EBK CHEMICAL PRINCIPLES
8th Edition
ISBN: 9781305856745
Author: DECOSTE
Publisher: CENGAGE LEARNING - CONSIGNMENT
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Chapter 8, Problem 93E
For which of the following is the
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Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base?
The pH will always be greater than 7, regardless of the acid and conjugate base.
The pH of the solution will be equal to the pKa of the acid.
The pH of the solution will be equal to Kw.
The pH will be equal to the concentration of the conjugate base.
The pH will be equal to the concentration of the acid.
Which of the following are capable of forming a buffer solution? Select the single best answer.
HNO3 and KNO3
NH3 and NH4Cl
Explain the difference between a buffered and an unbuffered solution.
How does the pH of an unbuffered solution change when an acid or base i
added to it? When a salt of a weak acid or weak base is added to it?
Chapter 8 Solutions
EBK CHEMICAL PRINCIPLES
Ch. 8 - Prob. 1DQCh. 8 - Prob. 2DQCh. 8 - Mixing together solutions of acetic acid and...Ch. 8 - Sketch two pH curves, one for the titration of a...Ch. 8 - Sketch a pH curve for the titration of a weak acid...Ch. 8 - You have a solution of the weak acid HA and add...Ch. 8 - You have a solution of the weak acid HA and add...Ch. 8 - Prob. 8DQCh. 8 - You are browsing through the Handbook of...Ch. 8 - A friend tells you: "The constant Ksp of a salt is...
Ch. 8 - What happens to the Ksp value of a solid as the...Ch. 8 - Which is more likely to dissolve in an acidic...Ch. 8 - Prob. 13DQCh. 8 - Under what circumstances can the relative...Ch. 8 - Define a buffered solution. What makes up a...Ch. 8 - A good buffer generally contains relatively equal...Ch. 8 - How many of the following are buffered solutions?...Ch. 8 - Which of the following can be classified as buffer...Ch. 8 - Prob. 19ECh. 8 - Derive an equation analogous to the Henderson—...Ch. 8 - Calculate the pH of each of the following...Ch. 8 - Calculate the pH after 0.020 mole of HCl is added...Ch. 8 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 8 - The results of Exercises 21-23 illustrate an...Ch. 8 - One of the most challenging parts of solving...Ch. 8 - a. Calculate the pH of a buffered solution that is...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH after 0.10mole of NaOH is added...Ch. 8 - Calculate the pH after 0.020mole of NaOH is added...Ch. 8 - Calculate the pH of a solution that is 0.40M H 2...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH of a buffered solution prepared...Ch. 8 - A buffered solution is made by adding...Ch. 8 - Prob. 35ECh. 8 - How many moles of NaOH must be added to...Ch. 8 - Calculate the number of moles of HCl(g) that must...Ch. 8 - You make 1.00L of a buffered solution (pH=4.00) by...Ch. 8 - Calculate the mass of sodium acetate that must be...Ch. 8 - Calculate the pH after 0.010mole of gaseous HCl is...Ch. 8 - An aqueous solution contains dissolved...Ch. 8 - What volumes of 0.50MHNO2and0.50MNaNO2 must be...Ch. 8 - Phosphate buffers are important in regulating the...Ch. 8 - Carbonate buffers are important in regulating the...Ch. 8 - When a person exercises, muscle contractions...Ch. 8 - Which of the following mixtures would result in a...Ch. 8 - Which of the following mixtures would result in a...Ch. 8 - Calculate the pH of a solution formed by mixing...Ch. 8 - Consider the acids in Table 7.2. Which acid would...Ch. 8 - Consider the bases in Table 7.3. Which base would...Ch. 8 - A solution contains 1.0106MHOCl and an unknown...Ch. 8 - In Section 8.3 an equation was derived for the...Ch. 8 - Consider a weak acid HA with a Ka value of 1.6107....Ch. 8 - Consider the following pH curves for 100.0mL of...Ch. 8 - An acid is titrated with NaOH. The following...Ch. 8 - Consider the titration of a generic weak acid HA...Ch. 8 - Sketch the titration curve for the titration of a...Ch. 8 - Draw the general titration curve for a strong acid...Ch. 8 - Consider the following four titrations:...Ch. 8 - A student titrates an unknown weak acid HA to a...Ch. 8 - The following plot shows the pH curves for the...Ch. 8 - The figure in the preceding exercise shows the pH...Ch. 8 - Consider the titration of...Ch. 8 - Prob. 64ECh. 8 - Prob. 65ECh. 8 - Prob. 66ECh. 8 - Prob. 67ECh. 8 - Prob. 68ECh. 8 - Prob. 69ECh. 8 - Prob. 70ECh. 8 - Calculate the pH at the halfway point and at the...Ch. 8 - You have 75.0mLof0.10MHA. After adding...Ch. 8 - A student dissolves 0.0100mole of an unknown weak...Ch. 8 - What is an acid—base indicator? Define the...Ch. 8 - Two drops of indicator HIn(Ka=1.0109), where HIn...Ch. 8 - A certain indicator HIn has a pKa of 3.00 and a...Ch. 8 - Estimate the pH of a solution in which bromcresol...Ch. 8 - A solution has a pHof7.0. What would be the color...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Methyl red has the following structure: It...Ch. 8 - Indicators can be used to estimate the pH values...Ch. 8 - When a diprotic acid, H2A, is titrated with NaOH,...Ch. 8 - A student was given a 0.10M solution of an unknown...Ch. 8 - Prob. 87ECh. 8 - Consider 100.0mLofa0.100M solution of...Ch. 8 - A 0.200-g sample of a triprotic acid...Ch. 8 - Consider the titration of 100.0mLof0.100MH3A...Ch. 8 - The titration of Na2CO3 with HCl has the following...Ch. 8 - Consider 100.0 mL of a solution of 0.200MNa2A,...Ch. 8 - For which of the following is the Ksp value of the...Ch. 8 - Ag2S(s) has a larger molar solubility than CuS...Ch. 8 - When Na3PO4(aq) is added to a solution containing...Ch. 8 - The common ion effect for ionic solids (salts) is...Ch. 8 - Prob. 97ECh. 8 - Calculate the solubility of each of the following...Ch. 8 - Use the following data to calculate the Ksp value...Ch. 8 - The concentration of Pb2+ in a solution saturated...Ch. 8 - The concentration of Ag+ in a solution saturated...Ch. 8 - The solubility of the ionic compound M2X3, having...Ch. 8 - For each of the following pairs of solids,...Ch. 8 - The solubility rules outlined in Chapter 4 say...Ch. 8 - Calculate the molar solubility of...Ch. 8 - The Ksp for silver sulfate (Ag2SO4) is 1.2105....Ch. 8 - Calculate the solubility (inmol/L) of Fe(OH)3...Ch. 8 - Prob. 108ECh. 8 - Calculate the solubility of solid Ca3(...Ch. 8 - The solubility of Ce( IO3)3 in a 0.20MKIO3...Ch. 8 - What mass of ZnS(Ksp=2.51022) will dissolve in...Ch. 8 - The concentration of Mg2+ in seawater is 0.052M....Ch. 8 - For the substances in Exercises 97and98, which...Ch. 8 - Explain the following phenomenon: You have a test...Ch. 8 - For which salt in each of the following groups...Ch. 8 - A solution is prepared by mixing 75.0mL of...Ch. 8 - Calculate the final concentrations of...Ch. 8 - A solution is prepared by mixing 50.0mLof0.10M Pb(...Ch. 8 - The Ksp of Al(OH)3 is 21032. At what pH will a...Ch. 8 - A solution is 1104M in NaF,Na2S, and Na3PO4. What...Ch. 8 - A solution contains 1.0105MNa3PO4. What is the...Ch. 8 - A solution contains 0.25MNi( NO3)2 and 0.25MCu(...Ch. 8 - Describe how you could separate the ions in each...Ch. 8 - If a solution contains either Pb2+(aq)orAg+(aq),...Ch. 8 - Sulfide precipitates are generally grouped as...Ch. 8 - Nanotechnology has become an important field, with...Ch. 8 - Prob. 127ECh. 8 - As a sodium chloride solution is added to a...Ch. 8 - The overall formation constant for HgI42is1.01030....Ch. 8 - A solution is prepared by adding 0.090mole of...Ch. 8 - Prob. 131ECh. 8 - Kf for the complex ion Ag( NH3)2+is1.7107. Ksp for...Ch. 8 - a. Using the Ksp for Cu(OH)2(1.61019) and the...Ch. 8 - The copper(I) ion forms a chloride salt that has...Ch. 8 - Solutions of sodium thiosulfate are used to...Ch. 8 - a. Calculate the molar solubility of AgI in pure...Ch. 8 - A series of chemicals was added to some...Ch. 8 - Will a precipitate of Cd(OH)2 form if 1.0mLof1.0M...Ch. 8 - Tris(hydroxymethyl)aminomethane, commonly called...Ch. 8 - Amino acids are the building blocks for all...Ch. 8 - The solubility of copper(II) hydroxide in water...Ch. 8 - The salts in Table 8.5, with the possible...Ch. 8 - You have the following