EBK GENERAL CHEMISTRY
11th Edition
ISBN: 9780134419022
Author: Bissonnette
Publisher: PEARSON CUSTOM PUB.(CONSIGNMENT)
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Chapter 17, Problem 10E
Lactic acid,
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Gallium hydroxide is a very sparingly soluble ionic salt. Given the molar solubility of gallium hydroxide is 7.21 x 10-10 M, what is the Ksp for the dissociation of gallium hydroxide?
The pertinent balanced chemical equation is: Ga(OH)3 (s) ↔ Ga3+ (aq) + 3 OH- (aq).
The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C.
(a) Write a balanced equation for the solubility equilibrium.
(b) Write the expression for the solubility product constant, Ksp, and calculate its value.
(c) Calculate the pH of a saturated solution of Fe(OH)2 at 25 °C.
Consider the following reaction:
Ag+ (ag) + 2 NH3 (aq) = Ag(NH3)2+ (aq) Keq = 7.99
An initial concentration of Ag+ = 0.0100 M was combined with NH3 and allowed to reach equilibrium. If the equilibrium concentration of Ag(NH3)2+= 0.00278 M, What was the initial concentration of NH3?
Chapter 17 Solutions
EBK GENERAL CHEMISTRY
Ch. 17 - For a solution that e 0.275M CH2CH2 COOH...Ch. 17 - For a solution that is 0164 U NH2 and 0.102MNH4Cl...Ch. 17 - Prob. 3ECh. 17 - In Example 16-4, we calculated the percent...Ch. 17 - Calculate [H2OOH-] in a solution that is (a)...Ch. 17 - Calculate [OH-] in a solution that is (a) 0.0062 U...Ch. 17 - What concentration of formate ion, [HCOO-], should...Ch. 17 - What concentration of ammonia. [NH2] , should be...Ch. 17 - Calculate the pH of a buffer that is a. 0.012 M...Ch. 17 - Lactic acid, CH2CH(OH)COOH , is found in sour...
Ch. 17 - Indicate which of the following aqueous solutions...Ch. 17 - The H2PO4-HPO4- combination plays a role in...Ch. 17 - What is the pH of a solution Obtained by adding...Ch. 17 - What the pH of solution prepared by dissolving...Ch. 17 - You wish to prepare a buffer solution w pH = 945...Ch. 17 - You prepare a buffer solution by dissolving 2.00 g...Ch. 17 - If 0.55 ml. of 12 M HCI is added to 0100 L of the...Ch. 17 - If 0.35 mL of 15 P.4 NH is added to 0750 L of the...Ch. 17 - You are asked to prepare e buffer solution why a...Ch. 17 - You are asked to reduce the pH of the 03001 of...Ch. 17 - Given 1.00 L of a solution that is 0.100 hl...Ch. 17 - Given 125mL of a solution that is 0.0500 M CH2NH2...Ch. 17 - A solution of volume 750 mL contars 15.5 mmol...Ch. 17 - A solution of volume 0.500 L contains 1.68 g NH...Ch. 17 - A handbook lets various procedures for preparing...Ch. 17 - An acetic acid-sodium acetate buffer can be...Ch. 17 - A handbook lists the following data: Which of...Ch. 17 - With reference to the indicators listed in...Ch. 17 - In use of acid—base indicators, a. Why is it...Ch. 17 - The indicator methyl red has a pKHIN=4.95 . It...Ch. 17 - Phenol red indicator changes from yellow to red in...Ch. 17 - Thymol blue indicator has two pH ranges. It...Ch. 17 - In the titration of 10.00 mL of 0.04050 M HCI with...Ch. 17 - Solution (a) is 1000 mL of 0.100 N HCI and...Ch. 17 - A 25.00 mL sample of H2PO4(aq) requires 31.15 mL...Ch. 17 - A 2000 ml sample of H2PO4(aq) requires 18.67 mL...Ch. 17 - Two aqueous solutions are mixed 50.0 mL of 0.0150M...Ch. 17 - Two solutions are mixed 100.0 mL of HCI(aq) with...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points m the titration...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points lithe titration of...Ch. 17 - Explain why the volume of 0.100 M NeOH required to...Ch. 17 - Explain whether the equivalence point of each of...Ch. 17 - Sketch the titration curves of the following...Ch. 17 - Determine the blowing characteristeristics of the...Ch. 17 - In the titration of 2000 mL of 0175 M NaOH,...Ch. 17 - In the titration of 25.00mL of 0.100M CH2COOH ,...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - For me titration of 25.00 mL of 0.100M NaOH with...Ch. 17 - For the titration of 25.00 mL 0.100M NH2 with...Ch. 17 - Is a solution that is 0.10 M Na2S(aq) likely to be...Ch. 17 - Is a solution of sodium dihydrogen citrate,...Ch. 17 - Sodium phosphate Na2PO4 , is made commecie1y by...Ch. 17 - Both sodium hydrogen carbonate (sodium...Ch. 17 - The pH of a solution of 19.5 g of malonic acid in...Ch. 17 - The ionization constants of ortho-phthalic acid...Ch. 17 - What stoichimetric concentration of the indicated...Ch. 17 - What stocichiometric concentration of the...Ch. 17 - Using appropriate equilibrium constants but...Ch. 17 - Prob. 62ECh. 17 - Sodium hydrogen sulfate NaHSO4 , an acidic salt...Ch. 17 - You are given 250.0mL of 0.100M CH3 CH2 COOH...Ch. 17 - Even though the carbonic acid-hydrogen carbonate...Ch. 17 - Thymol blue in its acid range is not a suitable...Ch. 17 - Rather than calculate the pH for different volumes...Ch. 17 - Use the method of Exercise 67 to determine the...Ch. 17 - A buffer solution can be prepared by starting with...Ch. 17 - You are asked to prepare a KH2PO4-Na2HPO2 solution...Ch. 17 - You are asked to bring the pH of 0.500 L of 0.500...Ch. 17 - Because an acid-base indicator a weak acid, I can...Ch. 17 - The neutralization of NaOH 2by HCl is represented...Ch. 17 - The titration of a weak acid by a weak base a not...Ch. 17 - At times a salt of a we base can be titrated by a...Ch. 17 - Sulfuric acid is a diprotic acid, strong in the...Ch. 17 - Carbonic acid is a weak diprotic acid (H2CO2) with...Ch. 17 - Prob. 78IAECh. 