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3, Assuming that the equilibeium FeNCS2 concentration is 6.06 x 1os Min a solution that initially...
1.20 x 10- and Ka - 5.37 x 10-Determine the pll of 0.259 M Maleic acid...
1.20 x 10- and Ka - 5.37 x 10-Determine the pll of 0.259 M Maleic acid (H.CH,0,) is a diri acid with K maleic acid ( HC,H,O,) solution. < Hint pH = Because Kal is much larger than Kas you can assume that very little of the intermediate species (HC, H, 0) will dissociate and that the diprotic acid acts like a monoprotie acid.
What's the concentration of [FeSCN2+] using limiting reactant theory and equation? For each test tube solution...
What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...
Calculate the initial concentration of iron(III) in
solution #1, #2, #3.
Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iron Fe(NO3)3 2.50 x 10 in 0.10 M HNO3 nitric acid HNO3 0.10 120 35 50 250 conc. SCN KSCN 0.50 30 50 dilute SCN KSCN 2.50 x 10-3 30 50 Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5...
can you please answer 1,2, and 3 and show the steps 1. Calculate the pH of...
can you please answer 1,2, and 3 and show the steps
1. Calculate the pH of a buffer solution made by adding 20.0 mL of 0.200 M acetic acid solution with 10.0 mL of a 0.200 solution of sodium acetate. K, for acetic acid is 1.8 x 109. Assume the total volume is 30.0 mL. 2. Calculate the pH of a buffer solution made by mixing 10.0 mL of 0.20 M ammonia with 15.0 mL of 0,15 M ammonium chloride...
For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x...
For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x 10 M AgNO3 with 200mL of 5.0M Na S O The stepwise formation equilibria are Ag +S203 Ag (S2O3) Ag(S2O3) +S20, Ag(S20s)2 17. What is the concentration of Ag(S203) in solution (5 points): A. 3.8x 10 B. 1.8 x 10 18 C. 4.3x 10 D. 5.6 x 10 K1 7.4 x 10 K2 3.9 x 104
3. How much solid NaCN must be added to 1.0 L of a 0.5 MHCN solution...
3. How much solid NaCN must be added to 1.0 L of a 0.5 MHCN solution to produce a solution with pH 7.0? K. - 6.2 x 10- for HCN. K 4. The following table shows many acid/base pairs with the corresponding K, values on the right. ACID/BASE 1.0 M NaHSO4/ 1.0M Na2SO4 1.2 x 10-2 1.0M HCIO/ 1.0M KCIO 3.5 x 10- 1.0M NH4Cl 1,0M NHI 5.6 x 10-10 1.0M (CH3)2NHCI/1.0M (CH3)2N 1.5 x 10-10 1.0M Na2HPO4/ 1.0M Na...
Determine the [H_3 O^+] in an aqueous solution of hypothetical diprotic acid, H_2 X, that is...
Determine the [H_3 O^+] in an aqueous solution of hypothetical diprotic acid, H_2 X, that is 0.10 M in H_2 X. (K_a1 = 1.0 times 10^-7, K_a2 = 1.0 times 10^-12) 1.0 times 10^-12 1.0 times 10^-19 1.0 times 10^-18 1.0 times 10^-4 0.10
A 15 L buffer solution is 0.250 Min HF and 250 M in Ne Calculate the...
A 15 L buffer solution is 0.250 Min HF and 250 M in Ne Calculate the pH of the solution after the addition of 0.0500 moles of sold NOH. Assume no volume change upon the addition of base. The K, for HF 35 x 104 351 3.54 3.46 3.63 Which of the following is TRUE? An effective buffer has a [base)(acid] ratio in the range of 10 -100. A buffer can not be destroyed by adding too much strong base....
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that...
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528 at 540 nm given that a 2.75 x 10A-4 M solution has an absorbance of .487 at 540 nm a. 2.98 x 10A-4 M B.) 3.35 x 10A3 M .)9.64 x 10 A-7 d.12.54 x 10 4 4. Calculate the equilibrium constant for the reaction Fe3+ (ago+SCN (aq) FescN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of...
1.20 x 10- and Ka - 5.37 x 10-Determine the pll of 0.259 M Maleic acid (H.CH,0,) is a diri acid with K maleic acid ( HC,H,O,) solution. < Hint pH = Because Kal is much larger than Kas you can assume that very little of the intermediate species (HC, H, 0) will dissociate and that the diprotic acid acts like a monoprotie acid.
What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
Calculate the initial concentration of iron(III) in
solution #1, #2, #3.
Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iron Fe(NO3)3 2.50 x 10 in 0.10 M HNO3 nitric acid HNO3 0.10 120 35 50 250 conc. SCN KSCN 0.50 30 50 dilute SCN KSCN 2.50 x 10-3 30 50 Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5...
can you please answer 1,2, and 3 and show the steps
1. Calculate the pH of a buffer solution made by adding 20.0 mL of 0.200 M acetic acid solution with 10.0 mL of a 0.200 solution of sodium acetate. K, for acetic acid is 1.8 x 109. Assume the total volume is 30.0 mL. 2. Calculate the pH of a buffer solution made by mixing 10.0 mL of 0.20 M ammonia with 15.0 mL of 0,15 M ammonium chloride...
For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x 10 M AgNO3 with 200mL of 5.0M Na S O The stepwise formation equilibria are Ag +S203 Ag (S2O3) Ag(S2O3) +S20, Ag(S20s)2 17. What is the concentration of Ag(S203) in solution (5 points): A. 3.8x 10 B. 1.8 x 10 18 C. 4.3x 10 D. 5.6 x 10 K1 7.4 x 10 K2 3.9 x 104
3. How much solid NaCN must be added to 1.0 L of a 0.5 MHCN solution to produce a solution with pH 7.0? K. - 6.2 x 10- for HCN. K 4. The following table shows many acid/base pairs with the corresponding K, values on the right. ACID/BASE 1.0 M NaHSO4/ 1.0M Na2SO4 1.2 x 10-2 1.0M HCIO/ 1.0M KCIO 3.5 x 10- 1.0M NH4Cl 1,0M NHI 5.6 x 10-10 1.0M (CH3)2NHCI/1.0M (CH3)2N 1.5 x 10-10 1.0M Na2HPO4/ 1.0M Na...
Determine the [H_3 O^+] in an aqueous solution of hypothetical diprotic acid, H_2 X, that is 0.10 M in H_2 X. (K_a1 = 1.0 times 10^-7, K_a2 = 1.0 times 10^-12) 1.0 times 10^-12 1.0 times 10^-19 1.0 times 10^-18 1.0 times 10^-4 0.10
A 15 L buffer solution is 0.250 Min HF and 250 M in Ne Calculate the pH of the solution after the addition of 0.0500 moles of sold NOH. Assume no volume change upon the addition of base. The K, for HF 35 x 104 351 3.54 3.46 3.63 Which of the following is TRUE? An effective buffer has a [base)(acid] ratio in the range of 10 -100. A buffer can not be destroyed by adding too much strong base....
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528 at 540 nm given that a 2.75 x 10A-4 M solution has an absorbance of .487 at 540 nm a. 2.98 x 10A-4 M B.) 3.35 x 10A3 M .)9.64 x 10 A-7 d.12.54 x 10 4 4. Calculate the equilibrium constant for the reaction Fe3+ (ago+SCN (aq) FescN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of...
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