General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 15, Problem 15.121SP
Give a method for separating the following pairs of ions by the addition of no more than two substances:
(a) Hg22+ and Co2+
(b) Na+ and Mg2+
(c) Fe2+ and Hg2+
(d) Ba2+and Pb2+
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
In an experiment on evaluation of antacid containing magnesium carbonate, a tablet weighing 2.50 g was completely dissolved using 5.00 mL of 1.00 M hydrochloric acid. The excess of acid was then back titrated with 1.00 M NaOH solution, with a pH indicator. The equivalence point was achieved when 2.30 mL of alkali was added. What was the content of magnesium carbonate in moles per gram?
(A) 0.00031 (B) 0.0042 (C) 0.0084 (D) 0.0011(E) None of the above. If so, what is your answer?
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration.
(a) Calculate the number of moles of NaOH required for the titration.
(b) Calculate the number of moles of KHP present in the impure sample of KHP.
(c) Calculate the number of grams of KHP present in the impure sample.
(d) Calculate the percent of KHP in the impure sample, using Equation 8.
Equation 8:
percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
3a. (2)A student prepared a 0.0750 M NaOH solution for a titration experiment. If it took 25.52 ml of the NaOH to turn the H2SO4 solution faint pink, how many moles of NaOH were required to reach the end point? 3b. (4)What was the mole of H2SO4 used from 3a. question?
Chapter 15 Solutions
General Chemistry: Atoms First
Ch. 15.1 - Write balanced net ionic equations for the...Ch. 15.1 - Write balanced net ionic equations for the...Ch. 15.2 - Calculate the concentrations of all species...Ch. 15.2 - Calculate the pH in a solution prepared by...Ch. 15.2 - Prob. 15.5CPCh. 15.3 - The following pictures represent solutions that...Ch. 15.3 - Calculate the pH of 0.100 L of a buffer solution...Ch. 15.3 - Calculate the change in pH when 0.002 mol of HNO3...Ch. 15.4 - Use the HendersonHasselbalch equation to calculate...Ch. 15.4 - Prob. 15.10P
Ch. 15.4 - Suppose you are performing an experiment that...Ch. 15.4 - Prob. 15.12PCh. 15.6 - A 40.0 mL volume of 0.100 M HCl is titrated with...Ch. 15.6 - A 40.0 mL volume of 0.100 M NaOH is titrated with...Ch. 15.7 - The following pictures represent solutions at...Ch. 15.7 - Consider the titration of 100.0 mL of 0.016 M HOCl...Ch. 15.7 - The following acid-base indicators change color in...Ch. 15.9 - Assume that 40.0 mL of 0.0800 M H2SO3 (Ka1 = 1.5 ...Ch. 15.9 - Assume that 40.0 mL of a 0.0250 M solution of the...Ch. 15.10 - Write the equilibrium-constant expression for Ksp...Ch. 15.11 - A saturated solution of Ca3(PO4)2 has [Ca2+] =...Ch. 15.11 - Prob. 15.22PCh. 15.11 - Which has the greater molar solubility: AgCl with...Ch. 15.11 - Prob. 15.24CPCh. 15.12 - Calculate the molar solubility of MgF2 in 0.10 M...Ch. 15.12 - Which of the following compounds are more soluble...Ch. 15.12 - In an excess of NH3(aq), Cu2+ ion forms a deep...Ch. 15.12 - Silver bromide dissolves in aqueous sodium...Ch. 15.13 - Prob. 15.29PCh. 15.13 - Will a precipitate form on mixing 25 mL of 1.0 ...Ch. 15.14 - Prob. 15.31PCh. 15.15 - Prob. 15.32PCh. 15 - The following pictures represent solutions that...Ch. 15 - The following pictures represent solutions that...Ch. 15 - The strong acid HA is mixed with an equal molar...Ch. 15 - The following pictures represent solutions at...Ch. 15 - The following pictures represent solutions at...Ch. 15 - The following pictures