Chemistry
3rd Edition
ISBN: 9780073402734
Author: Julia Burdge
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Textbook Question
Chapter 17, Problem 13QP
The pH of a sodium acetate-acetic acid buffer is 4.50. Calculate the ratio
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A solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka propionic acid = 1.4 x 10^-5 ).
a) calculate the moles of the reactants. Which is the limiting reactant?
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Draw the Lewis Dot structure for the following diprotic acid: HOOC-(CH2)2-COOH. 46.3 mL of a 0.099 M solution of this acid is titrated to the equivalence point with 0.15 M KOH. Write the balanced equation for this reaction and determine the volume of the base needed to completely neutralize the acid.
Chapter 17 Solutions
Chemistry
Ch. 17.1 - Practice ProblemATTEMPT Determine the pH at 25°C...Ch. 17.1 - Practice ProblemBUILD Determine the pH at 25°C of...Ch. 17.1 - Prob. 1PPCCh. 17.1 - Which of the following would cause a decrease in...Ch. 17.1 - What is the pH of a solution prepared by adding 0...Ch. 17.2 - Practice Problem ATTEMPT
Calculate the pH of 1 L...Ch. 17.2 - Practice Problem BUILD
How much must be added to...Ch. 17.2 - Practice Problem CONCEPTUALIZE
The first diagram...Ch. 17.2 - 17.2.1 Which of the following combinations can be...Ch. 17.2 - What is the pH of a buffer that is 0.76 M in HF...
Ch. 17.2 - 17.2.3 Consider 1 L of a buffer that is 0.85 M in...Ch. 17.2 - Consider 1 L of a buffer that is 1.5 M in...Ch. 17.2 - The solutions shown contain one or more of the...Ch. 17.2 - Prob. 6CPCh. 17.3 - Practice ProblemATTEMPT Select an appropriate acid...Ch. 17.3 - Prob. 1PPBCh. 17.3 - Practice ProblemCONCEPTUALIZE The diagrams...Ch. 17.3 - 17.3.1 For which of the following titrations will...Ch. 17.3 - 17.3.2 Calculate the pH at the equivalence point...Ch. 17.3 - Prob. 3CPCh. 17.3 - Calculate the pH after the addition of 35 mL of...Ch. 17.3 - Prob. 5CPCh. 17.3 - Prob. 6CPCh. 17.3 - Prob. 7CPCh. 17.3 - Prob. 8CPCh. 17.4 - Practice ProblemATTEMPT For the titration of 10.0...Ch. 17.4 - Practice ProblemBUILD For the titration of 25.0 mL...Ch. 17.4 - Prob. 1PPCCh. 17.4 - Prob. 1CPCh. 17.4 - Prob. 2CPCh. 17.4 - Prob. 3CPCh. 17.4 - Prob. 4CPCh. 17.4 - Prob. 5CPCh. 17.5 - Practice Problem ATTEMPT Calculate the pH at the...Ch. 17.5 - Practice Problem BUILD
A 50.0-mL quantity of a...Ch. 17.5 - Prob. 1PPCCh. 17.5 - 17.5.1 Calculate the molar solubility of AgCl in...Ch. 17.5 - Prob. 2CPCh. 17.5 - Prob. 3CPCh. 17.6 - Practice Problem ATTEMPT
Referring to Table 17.3,...Ch. 17.6 - Practice Problem BUILD
For which of the bases in...Ch. 17.6 - Practice Problem CONCEPTUALIZE
The diagram shows...Ch. 17.6 - Prob. 1CPCh. 17.6 - 17.6.2 Barium nitrate is added slowly to a...Ch. 17.7 - Prob. 1PPACh. 17.7 - Prob. 1PPBCh. 17.7 - Prob. 1PPCCh. 17.8 - Prob. 1PPACh. 17.8 - Prob. 1PPBCh. 17.8 - Prob. 1PPCCh. 17.9 - Prob. 1PPACh. 17.9 - Practice Problem BUILD What is the maximum mass...Ch. 17.9 - Prob. 1PPCCh. 17.10 - Practice ProblemATTEMPT Calculate the molar...Ch. 17.10 - Practice ProblemBUILD Arrange the following salts...Ch. 17.10 - Practice Problem CONCEPTUALIZE The diagram on the...Ch. 17.11 - Practice Problem ATTEMPT Determine if the...Ch. 17.11 - Practice Problem BUILD
Other than those in Sample...Ch. 17.11 - Practice Problem CONCEPTUALIZE
If an ionic...Ch. 17.12 - Practice ProblemATTEMPT In the presence of aqueous...Ch. 17.12 - Prob. 1PPBCh. 17.12 - Prob. 1PPCCh. 17.13 - Practice ProblemATTEMPT Lead(II) nitrate is added...Ch. 17.13 - Prob. 1PPBCh. 17.13 - Prob. 1PPCCh. 17 - Which of the acids in Table 16.6 can be used to...Ch. 17 - What molar ratio of sodium cyanide to hydrocyanic...Ch. 17 - How many moles of sodium benzoate must be added to...Ch. 17 - How much sodium fluoride must be dissolved in 250...Ch. 17 - Use Le Châtelier’s principle to explain how the...Ch. 17 - 17.2 Describe the effect on pH (increase,...Ch. 17 - Prob. 3QPCh. 17 - The p K a values of two monoprotic acids HA and HB...Ch. 17 - 17.5 Determine the pH of (a) a solution and (b) a...Ch. 17 - Determine the pH of (a) a 0 .20 M NH 3 solution,...Ch. 17 - Prob. 7QPCh. 17 - Prob. 8QPCh. 17 - Prob. 9QPCh. 17 - Prob. 10QPCh. 17 - Prob. 11QPCh. 17 - 17.12 What is the pH of the buffer
