LCPO CHEMISTRY W/MODIFIED MASTERING
8th Edition
ISBN: 9780135214756
Author: Robinson
Publisher: PEARSON
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Chapter 17, Problem 17.74SP
Interpretation Introduction
Interpretation:
The value of blood pH from the given data needs to be determined.
Concept introduction:
The pH is a measure of acidity or alkalinity of water soluble substance, or mathematically, pH is the negative logarithm of the molar hydrogen ion concentration.
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Complete the following table. The only density needed is already given. Show your
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LOCH 3
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Kumada Coupling:
1. m-Diisobutylbenzene below could hypothetically be synthesized by Friedel-Crafts reaction. Write out the reaction with a
mechanism and give two reasons why you would NOT get the desired product.
Draw the reaction (NOT a mechanism) for a Kumada coupling to produce the molecule above from m-dichlorobenzene.
Calculate the theoretical yield for the reaction in question 2 using 1.5 g of p-dichlorobenzene and 3.0 mL isobutyl bromide.
What signals appeared/disappeared/shifted that indicate that you have your intended product and not starting material? What
other impurities are present in your product and how do you know?
Wintergreen from Aspirin:
1. In isolating the salicylic acid, why is it important to press out as much of the water as possible?
2. Write the mechanism of the esterification reaction you did.
3.
What characteristic absorption band changes would you expect in the IR spectrum on going from aspirin to salicyclic acid and
then to methyl salicylate as you did in the experiment today? Give approximate wavenumbers associated with each functional
group change.
What signals appeared/disappeared/shifted that indicate that you have your intended product and not starting material? What
other impurities are present in your product and how do you know?
Chapter 17 Solutions
LCPO CHEMISTRY W/MODIFIED MASTERING
Ch. 17 - Write a balanced net ionic equation for the...Ch. 17 - APPLY 16.2 Write balanced net ionic equations for...Ch. 17 - PRACTICE 16.3 Calculate the concentrations of all...Ch. 17 - APPLY 16.4 Calculate the pH of a solution prepared...Ch. 17 - Conceptual PRACTICE 16.5 The following pictures...Ch. 17 - Conceptual APPLY 16.6 The following pictures...Ch. 17 - Calculate the pH of 0.100 1 of a buffer solution...Ch. 17 - Calculate the change in pH when 0.002 mol of HNO3...Ch. 17 - PRACTICE 16.10 Use the Henderson-Hasselbalch...Ch. 17 - APPLY 16.11 The of the amine group of the amino...
Ch. 17 - PRACTICE 16.12 How would you prepare anbuffer...Ch. 17 - APPLY 16.13 Suppose you are performing an...Ch. 17 - A 40.0 mL volume of 0.100 M HCl is titrated with...Ch. 17 - APPLY 16.15 A 40.0 mL volume of 0.100 M NaOH is...Ch. 17 - What is the pH at the equivalence point in the...Ch. 17 - The following pictures represent solutions at...Ch. 17 - Assume that 40.0 mL of 0.0800...Ch. 17 - Assume that 40.0 mL of a 0.0250 M solution of the...Ch. 17 - Write the equilibrium-constant expression for...Ch. 17 - The following pictures represent solutions of...Ch. 17 - Prob. 17.21PCh. 17 - Ca2, which causes clotting, is removed from...Ch. 17 - What is the molar solubility of Ag2CrO4 in water...Ch. 17 - Prior to having an X-ray exam of the upper...Ch. 17 - Calculate the molar solubility of MgF2 , in...Ch. 17 - Calculate the molar solubility of Zn(OH)2 , in a...Ch. 17 - In an excess of NH3(aq),Cu2+ ion forms a deep blue...Ch. 17 - Cyanide ion is used in gold mining because it...Ch. 17 - Prob. 17.29PCh. 17 - Prob. 17.30ACh. 17 - Prob. 17.31PCh. 17 - Will a precipitate form on mixing 25 m1 of...Ch. 17 - Prob. 17.33PCh. 17 - Prob. 17.34PCh. 17 - HCO3 And CO32 are the primary ions in the ocean...Ch. 17 - Coral and the shells of marine organisms are made...Ch. 17 - The following reactions represent the dissolution...Ch. 17 - Prob. 17.38CPCh. 17 - The following pictures represent initial...Ch. 17 - Prob. 17.40CPCh. 17 - The following plot shows two pH titration curves,...Ch. 17 - Prob. 17.42CPCh. 17 - The following pictures