Pre-lab question 1: Standard solutions are made using the volumes and concentrations listed in the table below. Calculate the final concentration of SCN and FeSCN2+ in the solution. Report all calculations involving the NaSCN data to 3 significant figures. A B C D E F Volume 0.00200 M 0.25 mL 0.50 mL 0.75 mL 1.00 mL 1.25 mL 6.00 mL NaSCN added mL [Fe3+] 0.200M added Approximate [Fe3+] in solution Mol NaSCN added Mol SCN added [SCN] ion in standard solution [FeSCN²+] in standard solution Absorbance 0.043 0.087 0.125 0.173 0.211 1.050

84 mL of 0.060 M NaF is mixed with 28 mL of 0.15 M Sr(NO3)2. Calculate the concentration of Sr2+ in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0 × 10-10) A. 0.038 M B. 0.00012 M C. 0.015 M D. 0.045 M E. 0.075 M

What is the mass percent of Fe for each trial ?   Mass of (NH4)2Ce(NO3)6 (in 100.00 mL) =   4.5038 g             Mass of unknown (in 250.00 mL) = 10.000 g     Trial # Volume of unknown solution (mL) Titration Volume (mL of Ce4+) Mass Percent(% Fe) 1 25.00 mL 7.20 mL   2 25.00 mL 7.40 mL   3 25.00 mL 7.60 mL   4 25.00 mL 7.50 mL

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

Answ GA 20. Answ My C X C Write C The F X C Whe x akeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. When 25.0 mL of a 1.99×104 M lead nitrate solution is combined with 15.0 mL of a 6.28×10-4 M sodium iodide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to Submit Answer Retry Entire Group 1 more group attempt remaining क Ni ENG US Home End Ins

Which of the following compounds is the most soluble in water based on its Ksp value? A. CuS, Ksp = 1.27 x 10^-36B. PbS, Ksp = 9.04 x 10^-29C. AgCl, Ksp = 1.77 x 10^-10D. AgI, Ksp = 8.51 x 10^-17E. There is not enough information in the prompt to answer this question.

5. A D CHEMISTRY 1110L LAB REPORT: PERIODIC PROPERTIES OF METALS Part One 1. Color of test solutions: 1 M Na₂CO3 1 M LICI 0.1 M MgCl₂ 0.1 M BaCl₂ Part Two 71FX Part Three 4. Flame colors and solubilities of the six unknown solutions Unknown A B C D E 0.1 M SrCl₂ 2. Does the color of the sodium flame depend upon the anion used? Why? F HWIS-1 MgClz CaCl₂ SrCl₂ BaCl, 3. Do you observe a trend in solubilities for the Group IIA sulfates? Group IIA carbonates? Does solubility increase or decrease as you go down a group? Color of Flame Identity of the Six Unknown Solutions B H₂SO4 Name Partner Desk # H₂SO4 1M NaCl 1M KBr 0.1 M CaCl, F Na₂CO3 Na₂CO3 32

Students performed three KHP titrations in Part 1 to standardize their NaOH solution. They reported the following measurements:   Determination #1 Determination #2 Determination #3 Mass of KHP + Vial 14.0862 g 14.5621 g 14.3998 g Mass of 'Empty' Vial 13.2492 g 13.7695 g 13.6887 g Final Burette Reading 45.10 mL 38.53 mL 37.17 mL Initial Burette Reading 5.08 mL 0.52 mL 3.19 mL How many moles of NaOH did they use in their first titration? Report your answer to the correct number of significant figures

Part A Determine if each compound shown is soluble or insoluble. Drag the appropriate items to their respective bins. View Available Hint(s) Soluble Submit BaSO4 AICI KCI KBr Cu(NO3)2 Cu(OH)₂ NaNO₂ NaCl Hgala Insoluble Reset Help

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