Ch. 17 - The pH of a sodium acetate-acetic acid buffer is...Ch. 17 - The pH of blood plasma is 7.40. Assuming the...Ch. 17 - 17.15 Calculate the pH of the buffer. What is the...Ch. 17 - 17.16 Calculate the of 1.00 L of the buffer ...Ch. 17 - Which of the following solutions can act as a...Ch. 17 - Which of the following solutions can act as a...Ch. 17 - A diprotic acid. H 2 A , has the following...Ch. 17 - Prob. 20QPCh. 17 - 17.21 The following diagrams contain one or more...Ch. 17 - The following diagrams represent solutions...Ch. 17 - Briefly describe what happens in an acid-base...Ch. 17 - Prob. 24QPCh. 17 - Explain how an acid-base indicator works in a...Ch. 17 - Prob. 26QPCh. 17 - A 0.2688-g sample of a monoprotic acid neutralizes...Ch. 17 - Prob. 28QPCh. 17 - 17.29 In a titration experiment, 12.5 mL of ...Ch. 17 - 17.30 In a titration experiment. 20.4 mL of 0.883...Ch. 17 - A 0.1276-g sample of an unknown monoprotic acid...Ch. 17 - Prob. 32QPCh. 17 - Calculate the pH at the equivalence point for the...Ch. 17 - Calculate the pH at the equivalence point for the...Ch. 17 - 17.35 A 25.0-mL solution of 0.100 M is titrated...Ch. 17 - 17.36 A 10.0-ml solution of 0.300 M is titrated...Ch. 17 - Prob. 37QPCh. 17 - Prob. 38QPCh. 17 - 17.39 The ionization constant of an indicator is...Ch. 17 - The K a of a certain indicator is 2.0 × 10 − 6 ....Ch. 17 - 17.41 The following diagrams represent solutions...Ch. 17 - The following diagrams represent solutions at...Ch. 17 - Use BaS O 4 to distinguish between the terms...Ch. 17 - 17.44 Why do we usually not quote the values for...Ch. 17 - 17.45 Write balanced equations and solubility...Ch. 17 - 17.46 Write the solubility product expression for...Ch. 17 - How can we predict whether a precipitate will form...Ch. 17 - 17.48 Silver chloride has a larger than silver...Ch. 17 - 17.49 Calculate the concentration of ions in the...Ch. 17 - From the solubility data given, calculate the...Ch. 17 - The molar solubility of MnCO 3 is 4 .2 × 10 -6 M ....Ch. 17 - The solubility of an ionic compound MX ( molar...Ch. 17 - The solubility of an ionic compound M 2 X 3 (...Ch. 17 - Using data from Table 17.4, calculate the molar...Ch. 17 - What is the pH of a saturated zinc hydroxide...Ch. 17 - The pH of a saturated solution of a metal...Ch. 17 - If 20.0 mL of 0.10 M Ba ( NO 3 ) 2 is added to...Ch. 17 - 17.58 A volume of 75 mL of 0.060 M NaF is mixed...Ch. 17 - 17.59 How does the common ion effect influence...Ch. 17 - The molar solubility of AgCl in 6.5 × 10 − 3 M...Ch. 17 - 17.61 Give an example to illustrate the general...Ch. 17 - How many grams of CaCO 3 will dissolve in 3 .0 ×...Ch. 17 - The solubility product of PbBr 2 is 8 .9 × 10 -6 ....Ch. 17 - Calculate the molar solubility of AgCl in a 1.00-L...Ch. 17 - 17.65 Calculate the molar solubility of in (a)...Ch. 17 - Which of the following ionic compounds will be...Ch. 17 - Which of the following will be more soluble in...Ch. 17 - Compare the molar solubility of Mg ( OH ) 2 in...Ch. 17 - Calculate the molar solubility of Fe ( OH ) 2 in a...Ch. 17 - 17.70 The solubility product of . What minimum ...Ch. 17 - Calculate whether or not a precipitate will form...Ch. 17 - 17.72 If 2.50 g of is dissolved in what are the...Ch. 17 - Calculate the concentrations of Cd 2+ , Cd ( CN )...Ch. 17 - If NaOH is added to 0 .010 M Al 3+ . which will be...Ch. 17 - Calculate the molar solubility of AgI in a 1 .0 M...Ch. 17 - Both Ag - and Zn 2- form complex ions with NH 3 ....Ch. 17 - 17.77 Explain, with balanced ionic equations, why...Ch. 17 - Outline the general procedure of qualitative...Ch. 17 - Give two examples of metal ions m each group (1...Ch. 17 - Solid NaI is slowly added to a solution that is 0...Ch. 17 - Find the approximate pH range suitable for the...Ch. 17 - 17.82 In a group 1 analysis, a student obtained a...Ch. 17 - 17.83 In a group 1 analysis, a student adds acid...Ch. 17 - Both KCl and XH 4 Cl are white solids. Suggest one...Ch. 17 - Describe a simple test that would allow you to...Ch. 17 - 17.86 