Homework Answers
pH of acidic buffer = pka + log(CH3COOH/CH3COONa)
pka of CH3COOH = 4.74
if [CH3COOH] = [CH3COONa] , buffer capacity will be maximum.so that,it will work effective at this conditions.
Hence, as the Concentration of CH3COOH,CH3COONa is same in both conditions the buffer capacity will be same in both conditions.
Answer: same in both conditions that is maximum.
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2. If you prepared a 0.15 M CH3CO2H - 0.15 M CH3CO,Na...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity t...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
2. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0 M HC red by diluting 0.25 mL of a 6.0 M HCl...
2. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0 M HC red by diluting 0.25 mL of a 6.0 M HCl with water to a total 1.25 ml. Record this pH in Part I data sheet, Beaker #1 for Theoretical Final pH. 3. Calculate the pH of a solution prepared by dilutine 0.25 mL of a 6.0 M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I...
3. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0M NaOH with water to a total volume of 20.25...
3. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I data sheet, Beaker #2 for Theoretical Final pH. 4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO2H and 10.0 mL of a 0.50 M CH,CO2Na. Record this pH in Part II data sheet, Beaker i#1 & #2 for Theoretical Initial...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHC...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHCO Na. Record this pH in Part II data sheet, Beaker #1 & N2 for Theoretical Initial pH. K for CHCOH = 1.8 x 10 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCL Record in Part Il data sheet, for Theoretical Final pH...
Calculate the pH of a bit a buller solution prepared by mixing 100 mlofa 10 M...
Calculate the pH of a bit a buller solution prepared by mixing 100 mlofa 10 M CH.CO.H and 100 mL of a 1.0 M CHCO Na. . Record this all in Part III data shss Beaker 1 & 2 for Thco Initial pH. K for CH,CO,H-1.8 x 109 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCI. Record in Part III data sheet, for Theoretical Final pH Beaker 1....
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of...
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
For the theoretical (theory/moles used), how do we get the "moles used" CALORIMETRY, Heat evolution from...
For the theoretical (theory/moles used), how do we get the
"moles used"
CALORIMETRY, Heat evolution from HCI+NaOH H+ ?? , H2O +AH (-70.3 kJ/mole) given value black-input, red CALC,blue-given + Volume HCI Density HCI mass HCI Molarity HCI 50.0 1.018 50.90 1.00 0.050 mL g/mL gramrs mole/L moles (mL 1000) L Volume NaOH 50.0 L Density NaOH 1.044 mass NaOH 52.20 1.50 (mL / 1000) m/L 0.075 moles of limiting reactant0.050 g/ml grams mole /L moles mole gramms Molarity NaOH...
Please help with the prelab questions! thank you!!!! Especially 2 and 3! Pre-Lab Questions 1. Calculate...
Please help with the prelab questions! thank you!!!!
Especially 2 and 3!
Pre-Lab Questions 1. Calculate the theoretical equivalence point (the volume!) in terms of ml NaOH adde each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2. Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa. What is the pH after...
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
2. If you prepared a 0.15 M CH.COH - 0.15 M CHCO Na buffer, would you expect the resulting buffer capacity to be higher, lower, or the same as the buffer you prepared in Part II of this lab? Be specific and use your data. c. Measure the pH of the Beaker #2 solution, via a pH meter, and record in data sheet. Part II: Dilute Buffer Solution In this section, the pH of a 0.25 M CH3CO2H - 0.25...
2. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0 M HC red by diluting 0.25 mL of a 6.0 M HCl with water to a total 1.25 ml. Record this pH in Part I data sheet, Beaker #1 for Theoretical Final pH. 3. Calculate the pH of a solution prepared by dilutine 0.25 mL of a 6.0 M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I...
3. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I data sheet, Beaker #2 for Theoretical Final pH. 4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO2H and 10.0 mL of a 0.50 M CH,CO2Na. Record this pH in Part II data sheet, Beaker i#1 & #2 for Theoretical Initial...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHCO Na. Record this pH in Part II data sheet, Beaker #1 & N2 for Theoretical Initial pH. K for CHCOH = 1.8 x 10 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCL Record in Part Il data sheet, for Theoretical Final pH...
Calculate the pH of a bit a buller solution prepared by mixing 100 mlofa 10 M CH.CO.H and 100 mL of a 1.0 M CHCO Na. . Record this all in Part III data shss Beaker 1 & 2 for Thco Initial pH. K for CH,CO,H-1.8 x 109 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCI. Record in Part III data sheet, for Theoretical Final pH Beaker 1....
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCI must be added to this buffer solution to change the pH by 0.40 units? Assume the total volume remains unchanged at 400 mL. For H2PO4, K = 6.3 x 10-8 0.013 mol 0.25 mol (Your answer) 0.50 mol 0.057 mol (Correct answer) 0.031 mol
For the theoretical (theory/moles used), how do we get the
"moles used"
CALORIMETRY, Heat evolution from HCI+NaOH H+ ?? , H2O +AH (-70.3 kJ/mole) given value black-input, red CALC,blue-given + Volume HCI Density HCI mass HCI Molarity HCI 50.0 1.018 50.90 1.00 0.050 mL g/mL gramrs mole/L moles (mL 1000) L Volume NaOH 50.0 L Density NaOH 1.044 mass NaOH 52.20 1.50 (mL / 1000) m/L 0.075 moles of limiting reactant0.050 g/ml grams mole /L moles mole gramms Molarity NaOH...
Please help with the prelab questions! thank you!!!!
Especially 2 and 3!
Pre-Lab Questions 1. Calculate the theoretical equivalence point (the volume!) in terms of ml NaOH adde each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2. Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa. What is the pH after...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
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