Table 15.3 Composition of solutions for the determination of Kc 0.00200 M Fe(NO3)3 (in 0.1 M HNO3) 0.00200 M NaSCN (in 0.1 M HNO3) Solution 0.1 M HNO3 Blank 5.00 mL 0.00 mL 5.00 mL 1 5.00 mL 1.00 mL 4.00 mL 2 5.00 mL 2.00 mL 3.00 mL 3 5.00 mL 3.00 mL 2.00 mL 5.00 mL 4.00 mL 1.00 mL 5.00 mL 5.00 mL 0.00 mL

Table 15.3 Composition of solutions for the determination of Kc 0.00200 M Fe(NO3)3 (in 0.1 M HNO3) 0.00200 M NaSCN (in 0.1 M HNO3) Solution 0.1 M HNO3 Blank 5.00 mL 0.00 mL 5.00 mL 1 5.00 mL 1.00 mL 4.00 mL 2 5.00 mL 2.00 mL 3.00 mL 3 5.00 mL 3.00 mL 2.00 mL 5.00 mL 4.00 mL 1.00 mL 5.00 mL 5.00 mL 0.00 mL

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 108A

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In preparing solution with 5.0 mL 2.00 x 10-3 M Fe(NO3)3 in 0.50 M HNO3 + 2.0 mL 2.00 x 10-3 M HSCN in 0.50 M HNO3 and 3.0 mL of 0.50 M HNO3. (The solvent for Fe(NO3)3 and HSCN solutions in 0.50 M HNO3). After combining these, what are the concentrations of Fe3+, HSCN, and H+ in the resulting solution?
What is the cobalt(II) ion concentration in a solution prepared by mixing 357 mL357 mL of 0.396 M0.396 M cobalt(II) nitrate with 475 mL475 mL of 0.399 M0.399 M sodium hydroxide? The ?spKsp of cobalt(II) hydroxide is 5.92×10−155.92×10−15 .
For which of the mixtures will Ag2SO4(s) precipitate? 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)
Consider a solution made by mixing 500.0 mL of 4.0M NH3 and 500.0mL of 0.40MAgNO3.Ag+ reacts with NH3, to form AgNH3+ and Ag(NH3)2+: Ag+(aq)+NH3(aq)AgNH3+(aq)+NH3(aq)⇌AgNH3+(aq)⇌Ag(NH3)2+(aq)K1=2.1×103K2=8.2×103 Determine the concentration of all species in solution. asap please.
Calculate the concentration of SCN in each of the following standard solutions. Use 0.0500 M Fe3+ and 0.00200 M SCN- a. 1.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) b. 2.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) c. 3.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) d. 4.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL)
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Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
set to standardize a solution of Mg(OH)2 with potassium hydrogen phthalate (KHP, M.W. = 204.22 g/mole): 2 KHPlaq) + Mg(OH)2/ag) = K2Plaq) + MPlaq) + 2 H2010 If 2.456 g KHP are dissolved in 50.0 mL H2O and the following burette readings for Mg(OH)2 are used what is the concentration of Mg(OH)2? Vinitial = 9.85 mL and Vinal = 34.94 mL
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Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 669669 mg of AgCl(s) in 100.0 mL of solution. The KspKsp of AgCl is 1.77×10−101.77×10−10.
When all of the following are mixed together in a beaker, what is the molar concentration of the SCN- ion in the solution just after mixing but before any reaction takes place? 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 4.00 mL of 2.00 x 10-3 M KSCN 4.00 mL of 0.50 M HNO3 answer is between 0.004 and 0.005, please explain how with steps.