EP CHEMISTRY:CENTRAL..-MOD.MASTERING
14th Edition
ISBN: 9780136781509
Author: Brown
Publisher: PEARSON CO
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Chapter 4.2, Problem 4.4.2PE
Interpretation Introduction
To determine: The net ionic reaction for the precipitation reaction of silver nitrate and potassium phosphate.
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Can you please help mne with this problem. Im a visual person, so can you redraw it, potentislly color code and then as well explain it. I know im given CO2 use that to explain to me, as well as maybe give me a second example just to clarify even more with drawings (visuals) and explanations.
Part 1. Aqueous 0.010M AgNO 3 is slowly added to a 50-ml solution containing both carbonate [co32-] = 0.105 M
and sulfate [soy] = 0.164 M anions. Given the ksp of Ag2CO3 and Ag₂ soy below. Answer the ff:
Ag₂ CO3 = 2 Ag+ caq) + co} (aq)
ksp = 8.10 × 10-12
Ag₂SO4 = 2Ag+(aq) + soy² (aq) ksp = 1.20 × 10-5
a) which salt will precipitate first?
(b)
What % of the first anion precipitated will remain in the solution.
by the time the second anion starts to precipitate?
(c) What is the effect of low pH (more acidic) condition on the separate of the carbonate and
sulfate anions via silver precipitation? What is the effect of high pH (more basic)? Provide appropriate
explanation per answer
Part 4. Butanoic acid (ka= 1.52× 10-5) has a partition coefficient of 3.0 (favors benzene) when distributed bet.
water and benzene. What is the formal concentration of butanoic acid in each phase when
0.10M aqueous butanoic acid is extracted w❘ 25 mL of benzene
100 mL of
a) at pit 5.00
b) at pH 9.00
Chapter 4 Solutions
EP CHEMISTRY:CENTRAL..-MOD.MASTERING
Ch. 4.1 - If you have an aqueous solution that contains 1.5...Ch. 4.1 - If you were to draw diagrams representing aqueous...Ch. 4.2 - Prob. 4.2.1PECh. 4.2 - Classify the following compounds as soluble or...Ch. 4.2 - Yes or No: Will a precipitate form when solutions...Ch. 4.2 - a. What compound precipitates when aqueous...Ch. 4.2 - What happens when you mix an aqueous solution of...Ch. 4.2 -
Write the net ionic equation for the...Ch. 4.3 - Prob. 4.5.1PECh. 4.3 -
Imagine a diagram showing 10 Na + ions and 10 OH-...
Ch. 4.3 -
Which of these substances, when dissolved in...Ch. 4.3 - Consider solutions in which 0.1 mol of each of the...Ch. 4.3 -
Which is the correct ionic equation for the...Ch. 4.3 - For the reaction of phosphorous acid (H3PO3) and...Ch. 4.4 - Prob. 4.8.1PECh. 4.4 - What is the oxidation state of the boldfaced...Ch. 4.4 - Which of the following statements is true about...Ch. 4.4 - Prob. 4.9.2PECh. 4.4 - Which of these metals is the easiest to oxidize?...Ch. 4.4 - Which of the following metals will be oxidized by...Ch. 4.5 - Prob. 4.11.1PECh. 4.5 - Calculate the molarity of a solution made by...Ch. 4.5 - Prob. 4.12.1PECh. 4.5 - What is the molar concentration of K+ions in a...Ch. 4.5 - Prob. 4.13.1PECh. 4.5 -
How many grams of Na2SO4 are there in 15 mL of...Ch. 4.5 - Prob. 4.14.1PECh. 4.5 - What volume of 2.50 M lead(II) nitrate solution...Ch. 4.6 - How many milligrams of sodium sulfide are needed...Ch. 4.6 -
How many grams of NaOH are needed to neutralize...Ch. 4.6 - Prob. 4.16.1PECh. 4.6 - Prob. 4.16.2PECh. 4.6 - Practice Exercise 1 A mysterious white powder is...Ch. 4.6 - Prob. 4.17.2PECh. 4 - Prob. 1DECh. 4 - Prob. 1ECh. 4 - Aqueous solutions of three different substances,...Ch. 4 -
4 3 Use the molecular representations shown here...Ch. 4 - The concept of chemical equilibrium is very...Ch. 4 -
4 5 You are presented with a white solid and told...Ch. 4 - Which of the following ions will always be a...Ch. 4 - The labels have fallen off three bottles...Ch. 4 - Explain how a redox reaction involves electrons in...Ch. 4 - Prob. 9ECh. 4 - Prob. 10ECh. 4 -
4.11 Which data set, of the two graphed here,...Ch. 4 - You are titrating an acidic solution with a basic...Ch. 4 - State whether each of the following statements is...Ch. 4 - State whether each of the following statements is...Ch. 4 -
