Chemistry
13th Edition
ISBN: 9781260162370
Author: Chang
Publisher: MCG
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Textbook Question
Chapter 16, Problem 16.52QP
Silver chloride has a larger Ksp than silver carbonate (see Table 16.2). Does this mean that AgCl also has a larger molar solubility than Ag2CO3?
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LTS
Solid:
AT=Te-Ti
Trial 1
Trial 2
Trial 3
Average
ΔΗ
Mass water, g
24.096
23.976
23.975
Moles of solid, mol
0.01763
001767
0101781
Temp. change, °C
2.9°C
11700
2.0°C
Heat of reaction, J
-292.37J -170.473
-193.26J
AH, kJ/mole
16.58K 9.647 kJ 10.85 kr
16.58K59.64701
KJ
mol
12.35k
Minimum AS,
J/mol K
41.582
mol-k
Remember: q = mCsAT (m = mass of water, Cs=4.184J/g°C) & qsin =-qrxn &
Show your calculations for:
AH in J and then in kJ/mole for Trial 1:
qa (24.0969)(4.1845/g) (-2.9°C)=-292.37J
qsin =
qrxn =
292.35 292.37J
AH in J = 292.375 0.2923kJ
0.01763m01
=1.65×107
AH in kJ/mol =
=
16.58K
0.01763mol
mol
qrx
Minimum AS in J/mol K (Hint: use the average initial temperature of the three trials, con
Kelvin.)
AS=AHIT
(1.65×10(9.64×103) + (1.0
Jimai
For the compound: C8H17NO2
Use the following information to come up with a plausible structure:
8
This compound has "carboxylic acid amide" and ether functional groups.
The peaks at 1.2ppm are two signals that are overlapping one another.
One of the two signals is a doublet that represents 6 hydrogens; the
other signal is a quartet that represents 3 hydrogens.
Vnk the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest bolling
point, choose 2 next to the substance with the next highest boiling point, and so on.
substance
C
D
chemical symbol,
chemical formula
or Lewis structure.
CH,-N-CH,
CH,
H
H 10: H
C-C-H
H H H
Cale
H 10:
H-C-C-N-CH,
Bri
CH,
boiling point
(C)
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Chapter 16 Solutions
Chemistry
Ch. 16.2 - What is the pH of a solution containing 0.30 M...Ch. 16.2 - Prob. 1RCFCh. 16.2 - What is the pH of a solution containing 0.25 M...Ch. 16.3 - Which of the following couples are buffer systems:...Ch. 16.3 - Calculate the pH of the 0.30 M NH3/0.36 M NH4Cl...Ch. 16.3 - How would you prepare a liter of carbonate buffer...Ch. 16.3 - Calculate the pH of the 0.40 M HF/0.48 M KF buffer...Ch. 16.3 - The diagrams (a)(d) represent solutions containing...Ch. 16.4 - Exactly 100 mL of 0.10 M nitrous acid (HNO2) are...Ch. 16.4 - Calculate the pH at the equivalence point in the...
Ch. 16.4 - For which of the following titrations will the pH...Ch. 16.4 - Calculate the pH at the equivalence point in the...Ch. 16.4 - calculate the pH in the titration of 50.0 mL of...Ch. 16.5 - Referring to Table 16.1, specify which indicator...Ch. 16.5 - Under what conditions will the end point of an...Ch. 16.6 - The solubility of lead chromate (PbCrO4) is 4.5 ...Ch. 16.6 - Calculate the solubility of silver chloride (AgCl)...Ch. 16.6 - Prob. 10PECh. 16.6 - Prob. 1RCFCh. 16.6 - Will a precipitate form when 50.0 mL of 0.0100 M...Ch. 16.6 - The diagrams (a)(d) represent solutions of AgCl,...Ch. 16.7 - The solubility products of AgCl and Ag3PO4 are 1.6...Ch. 16.7 - AgNO3 is slowly added to a solution that contains...Ch. 16.8 - Prob. 12PECh. 16.8 - Calculate the molar solubility of CaF2 in 0.0015 M...Ch. 16.9 - Is the solubility of the following compounds...Ch. 16.9 - Calculate whether or not a precipitate will form...Ch. 16.9 - Prob. 1RCFCh. 16.10 - Prob. 15PECh. 16.10 - Calculate the molar solubility of AgBr in a 1.0 M...Ch. 16.10 - Prob. 1RCFCh. 