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CHM122 E4 pH Measurement and Calculations Part B For all the substances in this part: anid...
Name 1) W Calculations ADVANCED STUDY ASSIGNMENT The pH of a solution is 5.000. Calculate the...
Name 1) W Calculations ADVANCED STUDY ASSIGNMENT The pH of a solution is 5.000. Calculate the [H*) in the solution. [H'] = Phelos lond sales to [na saugoti 1017) A 1.000 x 10-M solution of sodium carbonate, Na,Co, has a pH of 11.05. A 1.000 x 10-1M solutie Calculate and answer the following: a) [H] b) [OH'] c) Is this solution acidic or basic? d) Write the net ionic equation for this reaction. e) Write the Ko expression for this...
Additional calculations and questions 1. Calculate the expected pH of buffer 1 after adding 1.50 mL...
Additional calculations and questions 1. Calculate the expected pH of buffer 1 after adding 1.50 mL of the 1.00 M NaOH K=1.8 x 10-5 for HCH.O2 2. Calculate the expected pH of buffer 1 after adding 3.00 mL of 1.00 NaOH 3. Write the net ionic equation for the reaction of OH with your buffer. 4. Does adding NaOH raise or lower the concentration of HC2H3O2? 5. Does adding NaOH raise or lower the concentration of NaC2H302? 6. Does adding...
this is part a,b,c of one question. please answer all parts or leave to another tutor....
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
Name Experiment 8 CONCLUSIONS For each part of the experiment, write the balanced molecular react...
Name Experiment 8 CONCLUSIONS For each part of the experiment, write the balanced molecular reaction (using the chart at the end of this experiment to identify precipitates and weak acids). Also write the total ionic reaction and net ionic reaction. No reaction occurred, simply write "NO REACTION" in the space for the molecular reaction. 1 molecular reaction NaCl(aq) + KNO3(aq) total ionic reaction net ionic reaction 2 molecular reaction NaCI(aq)+ AgNO3(aq) total ionic reaction net ionic reaction 3 molecular reaction...
4 stion n an experiment on hydrolysis, the pH values of 0.1M sodium acetate (CHhcoONa) and...
4 stion n an experiment on hydrolysis, the pH values of 0.1M sodium acetate (CHhcoONa) and 0.1 chiorid recorded using pH paper of differentranges. Use these values to determine the correct pH then com Table Abelow DATA AND CALOULATONNS Table A MOH1 Paper Range Wide Range Paper Narrow Range Paper 0.1 MCHvcooNa 4 60 90 95 11 12 Calculations Part B Insert the net ionic equatioms, equilibriumconstant expressions, K. and Ka for the hydrolysable ions, in Table B. Show calculations...
unknown solutions A and B are 0.1 M solutions of either HCI or NaOH. According to your pH measurement, which is which...
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
Fill in the blanks and please show all work for Calculated Ka or Kb column and...
Fill in the blanks and please show all work for Calculated Ka
or Kb column and explain how to find which ion is hydrolyzed
?
Part 1: pH of Solutions of Salts: In this part you will measure the pH values for 0.1 M solutions of the following solutes. Sodium bicarbonate o M Copper(II) sulfate oOM Iron(III) nitrate 010M Sodium acetate O-10M Ammonium chloride O Ib M Sodium fluoride o10 M Methylammonium chloride o.o M For each solution, place the...
Review of Measurement Uncertainty Calculations Here are the rules for propagating uncertainties through a calculation Addition:...
Review of Measurement Uncertainty Calculations Here are the rules for propagating uncertainties through a calculation Addition: z m x + y δ,: 8x + 6y This works for any nunter of terms Subtraction:zx-y o&x + 5y This also works for any number of terns Multiplication by an exact value: z kx 82-kEx General multiplication/division: z-xy or z-:-a-Irl ) (This works for any number of factors) Exact power: z r-δε-121k] sine function: Z t, sin χ-82 tt lcos xlsr Cosine function...
Need help answering all questions. much appreciated. The Relative Strengths of Some Acids Results Solution pH...
Need help answering all questions. much
appreciated.
The Relative Strengths of Some Acids Results Solution pH from pH Paper pH from Indicators pH from pH Meter 2.8 14 1.99 1.4 1.4. HCL Ha POq HC2H30a Na HQ PO & AL (NO3)3 Zn(NO3)2 NH 4 NO3 1.7 1.7 4.63 2.4. 2.8 5.00 6.67 Questions 1. a. Calculate the concentration of H.O ions in the most acidic solution that you examined. Use your most precise pH measurement, 262 alculate the concentration of...
PART C. Properties of Buffers Buffer system selected_HCO -(0,2- Weak acid name _ NaC,H,O, pH of...
PART C. Properties of Buffers Buffer system selected_HCO -(0,2- Weak acid name _ NaC,H,O, pH of buffer 4.68 (H') = 2.09 XIOK 2.09x10 pH of diluted buffer 4.13 [H") = 1.8x10K - 1.8x10-5 pH after addition of five drops of NaOH 4.76 pH after addition of five drops of HCI - 4.69 pH of buffer in which (HA) = 0.10 5.66 K.- 2.188x106 pH after addition of excess NaOH 11.53 (2.188x10-6) (0.00) pH of distilled water 8.22 10.09) pH after...
Name 1) W Calculations ADVANCED STUDY ASSIGNMENT The pH of a solution is 5.000. Calculate the [H*) in the solution. [H'] = Phelos lond sales to [na saugoti 1017) A 1.000 x 10-M solution of sodium carbonate, Na,Co, has a pH of 11.05. A 1.000 x 10-1M solutie Calculate and answer the following: a) [H] b) [OH'] c) Is this solution acidic or basic? d) Write the net ionic equation for this reaction. e) Write the Ko expression for this...
Additional calculations and questions 1. Calculate the expected pH of buffer 1 after adding 1.50 mL of the 1.00 M NaOH K=1.8 x 10-5 for HCH.O2 2. Calculate the expected pH of buffer 1 after adding 3.00 mL of 1.00 NaOH 3. Write the net ionic equation for the reaction of OH with your buffer. 4. Does adding NaOH raise or lower the concentration of HC2H3O2? 5. Does adding NaOH raise or lower the concentration of NaC2H302? 6. Does adding...
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
Name Experiment 8 CONCLUSIONS For each part of the experiment, write the balanced molecular reaction (using the chart at the end of this experiment to identify precipitates and weak acids). Also write the total ionic reaction and net ionic reaction. No reaction occurred, simply write "NO REACTION" in the space for the molecular reaction. 1 molecular reaction NaCl(aq) + KNO3(aq) total ionic reaction net ionic reaction 2 molecular reaction NaCI(aq)+ AgNO3(aq) total ionic reaction net ionic reaction 3 molecular reaction...
4 stion n an experiment on hydrolysis, the pH values of 0.1M sodium acetate (CHhcoONa) and 0.1 chiorid recorded using pH paper of differentranges. Use these values to determine the correct pH then com Table Abelow DATA AND CALOULATONNS Table A MOH1 Paper Range Wide Range Paper Narrow Range Paper 0.1 MCHvcooNa 4 60 90 95 11 12 Calculations Part B Insert the net ionic equatioms, equilibriumconstant expressions, K. and Ka for the hydrolysable ions, in Table B. Show calculations...
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
Fill in the blanks and please show all work for Calculated Ka
or Kb column and explain how to find which ion is hydrolyzed
?
Part 1: pH of Solutions of Salts: In this part you will measure the pH values for 0.1 M solutions of the following solutes. Sodium bicarbonate o M Copper(II) sulfate oOM Iron(III) nitrate 010M Sodium acetate O-10M Ammonium chloride O Ib M Sodium fluoride o10 M Methylammonium chloride o.o M For each solution, place the...
Review of Measurement Uncertainty Calculations Here are the rules for propagating uncertainties through a calculation Addition: z m x + y δ,: 8x + 6y This works for any nunter of terms Subtraction:zx-y o&x + 5y This also works for any number of terns Multiplication by an exact value: z kx 82-kEx General multiplication/division: z-xy or z-:-a-Irl ) (This works for any number of factors) Exact power: z r-δε-121k] sine function: Z t, sin χ-82 tt lcos xlsr Cosine function...
Need help answering all questions. much
appreciated.
The Relative Strengths of Some Acids Results Solution pH from pH Paper pH from Indicators pH from pH Meter 2.8 14 1.99 1.4 1.4. HCL Ha POq HC2H30a Na HQ PO & AL (NO3)3 Zn(NO3)2 NH 4 NO3 1.7 1.7 4.63 2.4. 2.8 5.00 6.67 Questions 1. a. Calculate the concentration of H.O ions in the most acidic solution that you examined. Use your most precise pH measurement, 262 alculate the concentration of...
PART C. Properties of Buffers Buffer system selected_HCO -(0,2- Weak acid name _ NaC,H,O, pH of buffer 4.68 (H') = 2.09 XIOK 2.09x10 pH of diluted buffer 4.13 [H") = 1.8x10K - 1.8x10-5 pH after addition of five drops of NaOH 4.76 pH after addition of five drops of HCI - 4.69 pH of buffer in which (HA) = 0.10 5.66 K.- 2.188x106 pH after addition of excess NaOH 11.53 (2.188x10-6) (0.00) pH of distilled water 8.22 10.09) pH after...
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