The buffer range is defined by the equation...Ch. 17 - The p K a of the indicator methyl orange is 3.46....Ch. 17 - 17.88 Sketch the titration curve of a weak acid...Ch. 17 - A 200-mL volume of KaOH solution was added to 400...Ch. 17 - 17.90 The of butyric acid (HBut) is 4.7....Ch. 17 - A solution is made by mixing exactly 500 mL of...Ch. 17 - The titration curve shown here represents the...Ch. 17 - Cd ( OH ) 2 is an insoluble compound. It dissolves...Ch. 17 - A student mixes 50 .0 mL of 1 .00 M Ba ( OH ) 2...Ch. 17 - For which of the following reactions is the...Ch. 17 - Water containing Ca 2+ and Mg 2+ ions is called...Ch. 17 - Equal volumes of 0 .12 M AgNO 3 and 0 .14 M ZnCl 2...Ch. 17 - Find the approxite pH range suitable for...Ch. 17 - 17.99 Calculate the solubility (in g/L) of
Ch. 17 - 17.100 A volume of is titrated against a ...Ch. 17 - Prob. 101APCh. 17 - 17.102 When a KI solution was added to a solution...Ch. 17 - Which of the following compounds, when added to...Ch. 17 - The p K a of phenolphthalein is 9.10. Over what pH...Ch. 17 - Solid NaBr is slowly added to a solution that is...Ch. 17 - 17.106 Cacodylic acid is . Us ionization constant...Ch. 17 - Prob. 107APCh. 17 - Prob. 108APCh. 17 - Prob. 109APCh. 17 - CaSO 4 ( K sp = 2.4 × 10 − 5 ) has a larger K sp...Ch. 17 - Describe how you would prepare 1 − L0 .20 M CH 3...Ch. 17 - Phenolphthalein is the common indicator for the...Ch. 17 - Prob. 113APCh. 17 - 17.114 The molar mass of a certain metal...Ch. 17 - Consider the ionization of the following acid-base...Ch. 17 - One way to distinguish a buffer solution with an...Ch. 17 - 17.117 (a) Referring to Figure 17.4. describe how...Ch. 17 - AgNO 3 is added slowly to a solution that contains...Ch. 17 - The follwing diagrams represent solutions of MX,...Ch. 17 - 17.120 A 2.0-L kettle contains 116 g of boiler...Ch. 17 - 17.121 Radiochemical techniques are useful in...Ch. 17 - 17.122 One of the most common antibiotics is...Ch. 17 - 17.123 Barium is a toxic substance that can...Ch. 17 - 17.124 Tris [tris(hydroxymethyl)aminomethane] is a...Ch. 17 - Calcium oxalate is a major component of kidney...Ch. 17 - Histidine is one of the 20 amino acids found in...Ch. 17 - Amino acids are building blocks of proteins. These...Ch. 17 - 17.128 Oil paintings containing lead(II) compounds...Ch. 17 - 17.129 The maximum allowable concentration of ...Ch. 17 - Prob. 130APCh. 17 - When lemon juice is added to tea. the color...Ch. 17 - How many milliliters of 1.0 M NaOH must be added...Ch. 17 - Prob. 133APCh. 17 - Distribution curves show how the fractions of a...Ch. 17 - 17.135 A 1.0-L saturated silver carbonate solution...Ch. 17 - Draw distribution curves for an aqueous carbonic...Ch. 17 - 17.137 Acid-base reactions usually go to...Ch. 17 - Calculate x, the number of molecules of water in...Ch. 17 - Prob. 1SEPPCh. 17 - Aqueous acid reacts with carbonate Jons to produce...Ch. 17 - Aqueous acid reacts with carbonate Jons to produce...Ch. 17 - Prob. 4SEPP
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- Briefly describe how a buffer solution can control the pH of a solution when strong acid is added and when strong base is added. Use NH3/NH4Cl as an example of a buffer and HCl and NaOH as the strong acid and strong base.arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardWhat 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_forward
- A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?arrow_forwardIdentify each pair that could form a buffer. (a) HCl and CH3COOH (b) NaH2PO4 and Na2HPO4 (c) H2CO3 and NaHCO3arrow_forward8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.arrow_forward
- Identify 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_forwardPhenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?arrow_forwardConsider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.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_forwardMixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain. How does the amount of each solution added change the effectiveness of the buffer?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_forward
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