Chemical Principles
8th Edition
ISBN: 9781337247269
Author: Steven S. Zumdahl; Donald J. DeCoste
Publisher: Cengage Learning US
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Chapter 8, Problem 42E
What volumes of
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A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN = 9.20.
a) What volume of 0.100 mol L-1 HCl will be required to fully react with the above salt?
b) After the reaction in part (a) takes place, will the pH of the solution be acidic, basic or neutral?
c) What volume of 0.100 mol L-1 HCl is needed to adjust the pH of the originally provided solution to pH = 9.00? HINT: At pH 9.00, what kind of solution is created if the pKa of HCN is 9.20
A solution NH 3 that contains 78 mL of 0.043 M ammonia, NH 3, is titrated with 0.083 M HCI. The K₁ of ammonia is 1.8×10-5.
(a) What volume of 0.083 M HCI would be added to reach the equivalence point? Give the volume in mL.
40.41
mL
(b) At the equivalence point, what is the pH of the solution? (Assume that volumes are additive.)
4.56
A solution NH3 that contains 72 mL of 0.043 M ammonia, NH3, is titrated with 0.083 M HCl. The Kb of ammonia is 1.8x10-5.
(a) What volume of 0.083 M HCI would be added to reach the equivalence point? Give the volume in mL.
49 37
mL
(b) At the equivalence point, what is the pH of the solution? (Assume that volumes are additive.)
40
8.98
X
whawhat "at onubralence point" implies about the quantities of the combined acids and bases? Did you remember
Chapter 8 Solutions
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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- The equilibrium equations and Ka values for three reaction systems are given below. H2C2O4(aq)+H2OH3O+(aq)+HC2O4(aq);Ka=5.6102H3PO4(aq)+H2OH3O+(aq)+H2PO4(aq);Ka=6.9103HCOOH(aq)+H2OH3O+(aq)+HCOO(aq);Ka=1.7104 a Which conjugate pair would be best for preparing a buffer with a pH of 2.88? b How would you prepare 50 mL of a buffer with a pH of 2.88 assuming that you had available 0.10 M solutions of each pair?arrow_forwardWhat is the concentration of hydroxide ion in a 0.060 M aqueous solution of methylamine. CH3NH2? What is the pH?arrow_forwardWeak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/Aarrow_forward
- What volume of 0.120 M NaOH must be added to 100. mL of 0.100 M NaHC2O4 to reach a pH of 4.70?arrow_forwardAn important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?arrow_forwardA buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.arrow_forward
- What is the pH of a solution obtained by adding 13.0 g of NaOH to 795 mL of a 0.200 M solution of Sr(OH)2? Assume no volume change after NaOH is added.arrow_forwardAn important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. Consider blood with a pH of 7.44. a What is the ratio of [H2PO4] to [HPO42]? b What does the pH become if 25% of the hydrogen phosphate ions are converted to dihydrogen phosphate ion? c What does the pH become if 15% of the dihydrogen phosphate ions are converted to hydrogen phosphate ions?arrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forward
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