represent solutions at...Ch. 17 - Prob. 17.44CPCh. 17 - Prob. 17.45CPCh. 17 - Prob. 17.46CPCh. 17 - 16.50 Is the pH greater than, equal to, or less...Ch. 17 - Is the pH greater than, equal to, or less than 7...Ch. 17 - Prob. 17.49SPCh. 17 - Prob. 17.50SPCh. 17 - Prob. 17.51SPCh. 17 - Prob. 17.52SPCh. 17 - 16.56 The equilibrium constant for the...Ch. 17 - 16.57 The equilibrium constant for the...Ch. 17 - 16.58 Does the pH increase, decrease, or remain...Ch. 17 - 16.59 Does the pH increase, decrease, or remain...Ch. 17 - 16.60 Calculate the pH of a solution that is 0.25...Ch. 17 - Prob. 17.58SPCh. 17 - Prob. 17.59SPCh. 17 - The pH of a solution of NH3 and NH4Br is 8.90....Ch. 17 - Prob. 17.61SPCh. 17 - Prob. 17.62SPCh. 17 - Prob. 17.63SPCh. 17 - Which of the following gives a buffer solution...Ch. 17 - Prob. 17.65SPCh. 17 - Prob. 17.66SPCh. 17 - Prob. 17.67SPCh. 17 - Calculate the pH of a buffer solution prepared by...Ch. 17 - Prob. 17.69SPCh. 17 - Calculate the pH of 0.375 L of a 0.18 M acetic...Ch. 17 - Prob. 17.71SPCh. 17 - A food chemist studying the formation of lactic...Ch. 17 - Prob. 17.73SPCh. 17 - Prob. 17.74SPCh. 17 - Prob. 17.75SPCh. 17 - Give a recipe for preparing a CH3CO2HCH3C02NA Na...Ch. 17 - Prob. 17.77SPCh. 17 - Prob. 17.78SPCh. 17 - Consider a buffer solution that contains equal...Ch. 17 - Calculate the concentrations of NH4+ and NH3 and...Ch. 17 - Prob. 17.81SPCh. 17 - Make a rough plot of pH versus milliliters of acid...Ch. 17 - Prob. 17.83SPCh. 17 - Consider the titration of 50.0 mL of 0.116 M NaOH...Ch. 17 - Prob. 17.85SPCh. 17 - Consider the titration of 25.0 mL of 0.200 MHCO2H...Ch. 17 - On the same graph, sketch pH titration curves for...Ch. 17 - Prob. 17.88SPCh. 17 - A 100.0 mL sample of 0.100 M methylamine (...Ch. 17 - A 50.0 mL sample of 0.250 M ammonia (...Ch. 17 - Prob. 17.91SPCh. 17 - Prob. 17.92SPCh. 17 - Prob. 17.93SPCh. 17 - What is the pH at the equivalence point for the...Ch. 17 - Consider the titration of 50.0 mL of a 0.100 M...Ch. 17 - Prob. 17.96SPCh. 17 - Prob. 17.97SPCh. 17 - The titration of 0.02500 L of a diprotic acid...Ch. 17 - Prob. 17.99SPCh. 17 - Prob. 17.100SPCh. 17 - Prob. 17.101SPCh. 17 - Prob. 17.102SPCh. 17 - Prob. 17.103SPCh. 17 - Prob. 17.104SPCh. 17 - Prob. 17.105SPCh. 17 - Use the following solubility data to calculate a...Ch. 17 - Prob. 17.107SPCh. 17 - Prob. 17.108SPCh. 17 - Prob. 17.109SPCh. 17 - Prob. 17.110SPCh. 17 - Prob. 17.111SPCh. 17 - Prob. 17.112SPCh. 17 - Which of the following compounds are more soluble...Ch. 17 - Prob. 17.114SPCh. 17 - Consider saturated solutions of the slightly...Ch. 17 - Prob. 17.116SPCh. 17 - Is the solubility of Zn(OH)2 , increased,...Ch. 17 - Is the solubility of Fe(OH)3 increased, decreased,...Ch. 17 - Prob. 17.119SPCh. 17 - Prob. 17.120SPCh. 17 - Prob. 17.121SPCh. 17 - Prob. 17.122SPCh. 17 - Prob. 17.123SPCh. 17 - Calculate the molar solubility of Cr(OH)3 in 0.50...Ch. 17 - Zinc hydroxide, Zn(OH)2 = (kSP=4.11017) , is...Ch. 17 - Prob. 17.126SPCh. 17 - Prob. 17.127SPCh. 17 - “Hard” water contains alkaline earth cations such...Ch. 17 - Prob. 17.129SPCh. 17 - Prob. 17.130SPCh. 17 - Prob. 17.131SPCh. 17 - Prob. 17.132SPCh. 17 - Prob. 17.133SPCh. 17 - Prob. 17.134SPCh. 17 - Prob. 17.135SPCh. 17 - Using the qualitative analysis flowchart in Figure...Ch. 17 - Give a method for separating the following pairs...Ch. 17 - Prob. 17.138SPCh. 17 - Prob. 17.139SPCh. 17 - Prob. 17.140MPCh. 17 - Calculate the molar solubility of MnS in a 0.30 M...Ch. 17 - Prob. 17.142MPCh. 17 - A 100.0 mL sample of a solution that is 0.100 M in...Ch. 17 - A 0.0100mol sample of solid Cd(OH)2(Ksp=5.31015)...Ch. 17 - One type of kidney stone is a precipitate of...Ch. 17 - Prob. 17.146MPCh. 17 - Ethylenediamine ( NH2CH2CH2NH2 , abbreviated en)...Ch. 17 - A 40.0 mL sample of a mixture of HCI and H3PO4 was...Ch. 17 - A 1.000 L sample of HCI gas at 25 °C and 732.0 mm...Ch. 17 - Prob. 17.150MPCh. 17 - Consider the reaction that occurs on mixing 50.0...Ch. 17 - In qualitative analysis, Ca2+ and Ba2+ are...Ch. 17 - A railroad tank car derails and spills 36 tons of...Ch. 17 - Some progressive hair coloring products marketed...
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