Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 15, Problem 39QAP
Write net ionic equations for the reaction of H+ with
(a) Fe2S3
(b) Mg(OH)2
(c) MgCO3
(d) Pt(NH3)42+
(e) Hg2I2
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A 0.2219 g sample of pure iron wire was dissolved in acid and the iron reduced to +2 state. Then
the solution required 34.65 mL of cerium (IV) in a titration. Calculate the molar concentration of
Ce solution.
(A) 0.1147 M
(B) 0.1174 M
(C) 0.1417 M
(D) 0.1471 M
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C
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To oxidize the iron in 1.00 gram of FeSO4·(NH4)2SO4·6 H2O requires 5.00 mL of HNO3.(Fe 2++ NO3― + H+→ Fe 3++ NO + H2O)How much water must be added to 500 mL of this acid to make the concentration as an acid exactly one-tenth normal?
What are the oxidation numbers of the following:
(a) Ca in Ca2+
(b) Al in Al(OH)3
(c) Al in Al3+
Chapter 15 Solutions
Chemistry: Principles and Reactions
Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Calculate K for the reactions in Question 1.Ch. 15 - Calculate K for the reactions in Question 2.Ch. 15 - Calculate K for the reactions in Question 3.Ch. 15 - Calculate K for the reactions in Question 4.Ch. 15 - Calculate [H+] and pH in a solution in which...Ch. 15 - Calculate [OH-] and pH in a solution in which the...
Ch. 15 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 15 - Prob. 12QAPCh. 15 - A buffer solution is prepared by adding 15.00 g of...Ch. 15 - A buffer solution is prepared by adding 5.50 g of...Ch. 15 - A solution with a pH of 9.22 is prepared by adding...Ch. 15 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Copper(l) chloride, CuCl, is the starting material...Ch. 15 - Prob. 22QAPCh. 15 - Prob. 23QAPCh. 15 - Ksp for CaSO4 at 100C is estimated to be1.6105. At...Ch. 15 - Prob. 25QAPCh. 15 - At 25C, 10.24 mg of Cr(OH)2 are dissolved in...Ch. 15 - Calcium nitrate is added to a sodium sulfate...Ch. 15 - Cadmium(ll) chloride is added to a solution of...Ch. 15 - Water from a well is found to contain 3.0 mg of...Ch. 15 - Silver(I) sulfate (Ksp=1.2105) is used in the...Ch. 15 - A solution is prepared by mixing 13.00 mL of...Ch. 15 - A solution is prepared by mixing 45.00 mL of 0.022...Ch. 15 - A solution is 0.047 M in both NaF and Na2CO3....Ch. 15 - Solid lead nitrate is added to a solution that is...Ch. 15 - A solution is made up by adding 0.632 g of barium...Ch. 15 - A solution is made up by adding 0.839 g of...Ch. 15 - Prob. 37QAPCh. 15 - To a beaker with 500 mL of water are added 95 mg...Ch. 15 - Write net ionic equations for the reaction of H+...Ch. 15 - Prob. 40QAPCh. 15 - Prob. 41QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 43QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 45QAPCh. 15 - Write an overall net ionic equation and calculate...Ch. 15 - Consider the reaction...Ch. 15 - Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2...Ch. 15 - Aluminum hydroxide reacts with an excess of...Ch. 15 - Prob. 50QAPCh. 15 - Calculate the molar solubility of gold(I) chloride...Ch. 15 - Calculate the molar solubility of PbCl2 in 0.2 M...Ch. 15 - For the reaction...Ch. 15 - For the reaction Zn(OH)2(s)+2OH(aq)Zn(OH)42(aq)...Ch. 15 - What are the concentrations of Cu2+, NH3, and...Ch. 15 - Prob. 56QAPCh. 15 - Calcium ions in blood trigger clotting. To prevent...Ch. 15 - Prob. 58QAPCh. 15 - A town adds 2.0 ppm of F- ion to fluoridate its...Ch. 15 - Consider the following hypothetical dissociation:...Ch. 15 - Prob. 61QAPCh. 15 - Consider a 2.0-L aqueous solution of 4.17 M NH3,...Ch. 15 - Marble is almost pure CaCO3. Acid rain has a...Ch. 15 - Prob. 64QAPCh. 15 - Prob. 65QAPCh. 15 - The box below represents one liter of a saturated...Ch. 15 - Consider a saturated solution of BaCO3 at 7.5C....Ch. 15 - Prob. 68QAPCh. 15 - Consider the insoluble salts JQ, K2R, L2S3, MT2,...Ch. 15 - Prob. 70QAPCh. 15 - Consider the equilibrium curve for AgCl shown...Ch. 15 - Dissolving CaCO3 is an endothermic reaction. The...Ch. 15 - Challenge Problems Insoluble hydroxides such as...Ch. 15 - What is the solubility of CaF2 in a buffer...Ch. 15 - What is [Br-] just as AgCl begins to precipitate...Ch. 15 - Prob. 76QAPCh. 15 - Prob. 77QAPCh. 15 - Prob. 78QAP
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- This compound is used in the preliminary treatment of municipal water supply. (A) Al2(SO4)3 (B) Na2CO3 (C) NaOCl (D) Ca(OCl)2arrow_forwardCalculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution with 0.0.00010 M CN–.arrow_forward(a) What is the pH of a 0.32 M solution of a weak acid, HCNO if Ka for HCNO is 2.0 x 10-4? (SHOW CALCULATIONS) (b) How would the pH change if 0.10 M KCNO is added to the solution and show how you determined this change.arrow_forward
- 2. A common reagent is used to identify zinc and copper ions:A) Sodium sulideB) Potassium hexacyanoferrate (II)C) Potassium hexacyanoferrate (III)D) Ammonia solutionE) Potassium iodidearrow_forwardChoose the best answer below. Consider the following complex ion formation equilibrium and it's equilibrium constant, Kf. Which of the following statements is FALSE? Cu2* (aq) + 4CN" (aq) Û Cu(CN)4² (aq) K = 1.0x1025 Cu2* is a Lewis acid in the reaction, and CN' is a Lewis base Removing some of the Cu2* (e.g., by precipitation) will cause some of the complex ion to dissociate O If enough CN is added, the equilibrium mixture would contain zero Cu²+ The complex ion is a Lewis acid-base adduct Adding more CN" will cause more complex ion to form ) The equilibrium lies in favor of the complex ionarrow_forward0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???arrow_forward
- The composition of a hydrated sodium-salt of a chromium(III)-oxalate complex ion conforms to the general formula: NaxCr(C2O4)3·wH2O A 0.2547-g sample of this compound required 21.99 mL of 0.02925 M KMnO4 solution for the titration of all of the oxalate. a)What is the value of x? b)What is the value of w?arrow_forwardWhat is the net ionic equation for the reaction between aqueous solutions of Cu(C2H3O2)2 and NaOH?arrow_forwardA solution contains both NaI and NaBr. Which oxidizing agent could you add to the solution to selectively oxidize I-(aq) but not Br-(aq)?(a) Cl2 (b) H2O2 (c) CuCl2 (d) HNO3arrow_forward
- Given the balanced equation: 16H+ + 2MnO4- + 5C2O42- --> 2Mn+ + 10CO2 + 8H2O If .184 g of green K3[Fe(C2O4)3]*3H2O was titrated with 19.5 mL .0310 M KMnO4, what is the percent purity? (I do not understand because there are not even any potassium in the equation to begin with. I do not know what to use to calculate molar mass or mole rations)arrow_forwardGiven two possible formulas: K[Fe(C2O4)2(H2O)2] or K3[Fe(C2O4)3], a titration of 1.356g of the compound (one of the two formulas above requires 34.5 mL of 0.108 M KMnO4. Which formula matches the compound being titrated?arrow_forwardCalculate the pH of a solution that is 0.100 M in Fe(NO3)3.arrow_forward
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