GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
11th Edition
ISBN: 9780134193601
Author: Petrucci
Publisher: PEARSON
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Chapter 23, Problem 29E
When a soluble lead compound is added to a solution containing primarily orange dichromate ion, yellow lead chromate precipitates. Describe the equilibria involved.
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Chapter 23 Solutions
GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
Ch. 23 - By means of orbital diagrams, write electron...Ch. 23 - Arrange the following species according to the...Ch. 23 - Describe how the transition elements compare with...Ch. 23 - With only minor irregularities, the melting points...Ch. 23 - Why do the atomic radii vary so much for two...Ch. 23 - Prob. 6ECh. 23 - Which of me first transition series elements...Ch. 23 - Why is the number of common oxidation states for...Ch. 23 - As a group, the lanthanides are more reactive...Ch. 23 - The maximum difference in standard reduction...
Ch. 23 - Complete and balance the following equations. If...Ch. 23 - By means of e chemical equation, give an example...Ch. 23 - Prob. 13ECh. 23 - Prob. 14ECh. 23 - Prob. 15ECh. 23 - Prob. 16ECh. 23 - Prob. 17ECh. 23 - According to Figure 23-8, G decreases with...Ch. 23 - Prob. 19ECh. 23 - Prob. 20ECh. 23 - Write plausible half-equations to represent each...Ch. 23 - Prob. 22ECh. 23 - Use electrode potential data from this chapter or...Ch. 23 - You are given these three reducing agents: Zn(s);...Ch. 23 - Prob. 25ECh. 23 - Prob. 26ECh. 23 - Prob. 27ECh. 23 - Use data from the text to construct a standard...Ch. 23 - When a soluble lead compound is added to a...Ch. 23 - Prob. 30ECh. 23 - Prob. 31ECh. 23 - If CO2(g) under pressure is passed into...Ch. 23 - Use equation (23.19) to determine [Cr2O72] in a...Ch. 23 - If a solution is prepared by dissolving 1.505 g...Ch. 23 - Prob. 35ECh. 23 - Prob. 36ECh. 23 - Prob. 37ECh. 23 - Prob. 38ECh. 23 - Will reaction (23.25) still be spontaneous in the...Ch. 23 - Prob. 40ECh. 23 - Prob. 41ECh. 23 - Prob. 42ECh. 23 - Prob. 43ECh. 23 - Prob. 44ECh. 23 - Prob. 45ECh. 23 - Prob. 46ECh. 23 - Prob. 47ECh. 23 - At 400C , 2Hg(I)+O2(g)2HgO(s) for the reaction...Ch. 23 - Prob. 49ECh. 23 - Prob. 50ECh. 23 - Prob. 51ECh. 23 - Prob. 52ECh. 23 - Prob. 53ECh. 23 - Prob. 54ECh. 23 - The text notes that in small quantities, zinc is...Ch. 23 - Prob. 56ECh. 23 - What formulas would you expect for the metal...Ch. 23 - For the straight-line graphs in Figure 23-8...Ch. 23 - Prob. 59ECh. 23 - Prob. 60ECh. 23 - Prob. 61ECh. 23 - Prob. 62ECh. 23 - Prob. 63ECh. 23 - Prob. 64ECh. 23 - Prob. 65ECh. 23 - Prob. 66ECh. 23 - Prob. 67ECh. 23 - Prob. 68ECh. 23 - Prob. 69ECh. 23 - Prob. 70ECh. 23 - Prob. 71ECh. 23 - For a coordination number of four, the radius of...Ch. 23 - Prob. 73ECh. 23 - Prob. 74FPCh. 23 - Several transition metal ions are found in cation...Ch. 23 - Prob. 76SAECh. 23 - Briefly describe each of the following ideas. phe...Ch. 23 - Prob. 78SAECh. 23 - Prob. 79SAECh. 23 - Prob. 80SAECh. 23 - Prob. 81SAECh. 23 - Prob. 82SAECh. 23 - Prob. 83SAECh. 23 - Prob. 84SAECh. 23 - Prob. 85SAECh. 23 - Provide the missing name or formula for the...Ch. 23 - Prob. 87SAECh. 23 - Prob. 88SAECh. 23 - Prob. 89SAECh. 23 - Prob. 90SAE
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- To 200 ml of a solution containing 0.002 mol of aluminium chloride and 0.001 mol of calcium chloride is slowly added solid sodium phosphate (assuming no change in volume). How many grams of sodium phosphate must be added to precipitate as much of one ion as possible, while the other ion just doesn't precipitate? What percentage of the ion that will precipitate first is left in the solution at that moment?arrow_forwardIn a solution of potassium chromate, there is an equilibrium where chromate ions are bright yellow and dichromate ions are orange. What would you observe if you treated the orange solution with sodium hydroxide?arrow_forwardWhen you mix solutions of lead (II) nitrate and potassium iodide,(i) What is the colour of the precipitate formed? Name the compound evolved?arrow_forward
- Determine the percentage of CaO (56.08 g/mol) in the sample. Consider 0.4960 g of CaCO3 (100.09 g/mol) is dissolved in an acidic solution. The calcium is precipitated as CaC₂04 (110.12 g/mol) and the dry precipitate is found to 24 weigh 0.6186 g. a) 63.51% b) 31.50 % c) 71.87% d) 31.76 %arrow_forwardAfter completing a distillation to purify a mixture of sodium chloride and water, you decide to test the water to determine its purity. Upon addition of silver nitrate (AgNO3), a white solid precipitates out of the solution. Use the solubility table on Page 96 to determine the identity of the precipitate.arrow_forwardIn reaction with aqueous ammonia, Zn(OH)2 forms a complex ion. Explain the term complex ion, and explain how the formation of such a species can affect the solubility of a salt.arrow_forward
- Suppose you mistakenly used tap water instead of distilled water to dissolve your consumer product. When you did the test for chloride, you observe formation of a white precipitate after addition of silver nitrate. Can you rightly conclude that the product being tested contains chloride? Explain your reasoning.arrow_forwardA solution of potassium dichromate is made basic with sodium hydroxide;the color changes from red to yellow. Addition of silver nitrate to the yellow solution gives a precipitate. This precipitate dissolves in concentrated ammonia but re-forms when nitric acid is added. Write balanced net ionic equations for all the reactions in this sequence.arrow_forward(a) Halogen, V reacts with hydrogen gas to form HV only when heated to 200 °C in the presence of a platinum catalyst. An aqueous solution of HV is formed when HV is dissolved in water. When aqueous silver nitrate solution is added to the HV solution, precipitate W is formed. With the aid of a balanced chemical equation, explain the reaction between precipitate W and concentrated ammonia solution. () (i) The melting point of hydrogen fluoride, HF is higher than HV. Explain this phenomenon in terms of structure and bonding.arrow_forward
- Write out the correspoding solubility equilibrium equations that would give rise to a chromate precipitate. Form the chromate precipitates with 0.1 M Na2CrO4.arrow_forwardA solution contains 0.04500.0450 M Ca2+ and 0.09500.0950 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? -Ca3(PO4)2 -Ag3PO4 -Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?arrow_forwardAnalysis of an equilibrium solution of silver chromate indicates that the silver concentration is equal to 1.3 x 10-4 M. Calculate the solubility equilibrium constant (Ksp) for silverchromate.arrow_forward
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