Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.17 M hydrocyanic acid + 0.19 M sodium cyanide 0.21 M perchloric acid + 0.18 M potassium perchlorate 0.28 M ammonia + 0.33 M ammonium bromide 0.18 M barium hydroxide + 0.22 M barium bromide 0.35 M calcium nitrate + 0.22 M calcium chloride

Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.17 M hydrocyanic acid + 0.19 M sodium cyanide 0.21 M perchloric acid + 0.18 M potassium perchlorate 0.28 M ammonia + 0.33 M ammonium bromide 0.18 M barium hydroxide + 0.22 M barium bromide 0.35 M calcium nitrate + 0.22 M calcium chloride

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.5QE

See similar textbooks

Similar questions

A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL of the buffer. (b) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL pure (pH 7.00) water.
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.
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?
Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?