Which of the following mixtures are effective buffer solutions at equilibrium? Select all that apply. 10 mL 1.0 M acetic acid + 10 mL 0.5 M sodium hydroxide 10 mL of 1.0 M sodium acetate 10 mL 1.0 M acetic acid + 0.01 mL 1.0 M sodium acetate 10 mL 1.0 M acetic acid + 10 mL 1.0 M sodium hydroxide 10 mL 1.0 M NH3 + 10 mL 1.0 M nitric acid 10 mL 1.0 M NH3 + 5 mL 1.0 M nitric acid mL of 1.0 M NH3 + 6 mL of 1.0 M NH¼CI 10 mL of 1.0M acetic acid + 10 mL of 1.0 M sodium acetate

Which of the following mixtures are effective buffer solutions at equilibrium? Select all that apply. 10 mL 1.0 M acetic acid + 10 mL 0.5 M sodium hydroxide 10 mL of 1.0 M sodium acetate 10 mL 1.0 M acetic acid + 0.01 mL 1.0 M sodium acetate 10 mL 1.0 M acetic acid + 10 mL 1.0 M sodium hydroxide 10 mL 1.0 M NH3 + 10 mL 1.0 M nitric acid 10 mL 1.0 M NH3 + 5 mL 1.0 M nitric acid mL of 1.0 M NH3 + 6 mL of 1.0 M NH¼CI 10 mL of 1.0M acetic acid + 10 mL of 1.0 M sodium acetate

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 95AP

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Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
Which of the following aqueous solutions are good buffer systems?(more than one answer maybe required) a) 0.40 M sodium bromide + 0.30 M calcium bromide b) 0.25 M ammonia + 0.31 M barium hydroxide c) 0.14 M hypochlorous acid + 0.17 M sodium hypochlorite d) 0.25 M hydrochloric acid + 0.23 M potassium chloride e) 0.14 M potassium hydroxide + 0.24 M potassium chloride
A student is performing a titration using NaOH and HCI. The NaOH is in the burette, the HCI is in the Erlenmeyer Flask with 3 drops of indicator. The student accidentally adds two additional drops of NaOH past the endpoint. How will this effect them calculating the concentration of the acid? O The acid concentration will be calculated as being stronger O The will be no difference in the result of the calculated acid concentration O The acid concentration will be calculated as weaker
Refer to the table below to answer the succeeding questions: Weak acids pK, pK, pK, Acetic acid 4.74 Carbonic acid 6.10 10,4 Phosphoric acid 1.97 7.00 12.5 Citric acid 3.10 4.10 6.40 A 1.0-L 0.010 M buffer with pH 6.50 is given as an assignment to a group of students. Which is the most appropriate weak acid to be used in the buffer preparation? A. Citric Acid B. Acetic Acid C. Carbonic Acid D. Phosphoric Acid What is the concentration of the weak acid and its conjugate base, respectively? O 0.0240 M and 0.0760 M O 0.0285 M and 0.0715 M O 0.0443 M and 0.0557 M O 1.708 x 10-3 M and 0.0983 M What is the mass of the conjugate base component given the following molecular weights of the solid reagents: weak acid = 236.09 g/mol, conjugate base = 258.06 g/mol? 19.61 g O 14.37 g O 25.37 g O 18.45 g What is the mass of the weak acid component given the following molecular weights of the solid reagents: weak acid = 236.09 g/mol, conjugate base = 258.06 g/mol? O 5.67 g O 6.73 g O 10.46 g O 0.40 g
Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two solutions are mixed? Select all correct answers. 0.2 M HNO3 and 0.4 M NaNO3 0.2 M HNO3 and 0.4 M HF 0.2 M HNO3 and 0.4 M NaF 0.2 M HNO3 and 0.4 M NaOH 0.2 M NaF and 0.2 M HF