4.15 We have learned in this chapter that many...Ch. 4 - Prob. 16ECh. 4 -
4.17 Specify what ions are present in solution...Ch. 4 - Prob. 18ECh. 4 - Prob. 19ECh. 4 - Acetone. CH3COCH3, is a nonelectrolyte;...Ch. 4 -
4.21 Using solubility guidelines, predict whether...Ch. 4 - Prob. 22ECh. 4 - Prob. 23ECh. 4 - Prob. 24ECh. 4 - Which ions remain in solution, unreacted, after...Ch. 4 - Write balanced net ionic equations for the...Ch. 4 -
4.27 Separate samples of a solution of an unknown...Ch. 4 - Prob. 28ECh. 4 - Prob. 29ECh. 4 - Prob. 30ECh. 4 - Prob. 31ECh. 4 - Prob. 32ECh. 4 - State whether each of the following statements is...Ch. 4 - State whether each of the following statements is...Ch. 4 -
4.35 Label each of the following substances as an...Ch. 4 - An aqueous solution of an unknown solute is tested...Ch. 4 - Prob. 37ECh. 4 - Classify each of the following aqueous solutions...Ch. 4 - Complete and balance the following molecular...Ch. 4 - Write the balanced molecular and net ionic...Ch. 4 - Write balanced molecular and net ionic equations...Ch. 4 -
4.42 Because the oxide ion is basic, metal oxides...Ch. 4 -
4.43 Magnesium carbonate, magnesium oxide, and...Ch. 4 -
4.44 As K20 dissolves in water, the oxide ion...Ch. 4 - True or false: If a substance is oxidized, it is...Ch. 4 - Prob. 46ECh. 4 - Which region of the periodic table shown here...Ch. 4 - Determine the oxidation number of sulfur in each...Ch. 4 - Determine the oxidation number for the indicated...Ch. 4 - Determine the oxidation number for the indicated...Ch. 4 - Which element is oxidized, and which is reduced in...Ch. 4 - Which of the following are redox reactions? For...Ch. 4 -
4.53 Write balanced molecular and net ionic...Ch. 4 - Write balanced molecular and net ionic equations...Ch. 4 - Using the activity series (Table 4.5), write...Ch. 4 - Using the activity series (Table 4.5), write...Ch. 4 - The metal cadmium tends to form Cd2+ ions. The...Ch. 4 -
4.58 The following reactions (note that the...Ch. 4 - Is the concentration of a solution an intensive or...Ch. 4 - Prob. 60ECh. 4 - Calculate the molarity of a solution that contains...Ch. 4 -
4.62
Calculate the molarity of a solution made by...Ch. 4 - Prob. 63ECh. 4 - Prob. 64ECh. 4 - Prob. 65ECh. 4 -
4.66 The average adult male has a total blood...Ch. 4 -
4.67
How many grams of ethanol, CH2CH2OH should...Ch. 4 - Prob. 68ECh. 4 - Which will have the highest concentration of...Ch. 4 - Prob. 70ECh. 4 - Prob. 71ECh. 4 - Prob. 72ECh. 4 - Prob. 73ECh. 4 - Prob. 74ECh. 4 - Prob. 75ECh. 4 - Prob. 76ECh. 4 - Prob. 77ECh. 4 - Prob. 78ECh. 4 - Prob. 79ECh. 4 - Prob. 80ECh. 4 - Prob. 81ECh. 4 - Prob. 82ECh. 4 - Some sulfuric acid is spilled on a lab bench You...Ch. 4 -
4.84 The distinctive odor of vinegar is due to...Ch. 4 - A 4.36-g sample of an unknown alkali metal...Ch. 4 -
4.86 An 8.65-g sample of an unknown group 2A...Ch. 4 - A solution of 100.0 mL of 0.200 M KOH is mixed...Ch. 4 -
4.88 A solution is made by mixing 15.0 g of...Ch. 4 - Prob. 89ECh. 4 - A 1.248-9 sample of limestone rock is pulverized...Ch. 4 - 4.91 Uranium hexafluoride, UF6, is processed to...Ch. 4 - The accompanying photo shows the reaction between...Ch. 4 - Prob. 93AECh. 4 -
4.94 You choose to investigate some of the...Ch. 4 -
4 95 Antacids are often used to relieve pain and...Ch. 4 -
4 96 The commercial production of nitric acid...Ch. 4 - Consider the following reagents: zinc, copper,...Ch. 4 - 98 Bronze is a solid solution of Cu(s) and Sn(s);...Ch. 4 - Prob. 99AECh. 4 - Prob. 100AECh. 4 -
4.101 Hard water contains Ca2+ , Mg2 + , and Fe2+...Ch. 4 - Tartaric acid. H2C4H4O6, has two acidic hydrogens....Ch. 4 - Prob. 103AECh. 4 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 4 - Prob. 105IECh. 4 - Prob. 106IECh. 4 - Prob. 107IECh. 4 - A fertilizer railroad car carrying 34,300 gallons...Ch. 4 - Prob. 109IECh. 4 - Prob. 110IECh. 4 - Prob. 111IECh. 4 - Prob. 112IECh. 4 - Prob. 113IECh. 4 - Prob. 114IECh. 4 -
4.115 Federal regulations set an upper limit of...
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