represent solutions at...Ch. 15 - Prob. 15.40CPCh. 15 - Prob. 15.41CPCh. 15 - Prob. 15.42CPCh. 15 - Prob. 15.43CPCh. 15 - Is the pH greater than, equal to, or less than 7...Ch. 15 - Prob. 15.45SPCh. 15 - Which of the following mixtures has the higher pH?...Ch. 15 - Which of the following mixtures has the lower pH?...Ch. 15 - Phenol (C6H5OH, Ka = 1.3 1010) is a weak acid...Ch. 15 - Aniline (C6H5NH2, Kb = 4.3 1010) is a weak base...Ch. 15 - The equilibrium constant Kn for the neutralization...Ch. 15 - The equilibrium constant Kn for the neutralization...Ch. 15 - Prob. 15.52SPCh. 15 - Does the pH increase, decrease, or remain the same...Ch. 15 - Prob. 15.54SPCh. 15 - Calculate the pH of a solution prepared by mixing...Ch. 15 - Prob. 15.56SPCh. 15 - The pH of a solution of NH3 and NH4Br is 8.90....Ch. 15 - Prob. 15.58SPCh. 15 - Prob. 15.59SPCh. 15 - Prob. 15.60SPCh. 15 - Which of the following gives a buffer solution...Ch. 15 - Prob. 15.62SPCh. 15 - Prob. 15.63SPCh. 15 - Calculate the pH of a buffer solution that is 0.20...Ch. 15 - Prob. 15.65SPCh. 15 - Calculate the pH of 0.250 L of a 0.36 M formic...Ch. 15 - Calculate the pH of0.375 L of a 0.18 M acetic...Ch. 15 - Prob. 15.68SPCh. 15 - Use the HendersonHasselbalch equation to calculate...Ch. 15 - Prob. 15.70SPCh. 15 - Give a recipe for preparing a CH3CO2HCH3CO2Na...Ch. 15 - Prob. 15.72SPCh. 15 - Prob. 15.73SPCh. 15 - What is the Ka of the amino acid leucine if it is...Ch. 15 - Prob. 15.75SPCh. 15 - Prob. 15.76SPCh. 15 - Make a rough plot of pH versus milliliters of acid...Ch. 15 - Prob. 15.78SPCh. 15 - Consider the titration of 50.0 mL of 0.116 M NaOH...Ch. 15 - Consider the titration of 40.0 mL of 0.250 M HF...Ch. 15 - A 100.0 mL sample of 0.100 M methylamine (CH3NH2,...Ch. 15 - Prob. 15.82SPCh. 15 - Consider the titration of 25.0 mL of 0.0200 M...Ch. 15 - Prob. 15.84SPCh. 15 - The equivalence point was reached in titrations of...Ch. 15 - Prob. 15.86SPCh. 15 - What is the pH at the equivalence point for the...Ch. 15 - Prob. 15.88SPCh. 15 - Prob. 15.89SPCh. 15 - Prob. 15.90SPCh. 15 - Prob. 15.91SPCh. 15 - Prob. 15.92SPCh. 15 - Prob. 15.93SPCh. 15 - Prob. 15.94SPCh. 15 - Prob. 15.95SPCh. 15 - Prob. 15.96SPCh. 15 - Prob. 15.97SPCh. 15 - Use Le Chteliers principle to explain the...Ch. 15 - Use Le Chteliers principle to predict whether the...Ch. 15 - Calculate the molar solubility of PbCrO4 in:...Ch. 15 - Calculate the molar solubility of SrF2 in:...Ch. 15 - Which of the following compounds are more soluble...Ch. 15 - Which of the following compounds are more soluble...Ch. 15 - Prob. 15.104SPCh. 15 - Is the solubility of Fe(OH)3 increased, decreased,...Ch. 15 - Prob. 15.106SPCh. 15 - Prob. 15.107SPCh. 15 - Prob. 15.108SPCh. 15 - Prob. 15.109SPCh. 15 - Calculate the molar solubility of AgI in: (a)Pure...Ch. 15 - Calculate the molar solubility of Cr(OH)3 in 0.50...Ch. 15 - What compound, if any, will precipitate when 80 mL...Ch. 15 - Prob. 15.113SPCh. 15 - Prob. 15.114SPCh. 15 - In qualitative analysis, Al3+ and Mg2+ are...Ch. 15 - Prob. 15.116SPCh. 15 - Can Co2+ be separated from Zn2+ by bubbling H2S...Ch. 15 - Prob. 15.118SPCh. 15 - Prob. 15.119SPCh. 15 - Prob. 15.120SPCh. 15 - Give a method for separating the following pairs...Ch. 15 - Assume that you have three white solids: NaCl,...Ch. 15 - On the same graph, sketch pH titration curves for...Ch. 15 - Prob. 15.124CHPCh. 15 - Prob. 15.125CHPCh. 15 - A saturated solution of Mg(OH)2 in water has pH =...Ch. 15 - Prob. 15.128CHPCh. 