Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 17.4, Problem 1PPA
Practice Problem
ATTEMPT
For the titration of 10.0 mL of 0.15 M acetic acid with 0.10 M sodium hydroxide, determine the pH when (a) 10.0 mL of base has been added, (b) 15.0 mL of base has been added, and (c) 20.0 mL of base has been added.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Assignment:
Answer the following:
Solve for the pH level of an ammonia buffer. Given that it contains 500.0 mL of 0.3701 M ammonia and 500.0 mL of 0.5496 M ammonium and the Kb of ammonia is 1.7 x 10-9
Homework:
Answer the following:
Solve for the pH level of an ammonia buffer. Given that it contains 500.0 mL of 0.4481 M ammonia and 500.0 mL of 0.5069 M ammonium and the given Ka of ammonia is 1.300 x 10-4
Time (sec.)
pH of distilled water
pH of buffered solution
20
7.99
8.61
40
7.46
8.43
60
7.15
8.31
80
6.75
8.22
100
6.54
8.16
120
6.39
8.10
140
6.22
8.05
160
6.11
8.01
180
6.03
7.97
Conclusion
Explain your observations from the data table.
Which resists a change in pH the most, water or the buffered solution? Give reasons.
When you blow into the water, the pH goes up. Is the solution becoming more basic or acidic?
A buffer is usually made of a weak acid and a weak base. When you blow into a buffer the pH doesn’t change. What do you think is happening?
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. 17.3 - Referring to the titration curve shown in Figure...Ch. 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
Knowledge Booster
Learn more about
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
- Homework: Answer the following: Solve for the pH level of an acetate buffer. Given that it contains 500.0 mL of 0.4481 M acetic acid and 500.0 mL of 0.5069 M acetate and the given Ka of acetic acid is 1.300 x 10-4arrow_forwardPractice Question 19. Consider the titration of 20.0 mL of 0.20 M NaOH with 0.1 M HCl, Calculate the initial pH and then the new PH after adding 10mL of HCLarrow_forwardWhat is the pH at the equivalence point in the titration of a 18.3 mL sample of a 0.302 M aqueous nitrous acid solution with a 0.362 M aqueous barium hydroxide solution?pH = Submit Answerarrow_forward
- Which of the following pairs of solutions will form a buffer? Select all that apply Group of answer choices 0.100 M HF and 0.100 M NaF 0.100 M HCl and 0.100 M NaCl 0.100 M NaCl and 0.100 M KCl 0.100 M HCN and 0.100 M LiCNarrow_forwardWhat is the pH of 1.00 L of the 0.100 M hydrofluoric acid–0.120 M fluoride ion buffer system described in Worked Example 10.16 after 0.020 mol of NaOH is added?arrow_forward(clear handwritten answer please) 29.0 mL sample of a 0.441 M aqueous hypochlorous acid solution is titrated with a 0.429 M aqueous barium hydroxide solution. What is the pH at the start of the titration, before any barium hydroxide has been added?arrow_forward
- please answer provide in text or type buffer is prepared by mixing 53.7g of NH3 and 53.7g of NH4Cl in 0.493 L of solution. What is the pH of this buffer, and what will the pH change to if 7.91 g of HCl is then added to the mixture?arrow_forwardtopic: Proper Use and Calibration of the pH meter Calibration is done using buffer solutions every time the pH meter is used. Why? explain plsarrow_forwardI am extremely confused as to the logic behind these conceptual/theory problems can you please add a lot of detail: Consider a buffer solution where [weak acid] > [conjugate base]. How is the pH of the solution related to the pka value of the weak acid? If [conjugate base] > [weak acid], how is pH related to pka?arrow_forward
- Titration Problem (This is a question where you need to submit your own answer. You can show your work so that you can get partial credit in case you do not get it correct.) What is the concentration of a NaOH solution that takes 23.7 mL to neutralize 20.0 mL of 0.500 M HCl solution?arrow_forwardHow titration technique can be used to determine the concentration of acetic acid in vinegar sample? (3 sentences)arrow_forwardOnly typed explanation otherwise leave it A buffer solution is prepared by mixing 200mL of 0.20M salt solution and 400mL of 0.20M acid solution. What is the concentration of the resulting buffer solution?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY