Homework Answers
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN.
A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN. The student finds that the equilibrium concentration of FeSCN2+ is 5.6 x 10-4M. a. Set up the Kc expression for the following equation. Fe3+ + SCN- ↔ FeSCN2+b. What is the total volume of the solution? _______ mL c. Fill in the following table for the moles of each species.d. Find the concentration for the above ions. e. Calculate Kc for the reaction.
Calculate the concentrations of NaOH and maleic acid. 100 mL of 0.1 M NaOH was transferred...
Calculate the concentrations of NaOH and maleic acid. 100 mL of 0.1 M NaOH was transferred into a buret. 0.433 g of maleic acid was dissolved in a 100 mL volumetric flask. 25 mL of this solution was transferred into a plastic beaker, and 50 mL of distilled water was added. 6 mL of NaOH was added to get to the first equivalence point (brought pH to 1.99), and a total of 30 mL was added to reach the second...
Calculate the solubility at 25°c of CuBr in pure water and in a 0.0150 M CoBr,...
Calculate the solubility at 25°c of CuBr in pure water and in a 0.0150 M CoBr, solution. You'll find K, data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: 0 solubility in 0.0150 M CoBr2 solution: 0 x 6 ?
3. A 25.00 mL 0.0250 M calcium carbonate sample is titrated with 14.3 mM EDTA solution....
3. A 25.00 mL 0.0250 M calcium carbonate sample is titrated with 14.3 mM EDTA solution. Both sample and titrant are buffered at pH = 10.0 a. What is the titration reaction and what is the value of the conditional formation constant? b. What is the calcium ion concentration when 12.35 mL of titrant has been added? c. What is pCa2+ at the equivalence volume?
This problem deals with Acid-base titrations and pH scale for a weak acid and a weak...
This problem deals with Acid-base titrations and pH scale for a weak acid and a weak base. Calculate the pH of the solution that results from adding 7.5 [ml] of Ammonia (NH3) to a beaker that contains, 100 ml of distilled water and 15 ml of 0.1 M Acetic acid (HC2H3O2). A buret containing 50 mL of 0.1 M Ammonia (NH3) is being used as the titrant. The beaker containing 100 ml of distilled water, and 15 ml of 0.1...
We Have 1.250 M HCIO4 150.0 ML, What Will Be The New Concentration If 825.0 ML...
We Have 1.250 M HCIO4 150.0 ML, What Will Be The New Concentration If 825.0 ML More Water Is Added? (answer: 0.1923 Mol/L) 10. In A Beaker, We Add 0.50 ML Of 0.350 M Of AIBr3, 1.25 ML 0.467 M Of Ba(OH)2 And 9.25 ML Of Water. Please Calculate The Concentrations (morlarity) Of Bromide Ion And Hydroxide Ion In The Beaker Before The Chemical Reaction
Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) +...
Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) + H_2O(l) Calculate Delta G degree rxn using the following information HNO_3 (aq) NO(g) NO_2(g) H_2O(l) Delta H^degree (kJ/mol) -207 91.3 33.2 -285. 8 S^degree (J/mol K) 146 210.8 240.1 70.0 Calculate the value of the equilibrium constant, K, at 25 degree C At 25 degree C does the above reaction favor reactant or product formation? What evidence supports your conclusion? Procedure: Obtain the five...
Canvas +→ COD cuvet Question 11 25 pts A reaction mixture of 4.00 mL of 0.00200...
Canvas +→ COD cuvet Question 11 25 pts A reaction mixture of 4.00 mL of 0.00200 M SCN and 5.00 mL of 0.00200 M Fetis diluted to 10.00 mL with 0.1 MHNO, to form the blood-red FeNCS complex. The equilibrium molar concentration of the FeNCS?determined from a calibration curve, is 1.5 x 10 mol/L. Calculate the equilibrium constant for the reaction shown below. Fe3+ (aq) + SCN-(aq) + FENCS?+ (aq) HINT: Be sure to account for the dilutions of the...
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
Calculate the solubility at 25°c of CuBr in pure water and in a 0.0150 M CoBr, solution. You'll find K, data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: 0 solubility in 0.0150 M CoBr2 solution: 0 x 6 ?
Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) + H_2O(l) Calculate Delta G degree rxn using the following information HNO_3 (aq) NO(g) NO_2(g) H_2O(l) Delta H^degree (kJ/mol) -207 91.3 33.2 -285. 8 S^degree (J/mol K) 146 210.8 240.1 70.0 Calculate the value of the equilibrium constant, K, at 25 degree C At 25 degree C does the above reaction favor reactant or product formation? What evidence supports your conclusion? Procedure: Obtain the five...
Canvas +→ COD cuvet Question 11 25 pts A reaction mixture of 4.00 mL of 0.00200 M SCN and 5.00 mL of 0.00200 M Fetis diluted to 10.00 mL with 0.1 MHNO, to form the blood-red FeNCS complex. The equilibrium molar concentration of the FeNCS?determined from a calibration curve, is 1.5 x 10 mol/L. Calculate the equilibrium constant for the reaction shown below. Fe3+ (aq) + SCN-(aq) + FENCS?+ (aq) HINT: Be sure to account for the dilutions of the...
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