How would we find the net ionic equation for this?
![Part 1 Unknown # 10 Experimental [Hl pH 3.63 Theory pH Exp [H] Exp pH Part II HCI 0.10 M 0.010M Part III CH COOH 1.0 M 2.57](http://img.homeworklib.com/questions/9e2cbbe0-c2ea-11ec-8ab9-d79b1d5a4962.png?x-oss-process=image/resize,w_560)
For part 4, I mean.
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How would we find the net ionic equation for this?
For part 4, I mean.
Obtain...
based on instructions please help me fill out chart Use appropriate safety precautions for working with...
based on instructions please help me fill out chart
Use appropriate safety precautions for working with concentrated acids and bases. This includes splash-proof goggles, long pants, and closed-toe shoes. No eating, drinking, or chewing at any time in the laboratory. Part I: Comparing the Behavior of the Buffer with Distilled Water 1. Obtain a pH meter or probe. Make sure beakers are clean and dry. 2. Place 25 mL of distilled, deionized water in a clean dry 100-ml beaker. 3....
Prepare dilute acid and base solutions and buffered acid and base solutions to observe how buffering...
Prepare dilute acid and base solutions and buffered acid and base solutions to observe how buffering affects the pH. Use four clean, dry 50 ml beakers. Put these pH measurments in the Data Sheet Dilute NaOH Beaker 3 1. add 25 mL distilled H2O Buffered NaOH Beaker 4 1. add 25 mL of original buffer solution Dilute HCI Buffered HCI Beaker 1 Beaker 2 1. add 25 mL distilled 1. add 25 mL of H2O original buffer solution 2. Measure...
how would you calculate the expected pH for solution 7, 8, 9, 10, and 11? (I...
how
would you calculate the expected pH for solution 7, 8, 9, 10, and
11? (I am confused on how you calculate the dilutions for finding
the expected pH too)
Ka= 1.4x10^-5
pKa= 4.85
Part B - The Effect of Adding Acid or Base to a Buffered Solution Solution 6 16. Prepare a buffer solution by mixing 30.0 mL of 0.10 M HOAc and 40.0 mL of 0.10 M NaOAc. Measure the pH of the resulting solution with the pH...
I don't understand what calculations I would have made to create the buffer solution from Part...
I don't understand what calculations I would have made to create
the buffer solution from Part D of the lab. I understood the
procedures I took to create the solution but when the report asks
to show the calculations used to prepare the buffer solution I am
not sure other than mixing the volumes indicated in the procedures
section.
Thank you
pH of Butter Assigned by Instructor 5.12. Measured pH of Assigned B r .9 (Read the procedural Show the...
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH...
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O into a beaker. 1. Calculate the expected pH of pure water. pH ________ 2. Measured pH of pure water. pH ___3.88______ 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error __________ B. pH of Water and Strong Acid i. Measure out 30.0 mL DI H2O and 2.0...
i already know they answer please explain your solutions Ka for CH3COOH = 1.8x10^-5 pka i...
i already know they answer please explain your solutions
Ka
for CH3COOH = 1.8x10^-5
pka i calculated 4.74
ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...
thats all i'm given would it be the Ka1 which js 1.8x10^-5 pH and Buffers IV....
thats all i'm given
would it be the Ka1 which js 1.8x10^-5
pH and Buffers IV. pH of a Buffer Solution Mass of sodium acetate, CH,COONa, g 4.23g Calculated pH Measured pH buffer solution prepared with dissolved CH.COONa + 8.5 mL CH,COOH(aq) 13.84 40 ml buffer + 1.0 mL of 6.0 M HCl(aq) 1.30 40 ml. buffer + 1.0 mL of 6.0 M NaOH(aq) 5.90 Measured pH Calculated pH deionized water 5.78 1.55 40 mL DI water + 1.0 mL...
Oxalic addindate CH2OT-2H2 Fill out the table with the appropriate data from Part C, Trial 1...
Oxalic addindate CH2OT-2H2 Fill out the table with the appropriate data from Part C, Trial 1 Trial 2 439 Mass of Oxalic Acid Dihydrate (g) Moles of Oxalic Acid Dihydrate (Convert grams of oxalic acid to moles using the molecular weight of oxalic acid dihydrate) Moles of NaOH (Convert moles of Oxalic Acid Dihydrate to moles of NaOH using the mole ratio from the reaction) 25mL 41.6mL 41.35 mL Initial burette reading (mL) 2omL 32.00ML Final burette reading (mL) Volume...
1.How does adding NaOH to deionized water affect the pH differently than adding it to a...
1.How does adding NaOH to deionized water affect the pH differently
than adding it to a buffer?
2. how would you find the Ka of solution 4, after it is
diluted from solution 3? the measured pH was 4.98 which gave a [H+]
concentration of 1.05x10^-5.
Part A - Determining the Acid Ionization Constant for Acetic Acid Solution 1 6. Take a 30.0 mL sample of 10 M HOAc and place it in a beaker. Using a pH meter, measure...
based on instructions please help me fill out chart
Use appropriate safety precautions for working with concentrated acids and bases. This includes splash-proof goggles, long pants, and closed-toe shoes. No eating, drinking, or chewing at any time in the laboratory. Part I: Comparing the Behavior of the Buffer with Distilled Water 1. Obtain a pH meter or probe. Make sure beakers are clean and dry. 2. Place 25 mL of distilled, deionized water in a clean dry 100-ml beaker. 3....
Prepare dilute acid and base solutions and buffered acid and base solutions to observe how buffering affects the pH. Use four clean, dry 50 ml beakers. Put these pH measurments in the Data Sheet Dilute NaOH Beaker 3 1. add 25 mL distilled H2O Buffered NaOH Beaker 4 1. add 25 mL of original buffer solution Dilute HCI Buffered HCI Beaker 1 Beaker 2 1. add 25 mL distilled 1. add 25 mL of H2O original buffer solution 2. Measure...
how
would you calculate the expected pH for solution 7, 8, 9, 10, and
11? (I am confused on how you calculate the dilutions for finding
the expected pH too)
Ka= 1.4x10^-5
pKa= 4.85
Part B - The Effect of Adding Acid or Base to a Buffered Solution Solution 6 16. Prepare a buffer solution by mixing 30.0 mL of 0.10 M HOAc and 40.0 mL of 0.10 M NaOAc. Measure the pH of the resulting solution with the pH...
I don't understand what calculations I would have made to create
the buffer solution from Part D of the lab. I understood the
procedures I took to create the solution but when the report asks
to show the calculations used to prepare the buffer solution I am
not sure other than mixing the volumes indicated in the procedures
section.
Thank you
pH of Butter Assigned by Instructor 5.12. Measured pH of Assigned B r .9 (Read the procedural Show the...
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
i already know they answer please explain your solutions
Ka
for CH3COOH = 1.8x10^-5
pka i calculated 4.74
ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...
thats all i'm given
would it be the Ka1 which js 1.8x10^-5
pH and Buffers IV. pH of a Buffer Solution Mass of sodium acetate, CH,COONa, g 4.23g Calculated pH Measured pH buffer solution prepared with dissolved CH.COONa + 8.5 mL CH,COOH(aq) 13.84 40 ml buffer + 1.0 mL of 6.0 M HCl(aq) 1.30 40 ml. buffer + 1.0 mL of 6.0 M NaOH(aq) 5.90 Measured pH Calculated pH deionized water 5.78 1.55 40 mL DI water + 1.0 mL...
Oxalic addindate CH2OT-2H2 Fill out the table with the appropriate data from Part C, Trial 1 Trial 2 439 Mass of Oxalic Acid Dihydrate (g) Moles of Oxalic Acid Dihydrate (Convert grams of oxalic acid to moles using the molecular weight of oxalic acid dihydrate) Moles of NaOH (Convert moles of Oxalic Acid Dihydrate to moles of NaOH using the mole ratio from the reaction) 25mL 41.6mL 41.35 mL Initial burette reading (mL) 2omL 32.00ML Final burette reading (mL) Volume...
1.How does adding NaOH to deionized water affect the pH differently
than adding it to a buffer?
2. how would you find the Ka of solution 4, after it is
diluted from solution 3? the measured pH was 4.98 which gave a [H+]
concentration of 1.05x10^-5.
Part A - Determining the Acid Ionization Constant for Acetic Acid Solution 1 6. Take a 30.0 mL sample of 10 M HOAc and place it in a beaker. Using a pH meter, measure...
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