ALEKS 360 AC INTRD CHEM >I<
5th Edition
ISBN: 9781260977585
Author: BAUER
Publisher: MCG
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Chapter 13, Problem 127QP
Interpretation Introduction
Interpretation:
The chemical substance that is used to prepare buffer solution of formic acid is to be determined.
Concept Introduction:
Generally, an acidic buffer solution is prepared by mixing a weak acid and its salt of strong base. Whereas, a basic buffer solution is prepared by mixing a weak base and its salt of strong acid.
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4
A chemistry graduate student is given 100. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of
CH,NH,Cl should the student dissolve in the CH, NH, solution to turn it into a buffer with pH = 10.93?
You may assume that the volume of the solution doesn't change when the CH,NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to
2 significant digits.
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Ar
x10
4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine
pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH
as a titrant in varying volumes. Calculate the pH of the solution at the following points:
(Ka for HCN=6.2×10-¹0)
(a) Before addition of NaOH (initial pH),
(b) After 10.00 mL of titrant addition,
(c) After 25.00 mL of titrant addition,
(d) After 50.00 mL of titrant addition.
Consider the titration of 100 mL of 0.25 M formic acid (HCOOH) with 1.0 M NaOH. The Ka of formic acid is 1.77 × 10−4.
HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l)
What is the pH of the formic acid solution before any titrant (NaOH) is added?
Chapter 13 Solutions
ALEKS 360 AC INTRD CHEM >I<
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- Briefly describe how a buffer solution can control the pH of a solution when strong acid is added and when strong base is added. Use NH3/NH4Cl as an example of a buffer and HCl and NaOH as the strong acid and strong base.arrow_forwardIdentify each pair that could form a buffer. (a) HCl and CH3COOH (b) NaH2PO4 and Na2HPO4 (c) H2CO3 and NaHCO3arrow_forwardDoes the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?arrow_forward
- A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forwardThe composition diagram, or alpha plot, for the important acid-base system of carbonic acid, H2CO3, is illustrated. (See Study Question 1.7 for more information on such diagrams.) (a) Explain why the fraction of bicarbonate ion, HCO3, rises and then falls as the pH increases. (b) What is the composition of the solution when the pH is 6.0? When the pH is 10.0? (c) If you wanted to buffer a solution at a pH of 11.0, what should be the ratio of HCO3 to CO32?arrow_forward
- A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?arrow_forwardWhich of the following combinations could not be used to make an effective buffer? O NH4CI and NH3 O HNO2 and NANO2 O NAHSO3 and Na,SO4 O CH,CO,H and NaCH,CO,arrow_forwardA solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka propionic acid = 1.4 x 10^-5 ). a) calculate the moles of the reactants. Which is the limiting reactant? b) What will be the moles of the products? What are the moles of the excess reactant? c) calculate the pH of the acid bufferarrow_forward
- The solution started out clear, but when the 12 M HCl was added, lots of the white solid formed. The second round of the eight drops of HCl were added, which produced more white solid taking up most the volume of the test tube. Using the equation and Le Chatelier’s principle, what happened when the HCl was added to the reaction?arrow_forwardA solution is prepared that is initially 0.087 M in benzoic acid (HC6H5CO2) and 0.11 M in potassium benzoate (KC6H5CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. User to stand for the unknown change in [H3O+] You can leave out the M symbol for molarityarrow_forwardYou make 1.00 L of a buffered solution (pH=4.20) by mixing acetic acid and sodium acetate. You have 1.00 M solutions of each component of the buffered solution. What volume of each solution do you mix to make such a buffered solution? ( Ka for acetic acid is 1.8x10^-5) Volume of acetic acid = L Volume of sodium acetate= Larrow_forward
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