17 - Complete the derivation of equation (17.10)...Ch. 17 - Explain why equation (17.10) fads when applied to...Ch. 17 - Prob. 81IAECh. 17 - Prob. 82IAECh. 17 - Prob. 83IAECh. 17 - Prob. 84IAECh. 17 - Prob. 85IAECh. 17 - Calculate the pH of a solution that is 0.050 U...Ch. 17 - Prob. 87IAECh. 17 - The Henderson-Hasselbalch equation can be written...Ch. 17 - The pH of ocean water depends on the amount of...Ch. 17 - A sample of water contains 23.0 g L1 of Na+ (aq),...Ch. 17 - Prob. 91IAECh. 17 - Prob. 92FPCh. 17 - In some cases the titration curve for a mature of...Ch. 17 - Amino acids contain both an acidic carboxylic acid...Ch. 17 - In your own words, define or explain the following...Ch. 17 - Prob. 96SAECh. 17 - Explain the important distinctions between each...Ch. 17 - Write equations to show how each of the following...Ch. 17 - Sketch the titration curves that you would expect...Ch. 17 - A 2500-mL sample of 0.0100M C8C5COOH (Kg=6.3103)...Ch. 17 - Prob. 101SAECh. 17 - Prob. 102SAECh. 17 - Prob. 103SAECh. 17 - Prob. 104SAECh. 17 - Prob. 105SAECh. 17 - Calculate the pH of a 0.5 M solution of Ca(HSe)2...Ch. 17 - Prob. 107SAECh. 17 - Prob. 108SAECh. 17 - Prob. 109SAECh. 17 - Prob. 110SAECh. 17 - Prob. 111SAE
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- Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardTo a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be • no precipitate? • a precipitate of BaCO3 only? • a precipitate of CaCO3 only? • a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.arrow_forward= 1.6 x 10-10 Given the reactions below, calculate the molar solubility of AgCl (s) in 0.566 M NH3 (aq) at 25 degrees C. AgCl (s) →> Ag+ (aq) + Cl¯ (aq) K sp Ag+ (aq) + 2 NH3 (aq) →> Ag (NH3) + (aq) K = 1.7 x 107 f 2 Report your answer rounded to two significant figures and do NOT include units. Use "e" for scientific notation. For example, 1.0 x 10-14 is 1.0e-14.arrow_forward
- The solubility of TICI (thallium(I) chloride), an intermediate formed when thallium is being isolated from ores, is 3.12 grams per liter at 20 °C. What is its solubility product?arrow_forwardCalculate the Molar Solubility at 25.0 oC of an aqueous solution of calcium phosphate, Ca3(PO4)2, given that its Ksp = 1.20 x 10–26 at 25.0 oC.arrow_forwarda) Balance the following equation and write it below: Fe (s) + Mg3(PO,), (aq) → Fe;(P 0,), (aq) + Mg(s) b) If you added 134.2 grams of Iron to an excess of Mg,(PO,)2, how many moles of Iron have you added? c) Assuming the reaction is reversible, in which direction would the equilibrium shift if Fe was removed from the solution (left, right, or no change?) d) What type of reaction is this?arrow_forward
- 4 g The solubility of Fe(OH)2 in water at 25 °C is measured to be 5.2 × 10 L Round your answer to 2 significant digits. x10 S Use this information to calculate K sp for Fe(OH)2.arrow_forwardWhen Fe(OH)3 is added to 1.0 M HSCN, the following reaction occurs. Given that the pKa of HSCN is 1.1 and Kf for Fe(SCN)3 is 2.0x10^6, Fe(OH3)3(s)+ 3HSCN(aq)⇌Fe(SCN)3(aq)+ 3H2O(l) a.Calculate K for the reaction. b.Calculate the molar solubility of Fe(OH)3 in 1.0 M HSCN. c.Calculate the equilibrium [HSCN] and [Fe(SCN)3].arrow_forwardThe solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C. Write a balanced equation for the solubility equilibrium. Write the expression for the solubility product constant, Ksp, and calculate its value. Calculate the pH of a saturated solution of Fe(OH)2 at 25 °C.arrow_forward
- The following solubility equilibrium has K = 2.8 x 10–3 at 25oC. AgCl(s) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) + Cl–(aq) How many grams of AgCl (molar mass = 143.35 g/mol) will dissolve in 5.0 x 102 mL of 2.0 M NH3 solution at 25oC? (A) 0.76 g (B) 7.6 g (C) 6.9 g (D) 1.4 garrow_forwardAt 25 °C, an aqueous solution has an equilibrium concentration of 0.00217 M for a generic cation, A+(aq), and 0.00109 M for a generic anion, B2−(aq). What is the equilibrium constant, ?sp, of the generic salt A2B(s)?arrow_forwardThe following solubility equilibrium has K = 2.8 x 10–3 at 25oC. AgCl(s) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) + Cl–(aq) How many grams of AgCl (molar mass = 143.35 g/mol) will dissolve in 5.0 x 102 mL of 2.0 M NH3 solution at 25oC? (A) 0.76 g (B) 6.9 g Is the correct answer (A) or (B)?arrow_forward
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