16.11 - An aqueous solution contains both Zn2+ and Pb2+...Ch. 16 - Use Le Chteliers principle to explain how the...Ch. 16 - Describe the effect on pH (increase, decrease, or...Ch. 16 - The pKas of two monoprotic acids HA and HB are 5.9...Ch. 16 - Determine the pH of (a) a 0.40 M CH3COOH solution,...Ch. 16 - Determine the pH of (a) a 0.20 M NH3 solution, (b)...Ch. 16 - What is a buffer solution? What constitutes a...Ch. 16 - Which of the following has the greatest buffer...Ch. 16 - Which of the following solutions can act as a...Ch. 16 - Which of the following solutions can act as a...Ch. 16 - Calculate the pH of the buffer system made up of...Ch. 16 - Calculate the pH of the following two buffer...Ch. 16 - The pH of a bicarbonate-carbonic acid buffer is...Ch. 16 - What is the pH of the buffer 0.10 M Na2HPO4/0.15 M...Ch. 16 - The pH of a sodium acetateacetic acid buffer is...Ch. 16 - The pH of blood plasma is 7.40. Assuming the...Ch. 16 - Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl...Ch. 16 - Calculate the pH of 1.00 L of the buffer 1.00 M...Ch. 16 - A student is asked to prepare a buffer solution at...Ch. 16 - The diagrams (a)(d) contain one or more of the...Ch. 16 - The diagrams shown here represent solutions...Ch. 16 - How much NaOH (in moles) must be added to 1 L of a...Ch. 16 - How much HCl (in moles) must be added to 1 L of a...Ch. 16 - Briefly describe what happens in an acid-base...Ch. 16 - Sketch titration curves for the following...Ch. 16 - A 0.2688-g sample of a monoprotic acid neutralizes...Ch. 16 - A 5.00-g quantity of a diprotic acid was dissolved...Ch. 16 - In a titration experiment, 12.5 mL of 0.500 M...Ch. 16 - In a titration experiment, 20.4 mL of 0.883 M...Ch. 16 - A 0.1276-g sample of an unknown monoprotic acid...Ch. 16 - A solution is made by mixing 5.00 102 mL of 0.167...Ch. 16 - Calculate the pH at the equivalence point for the...Ch. 16 - Calculate the pH at the equivalence point for the...Ch. 16 - A 25.0-mL solution of 0.100 M CH3COOH is titrated...Ch. 16 - A 10.0-mL solution of 0.300 M NH3 is titrated with...Ch. 16 - The diagrams shown here represent solutions at...Ch. 16 - Prob. 16.38QPCh. 16 - A 0.054 M HNO2 solution is titrated with a KOH...Ch. 16 - A student titrates an unknown monoprotic acid with...Ch. 16 - Explain how an acid-base indicator works in a...Ch. 16 - The amount of indicator used in an acid-base...Ch. 16 - Referring to Table 16.1, specify which indicator...Ch. 16 - A student carried out an acid-base titration by...Ch. 16 - The ionization constant Ka of an indicator HIn is...Ch. 16 - Use BaSO4 to distinguish between solubility, molar...Ch. 16 - Why do we usually not quote the Ksp values for...Ch. 16 - Write balanced equations and solubility product...Ch. 16 - Write the solubility product expression for the...Ch. 16 - How can we predict whether a precipitate will form...Ch. 16 - Silver chloride has a larger Ksp than silver...Ch. 16 - From the solubility data given, calculate the...Ch. 16 - The molar solubility of MnCO3 is 4.2 106 M. What...Ch. 16 - The solubility of an ionic compound MX (molar mass...Ch. 16 - The solubility of an ionic compound M2X3 (molar...Ch. 16 - Using data from Table 16.2, calculate the molar...Ch. 16 - Prob. 16.59QPCh. 16 - The pH of a saturated solution of a metal...Ch. 16 - If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL...Ch. 16 - A volume of 75 mL of 0.060 M NaF is mixed with 25...Ch. 16 - Solid NaI is slowly added to a solution that is...Ch. 16 - Find the approximate pH range suitable for the...Ch. 16 - How does the common ion effect influence...Ch. 16 - Prob. 16.66QPCh. 16 - How many grams of CaCO3 will dissolve in 3.0 102...Ch. 16 - The solubility product of PbBr2 is 8.9 106....Ch. 16 - Calculate the molar solubility of AgCl in a 1.00-L...Ch. 16 - Calculate the molar solubility of BaSO4 (a) in...Ch. 16 - Prob. 16.71QPCh. 16 - Which of the following will be more soluble in...Ch. 16 - Prob. 16.73QPCh. 16 - Calculate the molar solubility of Fe(OH)2 