296 Experiment 36 Qualitative Analysis of Group I Cations 4. You are given an unknown solution that contains only one of the Group I cations and no other metallic cations. Develop the simplest procedure you can think of to determine which cation is present. Draw a flow diagram showing the procedure and the observations to be expected at each step with each of the possible cations. The information in Appendix IIA should be helpful.

296 Experiment 36 Qualitative Analysis of Group I Cations 4. You are given an unknown solution that contains only one of the Group I cations and no other metallic cations. Develop the simplest procedure you can think of to determine which cation is present. Draw a flow diagram showing the procedure and the observations to be expected at each step with each of the possible cations. The information in Appendix IIA should be helpful.

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...

See similar textbooks

Similar questions

Consider the colored precipitates you produced and the cations in those reactions. Identify the colorful cations and describe their location on the periodic table. What do they have in common? Select the statement that best answers the question They are from the same row on the periodic table They are from the same column on the periodic table They are all nonmetals They are transition metals They are all alkali metals
If your concentrations of acetic acid and sulfuric acid were the same, would you have to add the same or different amounts of titrant? Explain your answer using the chemicals formulas and the acid/base neutralization reactions involved in this experiment. Molarity acetic acid: 0.985 Molarity of Sulfuric acid: 0.519M
A balloon has a temperature of 56 C at 907 tor.what is the pressure if the temperature reaches 89 C?
PRE-LAB QUESTIONS 1. A student dissolves 2.006 g of FeSO4-7 H₂O in 40 mL of sulfuric acid and then dilutes it to 100.00 mL in a volumetric flask as described is Procedure steps 3-7. He then uses a pipet to transfer 10.00 mL of this solution into a flask for titration as in Procedure step 11. What mass of FeSO4-7 H₂O was transferred into the titration flask? (Keep this question in mind as you do your calculations for Pre-Lab Question 2 and for your calculations with your own data.) 2. Your partner has completed three acceptable titrations for standardizing the dilute potassium permanganate solution and he gives you all of the data. The solid standard used was FeSO4-7 H₂O, and it was dissolved and diluted to 100.00 mL. a. Calculate the molarities for the trials (Hint: you are going to need the balanced ionic equation and the formula mass of ferrous sulfate heptahydrate.) Mass of Standard Volume of Blank Volume of Standard Initial Buret Reading Final Buret Reading Volume of Titrant…
The antacid "Brand X" was titrated using 0.3 M HCl. The buret reading was initially 1.34 mL. After reaching the endpoint, the final volume reading was 12.67 mL. What volume of HCl was used in this titration? Include a unit in your answer.
Using solubility rules, predict the solubility in water of the following ionic compounds. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. PbS- AgNO3- Na2CO3- CaI2-
Suppose you are performing a titration. At the beginning of the titration, you read the titrant volume as 2.75 mL. After running the titration and reaching the endpoint, you read the titrant volume as 17.43 mL. What volume, in mL, of titrant was required for the titration?
1. Observe the physical properties of sulfur and antimony at room temperature. Note their physical state, color and solubility in carbon disulfide. The solubility may be observed qualitatively by dissolving a pinch of the powdered samples in about 3 ml of carbon disulfide and stirring until the solid sample has dissolved. Record your observations in the table below. Solubility in CS, Classification of the sample (Element/Compound) Sample Physical Color State Sulfur Antimony a. Was the system formed by the addition of sulfur to CS,, homogeneous or heterogeneous? b. Could its composition be varied or not? c. Explain your answer in la. d. Was the system formed by the addition of antimony to CS, homogeneous or heterogeneous? e. Explain your answer in 1d.
During a lab experiment performed at STP conditions, you prepare HCl by reacting 100. ml of Cl2 gas with an excess of H2 gas. How many ml of a solution of Ba(OH)2 0.230M do you need to neutralize all the HCl produced? Please show solution in one string using a dimensional analysis step-by-step.
Question 9 A student is attempting to identify the anion in an unknown solid. The student first dissolves the solid in aqueous solution, and then adds aqueous barium nitrate. A solid product forms. The student then adds hydrochloric acid, which causes the solid to dissolve. Which of the following anions might be in this unknown sample? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Phosphate Nitrate Carbonate d Sulfate e Chloride
MISSED THIS? Watch IWE: Acid-Base Titration; Read Section 5.7. You can click on the Review link to access the section in your e Text. A 17.00 mL sample of an unknown HClO4 solution requires titration with 17.32 mL of 0.1000 M NaOH to reach the equivalence point. Part A What is the concentration of the unknown HC1O4 solution? The neutralization reaction is HClO4 (aq) + NaOH(aq) → H₂O(1) + NaClO4 (aq) Express the molarity to four significant figures. ► View Available Hint(s) M(HCIO4) = Submit Provide Feedback VE ΑΣΦ VO www ? M Next >
If you used no antacid tablet in your titration, you would be titrating 25.00 mL of 0.500 M HCl with 0.100 M NaOH. What volume of NaOH solution would be required to reach neutralization in this case? Since you are using an antacid tablet, will the titration require moreor less NaOH solution than the amount determined in the experiment?