3.00 M sodium propionate, CH3CH2COONa 1. The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? ( in g) 2. Based on this information, what volume of acid should the student measure to make the buffer solution? (in ml)
1) In the laboratory, a general chemistry student measured the pH of a 0.554 M aqueous solution of nitrous acid to be 1.787. Use this information she obtained to determine the Ka for this acid? Ka .......................... ? 2) How many grams of solid potassium hydroxide ( molar mass= 56.1 g/mol) are needed to react with 26.7 mL of a 1.75 M hydroiodic acid solution? KOH + HI......> kI + H2o ................ grams
Find the pH of the following solutions. First write the balanced equilibrium equation of this salt in water. Determine whether the ion that determines the pH of the solution is a Brønsted acid or a Brønsted base, then start your calculations a) What is the Kb for ammonia? b) What is the Ka for hydrofluoric acid? c) What is the pH of 0.025 M ammonium nitrate? d) What is the pH of 0.025 M NaF?
The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. a) Write the chemical equation for the ionization of this acid in water. b) Write the Ka expression for this acid. c) What is the equilibrium concentration of each product and the reactant? d) What is the value of Ka? e) What is the pH of the solution?
6. Consider the reaction of 50.0 mL of 2.0 M nitric acid with 90.0 mL 1.0 M potassium hydroxide. Determine the pH, pOH, [H3O+], and [OH-] once the reaction is complete.
What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml of 3.66M Sodium Formate (NaHCO2) together? If you were to now add 18 ml of 1.2M NaOH to the buffer solution, what would the new pH be?
A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
A chemist wishes to prepare a standard aqueous solution that has a concentration of Fe3+ equal to 1.0x10-5 M. This solution is to be prepared by allowing water at a set pH to reach equilibrium with solid Fe(OH)3. Given the fact that pH = -log [H+], what pH should be used for the aqueous solution to give this desired concentration of [Fe3+].

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