in a...Ch. 16 - The solubility product of Mg(OH)2 is 1.2 1011....Ch. 16 - Calculate whether or not a precipitate will form...Ch. 16 - If 2.50 g of CuSO4 are dissolved in 9.0 102 mL of...Ch. 16 - Calculate the concentrations of Cd2+, Cd(CN3)42,...Ch. 16 - If NaOH is added to 0.010 M Al3+, which will be...Ch. 16 - Calculate the molar solubility of AgI in a 1.0 M...Ch. 16 - Both Ag+ and Zn2+ form complex ions with NH3....Ch. 16 - Explain, with balanced ionic equations, why (a)...Ch. 16 - Outline the general procedure of qualitative...Ch. 16 - Give two examples of metal ions in each group (1...Ch. 16 - In a group 1 analysis, a student obtained a...Ch. 16 - In a group 1 analysis, a student adds HCl acid to...Ch. 16 - Both KCl and NH4Cl are white solids. Suggest one...Ch. 16 - Describe a simple test that would enable you to...Ch. 16 - To act as an effective buffer, the concentrations...Ch. 16 - The pKa of the indicator methyl orange is 3.46....Ch. 16 - The iodide impurity in a 4.50-g sample of a metal...Ch. 16 - A sodium acetate-acetic acid buffer solution was...Ch. 16 - Prob. 16.95QPCh. 16 - A 200-mL volume of NaOH solution was added to 400...Ch. 16 - The pKa of butyric acid (HBut) is 4.7. Calculate...Ch. 16 - A solution is made by mixing 5.00 102 mL of 0.167...Ch. 16 - Cd(OH)2 is an insoluble compound. It dissolves in...Ch. 16 - A student mixes 50.0 mL of 1.00 M Ba(OH)2 with...Ch. 16 - For which of the following reactions is the...Ch. 16 - A 2.0-L kettle contains 116 g of boiler scale...Ch. 16 - Equal volumes of 0.12 M AgNO3 and 0.14 M ZnCl2...Ch. 16 - Prob. 16.104QPCh. 16 - Prob. 16.105QPCh. 16 - A volume of 25.0 mL of 0.100 M HCl is titrated...Ch. 16 - The molar solubility of Pb(IO3)2 in a 0.10 M NaIO3...Ch. 16 - When a KI solution was added to a solution of...Ch. 16 - Barium is a toxic substance that can seriously...Ch. 16 - Prob. 16.110QPCh. 16 - Solid NaBr is slowly added to a solution that is...Ch. 16 - Cacodylic acid is (CH3)2AsO2H. Its ionization...Ch. 16 - Radiochemical techniques are useful in estimating...Ch. 16 - The molar mass of a certain metal carbonate, MCO3,...Ch. 16 - Acid-base reactions usually go to completion....Ch. 16 - Calculate x, which is the number of molecules of...Ch. 16 - Describe how you would prepare a 1-L 0.20 M...Ch. 16 - Prob. 16.118QPCh. 16 - Prob. 16.119QPCh. 16 - What reagents would you employ to separate the...Ch. 16 - Look up the Ksp values for BaSO4 and SrSO4 in...Ch. 16 - In principle, amphoteric oxides, such as Al2O3 and...Ch. 16 - Prob. 16.123QPCh. 16 - When lemon juice is squirted into tea, the color...Ch. 16 - How many milliliters of 1.0 M NaOH must be added...Ch. 16 - The maximum allowable concentration of Pb2+ ions...Ch. 16 - Which of the following solutions has the highest...Ch. 16 - Prob. 16.129QPCh. 16 - Water containing Ca2+ and Mg2+ ions is called hard...Ch. 16 - Prob. 16.131QPCh. 16 - Prob. 16.132QPCh. 16 - (a) Referring to Figure 16.6, describe how you...Ch. 16 - Prob. 16.135QPCh. 16 - One way to distinguish a buffer solution with an...Ch. 16 - Prob. 16.137QPCh. 16 - A sample of 0.96 L of HCl at 372 mmHg and 22C is...Ch. 16 - (a) Assuming complete dissociation and no ion-pair...Ch. 16 - Calculate the maximum mass (in grams) of each of...Ch. 16 - A 1.0-L saturated silver carbonate solution at 5C...Ch. 16 - The two curves shown represent the titration of...Ch. 16 - Prob. 16.143QPCh. 16 - A 100-mL 0.100 M CuSO4 solution is mixed with a...Ch. 16 - The titration curve shown represents the titration...Ch. 16 - The titration curve shown represents the titration...Ch. 16 - Use appropriate equations to account for the...Ch. 16 - Prob. 16.148QPCh. 16 - Aspirin is a weak acid with pKa = 3.5. What is the...
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