15 - In qualitative analysis, Ag+, Hg22+, and Pb2+ are...Ch. 15 - Calculate the molar solubility of MnS in a 0.30 M...Ch. 15 - Prob. 15.131CHPCh. 15 - Prob. 15.132CHPCh. 15 - Prob. 15.133CHPCh. 15 - Prob. 15.134CHPCh. 15 - Prob. 15.135CHPCh. 15 - A 100.0 mL sample of a solution that is 0.100 M in...Ch. 15 - A 0.0100 mol sample of solid Cd(OH)2 (Ksp = 5.3 ...Ch. 15 - Zinc hydroxide, Zn(OH)2 (Ksp = 4.1 1017), is...Ch. 15 - Prob. 15.139CHPCh. 15 - Prob. 15.140MPCh. 15 - Ethylenediamine (NH2CH2CH2NH2, abbreviated en) is...Ch. 15 - A 40.0 mL sample of a mixture of HCl and H3PO4 was...Ch. 15 - A 1.000 L sample of HCl gas at 25 C and 732.0 mm...Ch. 15 - Prob. 15.144MPCh. 15 - Consider the reaction that occurs on mixing 50.0...Ch. 15 - In qualitative analysis, Ca2+ and Ba2+ are...Ch. 15 - A railroad tank car derails and spills 36 tons of...Ch. 15 - Prob. 15.148MP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Phosphate ions are abundant in cells, both as the ions themselves and as important substituents on organic molecules. Most importantly, the pKa for the H2PO4 ion is 7.20, which is very close to the normal pH in the body. H2PO4(aq) + H2O() H3O+(aq) + HPO42(aq) 1. What should the ratio [HPO42]/[H2PO4] be to control the pH at 7.40?arrow_forward7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)Truearrow_forwardYou prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.64 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?arrow_forward
- (a) A 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH is titrated into the solution until the pH is exactly 5.0. What is the concentration of the titrant (NaOH)? (b) In the second step, enough 5.85 M nitric acid is added to the solution after the titration in part (a) is complete until the pH is one unit lower than the pKa of acetylsalicylic acid. What volume (mL) of nitric acid was added?arrow_forwardA 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 26.0 mL of HNO₃ was required. What quantity in moles of HNO₃ are used in the titration?arrow_forwardComplete the changes in concentrations for each of the following reactions:(a) BaSO4(s) ⟶ Ba2+(aq) + SO4 2−(aq) x _____(b) Ag2 SO4(s) ⟶ 2Ag+(aq) + SO4 2−(aq) _____ x(c) Al(OH)3(s) ⟶ Al3+(aq) + 3OH−(aq) x _____(d) Pb(OH)Cl(s) ⟶ Pb2+(aq) + OH−(aq) + Cl−(aq) _____ x _____(e) Ca3(AsO4 )2(s) ⟶ 3Ca2+(aq) + 2AsO4 3−(aq) 3x _____arrow_forward
- 8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?arrow_forwardWhat volume of 0.15 M H3PO4(aq) is needed to completely titrate 75.0 mL of 0.25 M Na2CO3?arrow_forwardLimestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5143 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel the CO2: CaCO3(s) + 2H+ ⟶⟶ Ca2+ + CO2↑↑ + H2O The excess acid requied 39.96 mL of 0.1004 M NaOH for complete titration: OH- + H+ ⟶⟶ H2O Find the weight percent of calcite in the limestone.arrow_forward
- In the following acid-base titration experiment CH3COOH (aq) + NaOH (aq) ———-> CH3COONa (aq) + H2O (l). What is the molarity of the NaOH solution if 11.6 mL of 3.0 M acetic acid is required to neutralize the sodium hydroxide in 25.00 mL of NaOH solution? (a) 0.65 M (b) 6.5 M (c) 96.6 M (d) 1.392 Marrow_forwardIf 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium concentration of Ag+(aq) in the final solution? Kf[Ag(NH3)2+] = 1.7E7Include at least 3 significant figures in your answerarrow_forwardIf it required 23.9 mL of 0.0150 M Ca(OH)2 to neutralize 25.0 mL of HNO3 , what was the initial concentration of the nitric acid solution?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY