A solution contains some or all of the ions Cu2+Cu2+, Al3+Al3+, K+K+, Ca2+Ca2+, Ba2+Ba2+, Pb2+Pb2+, and NH4+NH4+. The following tests were performed, in order, on the solution. Addition of 6 MM HClHCl produced no reaction. Addition of H2SH2S with 0.2 MM HClHCl produced a black solid. Addition of (NH4)2S(NH4)2S produced a white solid. Addition of (NH4)2HPO4(NH4)2HPO4 in NH3NH3 produced no reaction. The final supernatant when heated produced a purple flame. Identify which of these ions were present in the solution, which were absent, and for which ones no conclusions can be drawn.

A solution contains some or all of the ions Cu2+Cu2+, Al3+Al3+, K+K+, Ca2+Ca2+, Ba2+Ba2+, Pb2+Pb2+, and NH4+NH4+. The following tests were performed, in order, on the solution. Addition of 6 MM HClHCl produced no reaction. Addition of H2SH2S with 0.2 MM HClHCl produced a black solid. Addition of (NH4)2S(NH4)2S produced a white solid. Addition of (NH4)2HPO4(NH4)2HPO4 in NH3NH3 produced no reaction. The final supernatant when heated produced a purple flame. Identify which of these ions were present in the solution, which were absent, and for which ones no conclusions can be drawn.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

See similar textbooks

Similar questions

25.0-mL samples "A" and "B" (both containing HCl) were titrated with 0.100 M NaOH. When titrating sample "A", it took 23.8 mL of titrant to reach the endpoint. When titrating sample "B", it also took 23.8 mL of titrant to reach the endpoint. Which of the following is correct? a. Sample A has a higher concentration of HCl b. Sample B has a higher concentration of HCl c. Sample A has the same concentration as Sample B d. We are unable to deduce the concentration of either sample.
15.0 mL of H2SO4 was neutralized with 35.0mL of 0.25 M NaOH. Write balanced equation for neutralization and determine the concentration of H2SO4?
Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI
1. Calculate the volume of 6.0M NaOH needed to make 0.50 L of 0.15M NaOH. 2. Determine the mass of H₂C2O4 2H₂O(s) needed to make 250. mL of 0.10M H₂C2O4. 3. If 32.96 mL of a NaOH solution are required to titrate 25.00 mL of 0.1042M H₂C₂O4 to the end point, what is the molarity of the sodium hydroxide? 4. If 24.92 mL of the NaOH solution from question 3 are required to titrate 0.2794 g of an unknown diprotic (n = 2) acid, what is its molar mass?
1. An aqueous solution of Ca(OH)2with a concentration of 0.146 M was used to titrate 25.00 mL of aqueous HCl. 12.03 mL of the Ca(OH)2was required to reach the endpoint of the titration. a. How many moles of base were required to react completely with the acid in this reaction? b. How many moles of HCl were present in the original 25.00 mL of acid? c. What is the molarity of the original HCl solution?
Calculate the volume (mL) of 0.120 M HCl to completely react with 0.1200 g of Na2CO3 (MW = 105.989 g/mole). This volume corresponds to the equivalence point. write the balanced equation for the reaction between HCl and Na2CO3. Determine the number of moles of HCl to completely react based on the mass of Na2CO3. Calculate the volume of the HCl solution to reach the equivalence point based on concentration of the HCl solution. Report the volume in mL.
A solution contains either Cr3+ or Ni2+ ion. Describe a reaction with a single reagent that will identify which ion is present.
A 15.00 mL sample of a NaOH solution was titrated with a 0.1053 M H2SO4 solution. If 17.88 mL of H2SO4 was used to reach the equivalence point, what is the concentration of NaOH? 3.011 M O 1.502 M 0.02510 M 0.2510 M
Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka 2.8 x 10 ) and KOBr and testing its behavior when strong acid or base is added to it. = Part 1 First, Lareina combines 81.42 g KOBr and 245 mL of 1.70 M HOBr, and adds enough distilled water to make 950 mL of solution. What is the pH of this solution? pH solution= Part 2 Next, Lareina adds 12.0 mL of 2.40 M HNO₂ to 385 mL of the solution made in Part 1. What is the pH of the solution after the HNO is added? pH after HNO, added = Part 3 Finally, Lareina 18.0 mL of 2.10 M NaOH ito 375 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added=
You 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 17.54 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?
Give typed solution not written
Question #7 Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka = 2.8 x 10-9) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 90.54 g KOBr and 255 mL of 1.30 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution? pH solution Part 2 = Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 350 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added? pH after HNO3 added Part 3 = Finally, Lareina adds 12.0 mL of 2.20 M NaOH ito 370 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =