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![..fe (OH), → Fe 3+ + 30H- Ksp = [Fe3+] [OH-] 3 @ for water as a solvent [H+] = [OH-] = 10-7 M. 7, Ksp = 4x10-38 [Fe3+] = Kg](http://img.homeworklib.com/questions/264bf370-d200-11eb-b43b-d54023f7f162.png?x-oss-process=image/resize,w_560)
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This question has multiple parts. Work all the parts to get the most...
Raferences) This question has multiple parts. Work all the parts to get the most points. A...
Raferences) This question has multiple parts. Work all the parts to get the most points. A buffer consists of 0.96-M propanoic acid (K-1.4 x 10) and 0.88-M sodium propanoate. a Calculate the pH of this buffer. pH-4.81 Correct b Calculate the pH after the addition of 2.1 mL of 0.10-M HCl to 0.010 L of the buffer pH-4.79 Correct c Calculate the pH after the addition of 8.8 mL of 1.0-M HCl to 0.010 L of the buffer. pH Submit...
i need help on C This question has multiple parts. Work all the parts to get the most points. buffer consists of 0.9...
i need help on C
This question has multiple parts. Work all the parts to get the most points. buffer consists of 0.96-M propanoic acid (K, -1.4 x 10 ) and 0.88-M sodium propanoate a Calculate the pH of this buffer. pH = 4.81 0 Correct b Calculate the pH after the addition of 2.1 mL of 0.10 M HCl to 0.010 L of the buffer. pH = 4.79 vô Correct C Calculate the pH after the addition of 8.8...
just b please thank you. This question has multiple parts. Work all the parts to get...
just b please thank you.
This question has multiple parts. Work all the parts to get the most points. A titration of 21.7 mL of a solution of the weak base aniline, CH NH, (K) = 4.0 x 10-1), requires 24.35 mL of 0.175 M HCl to reach the equivalence point. C.H NH, (aq) + H, 0+ (aq) = CH NH,+ (aq) + H, 0(1) a What was the concentration of aniline in the original solution? Concentration - 196 MV...
This question has multiple parts. Work all the parts to get the most points. The titration...
This question has multiple parts. Work all the parts to get the most points. The titration of 50.00 mL of 0.130-M HCl with 0.130-M NaOH (the titrant) is carried out in a chemistry laboratory. Calculate the pH of the solution after these volumes of the titrant have been added: a i. 0.00 mL pH = .88 ii. 25.00 mL pH = 1.37 ✓ iii. 49.9 mL pH = 4 Correct Result: i. 0.886 ii. 1.363 iii. 3.9 Analyze: Initially heherinaridisconto...
This question has multiple parts. Work all the parts to get the most points. Draw the...
This question has multiple parts. Work all the parts to get the most points. Draw the complete mechanism for the radical reaction shown. CH4 + light Cl2 CH3CI a Use curved arrows to show the mechanism of the initiation step below. Make the ends of your arrows specify the origin and destination of reorganizing electrons. Arrow-pushing Instructions no XT : —: light, An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
HELP PLEASE 5 – Calculate the concentrations of H+, HCO3- and CO32- in a 0.025 M...
HELP PLEASE 5 – Calculate the concentrations of H+, HCO3- and CO32- in a 0.025 M H2CO3 solution. 6 – Classify the following as a Lewis acid, Lewis base, both or neither:CO2, H2O, I-, SO2, NH3, OH-, H+, BCl37 – 7-Calculate the pH of a solution that is 0.20 M NH3 and 0.30 M NH4Cl.8 – 8-The pH of blood plasma is 7.40. Assuming the principal buffer system is HCO3-/H2CO3, calculate the ratio [HCO3-]/[H2CO3] . 9 – A 0.2688 g...
This question has multiple parts. Work all the parts to get the most points. a Calculate...
This question has multiple parts. Work all the parts to get the most points. a Calculate the pH of a solution that is 0.20 M HOCl and 0.86 M KOC). Ka=3.5x10-8 pH = Submit
help me out, please! answer all the multiple choice. (15) A phosphate buffer solution is prepared by mixing 100. m...
help me out, please! answer all the multiple
choice.
(15) A phosphate buffer solution is prepared by mixing 100. mL. of 0.300 M KH PO, and 150.ml 0.500 M K HPO (a) Calculate the molar concentrations of H:PO, and that of HPO,2 in the buffer solution. (b) What is the pH of the buffer solution? (H,PO, has K,-6.2 x 10 (c) Write a net ionic equation for the bufering reaction against a strong acid, Hjo (d) Calculate the new concentration...
This question has multiple parts. Work all the parts to get the most points. A 50.00-mL aliquot of 0.1900 M NaOH is tit...
This question has multiple parts. Work all the parts to get the most points. A 50.00-mL aliquot of 0.1900 M NaOH is titrated with 0.1900 M HCl. Calculate the pH of the solution after the addition of (Use a spreadsheet to complete this question.) a 0.00 mL of acid pH = 10.00 mL of acid pH = 40.00 mL of acid pH = 45.00 mL of acid pH = 49.00 mL of acid pH = 50.00 mL of acid pH...
This question has multiple parts. Work all the parts to get the most points. a What...
This question has multiple parts. Work all the parts to get the most points. a What mass of HCl does 1.39 L of 7.50 M HCl solution contain? Mass = g HCI b What mass of NaOH does 11.3 mL of 0.260 M NaOH solution contain? Mass = g NaOH What mass of HNO3 does 251 mL of 1.77 M HNO3 solution contain? Mass = g HNO3 d What mass of CaCl, does 3.65 L of 0.522 M CaCl, solution...
Raferences) This question has multiple parts. Work all the parts to get the most points. A buffer consists of 0.96-M propanoic acid (K-1.4 x 10) and 0.88-M sodium propanoate. a Calculate the pH of this buffer. pH-4.81 Correct b Calculate the pH after the addition of 2.1 mL of 0.10-M HCl to 0.010 L of the buffer pH-4.79 Correct c Calculate the pH after the addition of 8.8 mL of 1.0-M HCl to 0.010 L of the buffer. pH Submit...
i need help on C
This question has multiple parts. Work all the parts to get the most points. buffer consists of 0.96-M propanoic acid (K, -1.4 x 10 ) and 0.88-M sodium propanoate a Calculate the pH of this buffer. pH = 4.81 0 Correct b Calculate the pH after the addition of 2.1 mL of 0.10 M HCl to 0.010 L of the buffer. pH = 4.79 vô Correct C Calculate the pH after the addition of 8.8...
just b please thank you.
This question has multiple parts. Work all the parts to get the most points. A titration of 21.7 mL of a solution of the weak base aniline, CH NH, (K) = 4.0 x 10-1), requires 24.35 mL of 0.175 M HCl to reach the equivalence point. C.H NH, (aq) + H, 0+ (aq) = CH NH,+ (aq) + H, 0(1) a What was the concentration of aniline in the original solution? Concentration - 196 MV...
This question has multiple parts. Work all the parts to get the most points. The titration of 50.00 mL of 0.130-M HCl with 0.130-M NaOH (the titrant) is carried out in a chemistry laboratory. Calculate the pH of the solution after these volumes of the titrant have been added: a i. 0.00 mL pH = .88 ii. 25.00 mL pH = 1.37 ✓ iii. 49.9 mL pH = 4 Correct Result: i. 0.886 ii. 1.363 iii. 3.9 Analyze: Initially heherinaridisconto...
This question has multiple parts. Work all the parts to get the most points. Draw the complete mechanism for the radical reaction shown. CH4 + light Cl2 CH3CI a Use curved arrows to show the mechanism of the initiation step below. Make the ends of your arrows specify the origin and destination of reorganizing electrons. Arrow-pushing Instructions no XT : —: light, An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
This question has multiple parts. Work all the parts to get the most points. a Calculate the pH of a solution that is 0.20 M HOCl and 0.86 M KOC). Ka=3.5x10-8 pH = Submit
help me out, please! answer all the multiple
choice.
(15) A phosphate buffer solution is prepared by mixing 100. mL. of 0.300 M KH PO, and 150.ml 0.500 M K HPO (a) Calculate the molar concentrations of H:PO, and that of HPO,2 in the buffer solution. (b) What is the pH of the buffer solution? (H,PO, has K,-6.2 x 10 (c) Write a net ionic equation for the bufering reaction against a strong acid, Hjo (d) Calculate the new concentration...
This question has multiple parts. Work all the parts to get the most points. A 50.00-mL aliquot of 0.1900 M NaOH is titrated with 0.1900 M HCl. Calculate the pH of the solution after the addition of (Use a spreadsheet to complete this question.) a 0.00 mL of acid pH = 10.00 mL of acid pH = 40.00 mL of acid pH = 45.00 mL of acid pH = 49.00 mL of acid pH = 50.00 mL of acid pH...
This question has multiple parts. Work all the parts to get the most points. a What mass of HCl does 1.39 L of 7.50 M HCl solution contain? Mass = g HCI b What mass of NaOH does 11.3 mL of 0.260 M NaOH solution contain? Mass = g NaOH What mass of HNO3 does 251 mL of 1.77 M HNO3 solution contain? Mass = g HNO3 d What mass of CaCl, does 3.65 L of 0.522 M CaCl, solution...
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