Use the following information to answer the next question. A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture w filtered and further tests were done on the filtrate. The results are as follows. First test: solution is a pink colour NaIO3(aq) added and no precipitate forms Second test: Third test: flame colour is red Fourth test: NazCO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a. lithium and cobalt(II) O b. strontium and cobalt(II) Oc. lithium and manganese(II) O d. strontium and manganese(II)

Use the following information to answer the next question. A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture w filtered and further tests were done on the filtrate. The results are as follows. First test: solution is a pink colour NaIO3(aq) added and no precipitate forms Second test: Third test: flame colour is red Fourth test: NazCO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a. lithium and cobalt(II) O b. strontium and cobalt(II) Oc. lithium and manganese(II) O d. strontium and manganese(II)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A solution containing a mixture of metal cations was treated with dilute HClHCl and a precipitate formed. The solution was filtered, and H2SH2S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 88 and H2SH2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in the formation of a precipitate. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it was possible they were present in the original mixture.
• An unknown acid (HA) was titrated with NaOH(aq). • The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 2. 4 9. 8. 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Which of the following net ionic equations explains the pH of the analyte solution before any titrant is added? A (aq) + H20(1) HA(aq) + OH (aq) A (aq) + H3O*(aq) --> HA(aq) + H20(1) O H*(aq) + OH (aq) H20(1) --> O HA(aq) + OH (aq) --> H2O(aq) + A (aq) HA(aq) + H20() H3O*(aq) + A (aq)
2. After dissolving the KHP with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 sec and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared! a) What happened? b) What can the student do to correct for this erTor and salvage this trial? How should the data sheet be modified to reflect this correction? 3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red! a) What happened? b) What can the student do to correct for this error and salvage this trial? How should the data sheet…
10.00mL of 0.10M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: Ignore the volume of the indicator added, as the volume is tiny compared to 100mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00mL of 0.100M NaOH? Question 3 options: 7.22 6.9 8.35 7.00
Why is it normal to add a slight excess of silver nitrate solution when precipitating chloride ion?
A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Ag* Hg²+ Lit Ba²+ Pb2+ Mg²+ Hg3* 2+ Answer Bank Zn2+ Sn2+ Ni2+ Cu2+ Bi3+ A13+ Incorrect
why is it important in the heavy metal test to look for new precipitation (solid)?
A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a pink colourNaIO3(aq) added and no precipitate formsflame colour is redNa2CO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a.lithium and manganese(II) b. strontium and cobalt(II) c. strontium and manganese(II) d. lithium and cobalt(II)
Calcium and magnesium ions can occur in our water supplies (e.g. through rocks and geological formations). A sample of tap water was tested and the calcium ion concentration was measured at 2.1E-5M and the magnesium ion concentration was measured at 1.2E-3M. If carbonate ion is added into the tap water, which ion will precipitate out of solution first? Explain your reasoning. The Ksp values of CaCo3 and MgCO3 are 5.0E-9 and 6.8E-6, respectively.
We have 4 test tubes filled with aqueous solution, one of which is definitely yellow. Use the information below to determine the composition of the solutions. Give the name of the cation and anion of the compunds! (there will be 4) Upon pooling of the contents of tubes 1 and 2, a white precipitate is formed which dissolves not in nitric acid but in ammonia. A yellow precipitate forms when the contents of tubes 1 and 3 are combined. When the contents of tubes 1 and 4 were combined, a brown precipitate formed. The solution turns brown when the contents of tubes 2 and 3 are combined. A yellow precipitate forms when the contents of tubes 1 and 3 are combined. When the contents of tubes 2 and 4 were combined, a reddish-brown, gelatinous precipitate formed which did not dissolve in excess reagent. No change is made when the contents of tubes 3 and 4 are pooled. Aqueous solutions of some tubes give a positive reaction to potassium and nitrate ions and must not contain sodium ions.
SOLVE THE FOLLOWING PROBLEM AND SHOW YOUR COMPLETE SOLUTIONS. EXPLAIN YOUR ANSWERS FOR BETTER UNDERSTANDING.
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%)