CHEMISTRY 1111 LAB MANUAL >C<
1st Edition
ISBN: 9781307092097
Author: Chang
Publisher: MCG/CREATE
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Textbook Question
Chapter 16, Problem 16.45QP
The ionization constant Ka of an indicator HIn is 1.0 × 10−6. The color of the nonionized form is red and that of the ionized form is yellow. What is the color of this indicator in a solution whose pH is 4.00?
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redraw the flowchart with boxes and molecules written in them
Part I.
a) Elucidate
the structure of compound A using the following information.
• mass spectrum: m+ = 102, m/2=57
312=29
• IR spectrum:
1002.5
% TRANSMITTANCE
Ngg
50
40
30
20
90
80
70
60
MICRONS
5
8
9 10
12
13
14 15 16
19
1740 cm
M
10
0
4000
3600
3200
2800
2400
2000
1800
1600
13
• CNMR
'H
-NMR
Peak
8
ppm (H)
Integration
multiplicity
a
1.5 (3H)
triplet
b
1.3
1.5 (3H)
triplet
C
2.3
1 (2H)
quartet
d
4.1
1 (2H)
quartet
& ppm (c)
10
15
28
60
177 (C=0)
b) Elucidate the structure of compound B using the following information
13C/DEPT NMR 150.9 MHz
IIL
1400
WAVENUMBERS (CM-1)
DEPT-90
DEPT-135
85 80 75
70
65
60
55
50
45 40
35
30 25 20
ppm
1200
1000
800
600
400
•
Part II.
a) Elucidate The structure of compound c w/ molecular formula C10 11202 and the following data below:
• IR spectra
% TRANSMITTANCE
1002.5
90
80
70
60
50
40
30
20
10
0
4000
3600
3200
2800
2400
2000
1800
1600
• Information from 'HAMR
MICRONS
8 9 10
11
14 15 16
19
25
1400
WAVENUMBERS (CM-1)
1200
1000
800
600
400
peak
8 ppm
Integration
multiplicity
a
2.1
1.5 (3H)
Singlet
b
3.6
1 (2H)
singlet
с
3.8
1.5 (3H)
Singlet
d
6.8
1(2H)
doublet
7.1
1(2H)
doublet
Information from 13C-nmR
Normal carbon
29ppm
Dept 135
Dept -90
+
NO peak
NO peak
50 ppm
55 ppm
+
NO peak
114 ppm
t
126 ppm
No peak
NO peak
130 ppm
t
+
159 ppm
No peak
NO peak
207 ppm
по реак
NO peak
Chapter 16 Solutions
CHEMISTRY 1111 LAB MANUAL >C<
Ch. 16.2 - What is the pH of a solution containing 0.30 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 - 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. 16.5 - Referring to Table 16.1, specify which indicator...Ch. 16.5 - Under what conditions will the end point of an...
Ch. 16.6 - The diagrams (a)(d) represent solutions of AgCl,...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. 16.7 - 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. 16.9 - Is the solubility of the following compounds...Ch. 16.9 - Calculate whether or not a precipitate will form...Ch. 16.10 - Prob. 15PECh. 16.10 - Calculate the molar solubility of AgBr in a 1.0 M...Ch. 16.10 - Prob. 1RCCh. 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. 16.148IMECh. 16 - Aspirin is a weak acid with pKa = 3.5. What is the...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- What is/are the product(s) of the following reaction? Select all that apply. * HI A B C OD OH A B OH D Carrow_forwardIn the image, the light blue sphere represents a mole of hydrogen atoms, the purple or teal spheres represent a mole of a conjugate base. A light blue sphere by itself is H+. Assuming there is 2.00 L of solution, answer the following: The Ka of the left & right solution is? The pH of the left & right solution is? The acid on the left & right is what kind of acid?arrow_forwardNonearrow_forward
- Nonearrow_forwardNonearrow_forwardWhat spectral features allow you to differentiate the product from the starting material? Use four separate paragraphs for each set of comparisons. You should have one paragraph each devoted to MS, HNMR, CNMR and IR. 2) For MS, the differing masses of molecular ions are a popular starting point. Including a unique fragmentation is important, too. 3) For HNMR, CNMR and IR state the peaks that are different and what makes them different (usually the presence or absence of certain groups). See if you can find two differences (in each set of IR, HNMR and CNMR spectra) due to the presence or absence of a functional group. Include peak locations. Alternatively, you can state a shift of a peak due to a change near a given functional group. Including peak locations for shifted peaks, as well as what these peaks are due to. Ideally, your focus should be on not just identifying the differences but explaining them in terms of functional group changes.arrow_forward
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