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 17.12, Problem 1PPA
Practice Problem
ATTEMPT
In the presence of aqueous ammonia, cobalt(III) forms the complex ion
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
31. Lead(II) iodide has a solubility product constant of 1.4 x
10-8. What is the concentration of I- in a saturated
solution of PbI2?
(A) 1.2 x 104 M
(B) 2.4 × 104 M
(C) 1.5 x 10-3 M
(D) 3.0 x 10-3 M
Give typed full explanation not a single word hand written otherwise leave it
Calculate the molar solubility of Mn(OH)2 in an aqueous solution buffered to a pH of 12.3. Ksp of Mn(OH)2 is 1.6x10-13.(a) 3.4 x 10-5 M(b) 8.0 x 10-12 M(c) 4.0 x 10-10 M(d) 6.4 x 1011 M
Cobalt(II) complex ion solution:
[Co(H20)s]*2(aq) + 4Cl (aq)
+ [COC14]?(aq) + 6H20(1)
Pink
Blue
(3) According to the first video
(a) What will happen when HCl is added ? That is in which direction the equilibrium
shifts and the conc of which cobalt compound increases and which one
decreases ?
(b) What will happen if instead of HCI , CaCl, is added ?
(c) What will happen when water is added to test tube (1) ? That is in which
direction the equilibrium shifts and the conc of which cobalt compound increases
and which one decreases ?
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
- nemistLI What is the approximate concentration of free Ni²+ ion at equilibrium when 1.61×10-2 mol nickel nitrate is added to 1.00 L of solution that is 1.010 M in CN. For [Ni(CN)41², Kf= 2.0x1031. [Ni²*] = M Submit Answerarrow_forwardCalculate the K, of the following compounds, given their molar solubilities. (a) CoS 6.31 x 10 M (b) Zn(OH)2. 1.95 x 10 M (c) Mg, (PO4)2, 6.20 x 10 M Submit Answer Retry Entire Group No more group attempts remainarrow_forwardPlease provide only typed answer solution no handwritten solution needed allowedarrow_forward
- Please fast solvearrow_forwardExplain how (in procedures step format), the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) and nickel(II) hydroxide. The mixture of Ni+2 and Fe+3 solution when NH3 is added Ni will form soluble complex but Fe+3 does not react with NH3 .arrow_forwardABP Question 15 of 15 A solution contains 0.040 M in Cu 2 and 0.30 M in CN. If the Kf for Cu(CN)4 2 is 1.0x 1025, how much copper ion remains at equilibrium? A) 2.9 × 10 26 M B) 8.8 × 10 25 M C) 1.0 × 10 23 M D) 1.5 x 10 26 M W e here to search DELL -arrow_forward
- AgBr has very low solubility in water. Then thiosulfate ion, S2O32-, is added to a solution containing silver ions, the silver ions form a complex ion with thiosulfate according to the equation shown. Ag+(aq) + 2S2O32–(aq) [Ag(S2O3)2] 3–(aq) If sodium thiosulfate is added to a saturated solution of AgBr in equilibrium with solid AgBr, how will the concentrations of Br–(aq) change? a. SBr precipitates b. [Br–(aq)] increases c. [Br–(aq)] decreases d. [Br–(aq)] does not changearrow_forwardYou have a solution consisting of 0.10 M PO4 3– and 0.10 M I - . You add 0.10 M silver nitrate dropwise to this solution. Given that the Ksp for AgI is 1.5 × 10–16 , and that for Ag3PO4 is 1.3 × 10–20 , which of the following will precipitate first? (show work) a) Silver iodide b) Silver Phosphate c) Silver Nitrate d) none of thesearrow_forwardA solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration valuearrow_forward
- What is the minimum pH at which Cd(OH)2(s) will precipitate from a solution that is 0.0055M in Cd2+(aq)? Ksp for Cd(OH)2(s) is 2.5*10-14. a)13.60 b) 11.70 c) 9.27 d) 12.20 e) 8.33arrow_forwardA solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) Use your correct answers from #7 to answer this question. What is Kf, the formation constant, for this complex?arrow_forwardA solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) What is Kf, the formation constant, for this complex?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY