Chemistry
13th Edition
ISBN: 9781259911156
Author: Raymond Chang Dr., Jason Overby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 16.6, Problem 8PE
The solubility of lead chromate (PbCrO4) is 4.5 × 10−5 g/L. Calculate the solubility product of this compound.
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Chemistry
Ch. 16.2 - What is the pH of a solution containing 0.30 M...Ch. 16.2 - Prob. 1RCFCh. 16.2 - What is the pH of a solution containing 0.25 M...Ch. 16.3 - Which of the following couples are buffer systems:...Ch. 16.3 - Calculate the pH of the 0.30 M NH3/0.36 M NH4Cl...Ch. 16.3 - How would you prepare a liter of carbonate buffer...Ch. 16.3 - Calculate the pH of the 0.40 M HF/0.48 M KF buffer...Ch. 16.3 - The diagrams (a)(d) represent solutions containing...Ch. 16.4 - Exactly 100 mL of 0.10 M nitrous acid (HNO2) are...Ch. 16.4 - Calculate the pH at the equivalence point in the...
Ch. 16.4 - For which of the following titrations will the pH...Ch. 16.4 - Calculate the pH at the equivalence point in the...Ch. 16.4 - calculate the pH in the titration of 50.0 mL of...Ch. 16.5 - Referring to Table 16.1, specify which indicator...Ch. 16.5 - Under what conditions will the end point of an...Ch. 16.6 - The solubility of lead chromate (PbCrO4) is 4.5 ...Ch. 16.6 - Calculate the solubility of silver chloride (AgCl)...Ch. 16.6 - Prob. 10PECh. 16.6 - Prob. 1RCFCh. 16.6 - Will a precipitate form when 50.0 mL of 0.0100 M...Ch. 16.6 - The diagrams (a)(d) represent solutions of AgCl,...Ch. 16.7 - The solubility products of AgCl and Ag3PO4 are 1.6...Ch. 16.7 - AgNO3 is slowly added to a solution that contains...Ch. 16.8 - Prob. 12PECh. 16.8 - Calculate the molar solubility of CaF2 in 0.0015 M...Ch. 16.9 - Is the solubility of the following compounds...Ch. 16.9 - Calculate whether or not a precipitate will form...Ch. 16.9 - Prob. 1RCFCh. 16.10 - Prob. 15PECh. 16.10 - Calculate the molar solubility of AgBr in a 1.0 M...Ch. 16.10 - Prob. 1RCFCh. 16.11 - An aqueous solution contains both Zn2+ and Pb2+...Ch. 16 - Use Le Chteliers principle to explain how the...Ch. 16 - Describe the effect on pH (increase, decrease, or...Ch. 16 - The pKas of two monoprotic acids HA and HB are 5.9...Ch. 16 - Determine the pH of (a) a 0.40 M CH3COOH solution,...Ch. 16 - Determine the pH of (a) a 0.20 M NH3 solution, (b)...Ch. 16 - What is a buffer solution? What constitutes a...Ch. 16 - Which of the following has the greatest buffer...Ch. 16 - Which of the following solutions can act as a...Ch. 16 - Which of the following solutions can act as a...Ch. 16 - Calculate the pH of the buffer system made up of...Ch. 16 - Calculate the pH of the following two buffer...Ch. 16 - The pH of a bicarbonate-carbonic acid buffer is...Ch. 16 - What is the pH of the buffer 0.10 M Na2HPO4/0.15 M...Ch. 16 - The pH of a sodium acetateacetic acid buffer is...Ch. 16 - The pH of blood plasma is 7.40. Assuming the...Ch. 16 - Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl...Ch. 16 - Calculate the pH of 1.00 L of the buffer 1.00 M...Ch. 16 - A student is asked to prepare a buffer solution at...Ch. 16 - The diagrams (a)(d) contain one or more of the...Ch. 16 - The diagrams shown here represent solutions...Ch. 16 - How much NaOH (in moles) must be added to 1 L of a...Ch. 16 - How much HCl (in moles) must be added to 1 L of a...Ch. 16 - Briefly describe what happens in an acid-base...Ch. 16 - Sketch titration curves for the following...Ch. 16 - A 0.2688-g sample of a monoprotic acid neutralizes...Ch. 16 - A 5.00-g quantity of a diprotic acid was dissolved...Ch. 16 - In a titration experiment, 12.5 mL of 0.500 M...Ch. 16 - In a titration experiment, 20.4 mL of 0.883 M...Ch. 16 - A 0.1276-g sample of an unknown monoprotic acid...Ch. 16 - A solution is made by mixing 5.00 102 mL of 0.167...Ch. 16 - Calculate the pH at the equivalence point for the...Ch. 16 - Calculate the pH at the equivalence point for the...Ch. 16 - A 25.0-mL solution of 0.100 M CH3COOH is titrated...Ch. 16 - A 10.0-mL solution of 0.300 M NH3 is titrated with...Ch. 16 - The diagrams shown here represent solutions at...Ch. 16 - Prob. 16.38QPCh. 16 - A 0.054 M HNO2 solution is titrated with a KOH...Ch. 16 - A student titrates an unknown monoprotic acid with...Ch. 16 - Explain how an acid-base indicator works in a...Ch. 16 - The amount of indicator used in an acid-base...Ch. 16 - Referring to Table 16.1, specify which indicator...Ch. 16 - A student carried out an acid-base titration by...Ch. 16 - The ionization constant Ka of an indicator HIn is...Ch. 16 - Use BaSO4 to distinguish between solubility, molar...Ch. 16 - Why do we usually not quote the Ksp values for...Ch. 16 - Write balanced equations and solubility product...Ch. 16 - Write the solubility product expression for the...Ch. 16 - How can we predict whether a precipitate will form...Ch. 16 - Silver chloride has a larger Ksp than silver...Ch. 16 - From the solubility data given, calculate the...Ch. 16 - The molar solubility of MnCO3 is 4.2 106 M. What...Ch. 16 - The solubility of an ionic compound MX (molar mass...Ch. 16 - The solubility of an ionic compound M2X3 (molar...Ch. 16 - Using data from Table 16.2, calculate the molar...Ch. 16 - Prob. 16.59QPCh. 16 - The pH of a saturated solution of a metal...Ch. 16 - If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL...Ch. 16 - A volume of 75 mL of 0.060 M NaF is mixed with 25...Ch. 16 - Solid NaI is slowly added to a solution that is...Ch. 16 - Find the approximate pH range suitable for the...Ch. 16 - How does the common ion effect influence...Ch. 16 - Prob. 16.66QPCh. 16 - How many grams of CaCO3 will dissolve in 3.0 102...Ch. 16 - The solubility product of PbBr2 is 8.9 106....Ch. 16 - Calculate the molar solubility of AgCl in a 1.00-L...Ch. 16 - Calculate the molar solubility of BaSO4 (a) in...Ch. 16 - Prob. 16.71QPCh. 16 - Which of the following will be more soluble in...Ch. 16 - Prob. 16.73QPCh. 16 - Calculate the molar solubility of Fe(OH)2 in a...Ch. 16 - The solubility product of Mg(OH)2 is 1.2 1011....Ch. 16 - Calculate whether or not a precipitate will form...Ch. 16 - If 2.50 g of CuSO4 are dissolved in 9.0 102 mL of...Ch. 16 - Calculate the concentrations of Cd2+, Cd(CN3)42,...Ch. 16 - If NaOH is added to 0.010 M Al3+, which will be...Ch. 16 - Calculate the molar solubility of AgI in a 1.0 M...Ch. 16 - Both Ag+ and Zn2+ form complex ions with NH3....Ch. 16 - Explain, with balanced ionic equations, why (a)...Ch. 16 - Outline the general procedure of qualitative...Ch. 16 - Give two examples of metal ions in each group (1...Ch. 16 - In a group 1 analysis, a student obtained a...Ch. 16 - In a group 1 analysis, a student adds HCl acid to...Ch. 16 - Both KCl and NH4Cl are white solids. Suggest one...Ch. 16 - Describe a simple test that would enable you to...Ch. 16 - To act as an effective buffer, the concentrations...Ch. 16 - The pKa of the indicator methyl orange is 3.46....Ch. 16 - The iodide impurity in a 4.50-g sample of a metal...Ch. 16 - A sodium acetate-acetic acid buffer solution was...Ch. 16 - Prob. 16.95QPCh. 16 - A 200-mL volume of NaOH solution was added to 400...Ch. 16 - The pKa of butyric acid (HBut) is 4.7. Calculate...Ch. 16 - A solution is made by mixing 5.00 102 mL of 0.167...Ch. 16 - Cd(OH)2 is an insoluble compound. It dissolves in...Ch. 16 - A student mixes 50.0 mL of 1.00 M Ba(OH)2 with...Ch. 16 - For which of the following reactions is the...Ch. 16 - A 2.0-L kettle contains 116 g of boiler scale...Ch. 16 - Equal volumes of 0.12 M AgNO3 and 0.14 M ZnCl2...Ch. 16 - Prob. 16.104QPCh. 16 - Prob. 16.105QPCh. 16 - A volume of 25.0 mL of 0.100 M HCl is titrated...Ch. 16 - The molar solubility of Pb(IO3)2 in a 0.10 M NaIO3...Ch. 16 - When a KI solution was added to a solution of...Ch. 16 - Barium is a toxic substance that can seriously...Ch. 16 - Prob. 16.110QPCh. 16 - Solid NaBr is slowly added to a solution that is...Ch. 16 - Cacodylic acid is (CH3)2AsO2H. Its ionization...Ch. 16 - Radiochemical techniques are useful in estimating...Ch. 16 - The molar mass of a certain metal carbonate, MCO3,...Ch. 16 - Acid-base reactions usually go to completion....Ch. 16 - Calculate x, which is the number of molecules of...Ch. 16 - Describe how you would prepare a 1-L 0.20 M...Ch. 16 - Prob. 16.118QPCh. 16 - Prob. 16.119QPCh. 16 - What reagents would you employ to separate the...Ch. 16 - Look up the Ksp values for BaSO4 and SrSO4 in...Ch. 16 - In principle, amphoteric oxides, such as Al2O3 and...Ch. 16 - Prob. 16.123QPCh. 16 - When lemon juice is squirted into tea, the color...Ch. 16 - How many milliliters of 1.0 M NaOH must be added...Ch. 16 - The maximum allowable concentration of Pb2+ ions...Ch. 16 - Which of the following solutions has the highest...Ch. 16 - Prob. 16.129QPCh. 16 - Water containing Ca2+ and Mg2+ ions is called hard...Ch. 16 - Prob. 16.131QPCh. 16 - Prob. 16.132QPCh. 16 - (a) Referring to Figure 16.6, describe how you...Ch. 16 - Prob. 16.135QPCh. 16 - One way to distinguish a buffer solution with an...Ch. 16 - Prob. 16.137QPCh. 16 - A sample of 0.96 L of HCl at 372 mmHg and 22C is...Ch. 16 - (a) Assuming complete dissociation and no ion-pair...Ch. 16 - Calculate the maximum mass (in grams) of each of...Ch. 16 - A 1.0-L saturated silver carbonate solution at 5C...Ch. 16 - The two curves shown represent the titration of...Ch. 16 - Prob. 16.143QPCh. 16 - A 100-mL 0.100 M CuSO4 solution is mixed with a...Ch. 16 - The titration curve shown represents the titration...Ch. 16 - The titration curve shown represents the titration...Ch. 16 - Use appropriate equations to account for the...Ch. 16 - Prob. 16.148QPCh. 16 - Aspirin is a weak acid with pKa = 3.5. What is the...
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- The concentration of barium in a saturated solution of barium sulfate at a particular temperature is 1.2 g/mL. Calculate Ksp at this temperature.arrow_forwardSolubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forwardThe solubility of Mg(OH)2 in water is approximately 9.6 mg/L at a given temperature. Calculate the Ksp of magnesium hydroxide. Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg Mg2+ per liter remains in the solution.arrow_forward
- Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.arrow_forwardA solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?arrow_forward12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its Ksp.arrow_forward
- Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?arrow_forwardWhat is the difference between the ion product, Q, and the solubility product, Ksp? What happens when Q Ksp? Q Ksp? Q = Ksp?arrow_forwardHow many grams of Milk of Magnesia, Mg(OH)2 (s) (58.3 g/mol), would be soluble in 200 mL of water. (KSP=7.11012). Include the ionic reaction and the expression for Ksp, in your answer. (Kw=11014=[H3O+][HO]).arrow_forward
- Write the Ksp expression for each of these slightly soluble salts: CuBr HgI2 SrSO4arrow_forwardSolubility Equilibria Consider three hypothetical ionic solids: AX, AX2, and AX3 (each X forms X). Each of these solids has the same Ksp value, 5.5 10 7. You place 0.25 mol of each compound in a separate container and add enough water to bring the volume to 1.0 L in each case. a Write the chemical equation for each of the solids dissolving in water. b Would you expect the concentration of each solution to be 0.25 M in the compound? Explain, in some detail, why or why not. c Would you expect the concentrations of the A cations (A+, A2+, and A3+) in the three solutions to be the same? Does just knowing the stoichiometry of each reaction help you determine the answer, or do you need something else? Explain your answer in detail, but without doing any arithmetic calculations. d Of the three solids, which one would you expect to have the greatest molar solubility? Explain in detail, but without doing any arithmetic calculations. e Calculate the molar solubility of each compound.arrow_forwardHow would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?arrow_forward
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