reagents on hand: What...Ch. 8 - Prob. 144AECh. 8 - One method for determining the purity of aspirin...Ch. 8 - Another way to treat data from a pH titration is...Ch. 8 - Potassium hydrogen phthalate, known as KHP...Ch. 8 - sample of the ionic compound NaA, where A is the...Ch. 8 - What mass of Ca( NO3)2 must be added to 1.0L of a...Ch. 8 - The equilibrium constant for the following...Ch. 8 - Calculate the concentration of Pb2+ in each of the...Ch. 8 - Consider saturated solutions of the following...Ch. 8 - A certain acetic acid solution has pH=2.68 ....Ch. 8 - Calculate the volume of 1.5010-2MNaOH that must be...Ch. 8 - A 0.400M solution of ammonia was titrated with...Ch. 8 - A student intends to titrate a solution of a weak...Ch. 8 - The active ingredient in aspirin is...Ch. 8 - A solution is formed by mixing 50.0mL of 10.0MNaX...Ch. 8 - When phosphoric acid is titrated with a NaOH...Ch. 8 - Consider the following two acids: In two separate...Ch. 8 - Consider 1.0L of a solution that is 0.85MHOC6H5...Ch. 8 - What concentration of NH4Cl is necessary to buffer...Ch. 8 - Consider the following acids and bases:...Ch. 8 - Consider a buffered solution containing CH3NH3Cl...Ch. 8 - Consider the titration of 150.0mL of 0.100MHI by...Ch. 8 - Prob. 166AECh. 8 - Prob. 167AECh. 8 - Prob. 168AECh. 8 - Assuming that the solubility of Ca3( PO4)2(s) is...Ch. 8 - Order the following solids (ad) from least soluble...Ch. 8 - The Ksp for PbI2(s) is 1.410-8 . Calculate the...Ch. 8 - Prob. 172AECh. 8 - A 50.0-mL sample of 0.0413MAgNO3(aq) is added to...Ch. 8 - The Hg2+ ion forms complex ions with I as follows:...Ch. 8 - A buffer is made using 45.0mL of...Ch. 8 - What volume of 0.0100MNaOH must be added to 1.00L...Ch. 8 - For solutions containing salts of the form NH4X ,...Ch. 8 - Prob. 178CPCh. 8 - The copper(I) ion forms a complex ion with CN...Ch. 8 - Calcium oxalate (CaC2O4) is relatively insoluble...Ch. 8 - a. Calculate the molar solubility of SrF2 in...Ch. 8 - What is the maximum possible concentration of Ni2+...Ch. 8 - Prob. 183CPCh. 8 - Consider 1.0L of an aqueous solution that contains...Ch. 8 - Calculate the solubility of AgCN(s)(Ksp=2.21012)...Ch. 8 - Consider the titration of 100.0mL of a 1.00104M...Ch. 8 - Consider a solution formed by mixing 200.0mL of...Ch. 8 - Prob. 188CPCh. 8 - Calculate the pH of a solution prepared by mixing...Ch. 8 - Consider the titration of 100.0mL of 0.10M...Ch. 8 - In the titration of 100.0mL of a 0.0500M solution...Ch. 8 - Consider the titration curve in Exercise91 for the...Ch. 8 - Consider a solution prepared by mixing the...Ch. 8 - Prob. 194MP
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- What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.arrow_forwardWhat do you suppose happens to the Ksp, value of a solid as the temperature of the solution changes? Consider both increasing and decreasing temperatures, and explain your answer.arrow_forwardMethyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?arrow_forward
- A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?arrow_forwardFor which of the following is the Ksp value of the ionic compound the largest? The smallest? Explain your answer.arrow_forwardA solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.arrow_forward
- Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Clarrow_forwardConsider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0arrow_forwardYou have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you make up 0.10 M solutions by adding sufficient water to each of the acid samples. When you measure the pH of these samples, you find that the pH of HX is greater than the pH of HY, which in turn is greater than the pH of HZ. a Which of the acids is the least ionized in its solution? b Which acid has the largest Kd?arrow_forward
- 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?arrow_forward8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.arrow_forwardIdentify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forward
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