PLEASE explain part (c) clearly with detailed steps...I know the answer is 19 mL
Homework Answers
Note:
Volume in part C is different than you have suggested.
I have varified this volume using Henderson Hasselbalch equation.
You should also check my answer using this equation.
Add Answer to:
PLEASE explain part (c) clearly with detailed steps...I know the
answer is 19 mL
6. A...
A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa...
A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN = 9.20. a) What volume of 0.100 mol L-1 HCl will be required to fully react with the above salt? b) After the reaction in part a) takes places, will the pH of the solution be acidic, basic or neutral? c) What volume of 0.100 mol L-1 HCl is needed to adjust the pH of the originally provided solution to pH =...
These are all part of the same problem. please show steps for each question and explain....
These are all part of the same problem. please show steps for
each question and explain.
QUESTION 1 · 1 POINT *This is a part of the 6 part titration practice problem. The titration set up is as follows: 35.0 mL of 0.125 M HCN is titrated with 0.200 M KOH. The pka of HCN is 9.21. What is the pH once half of the equivalence volume has been added? Select the correct answer below: 11.34 9.21 O 7.00 10.22...
please answer every part part 1 part 2 A buffer solution contains 0.90 mol of hydrocyanic...
please answer every part
part 1
part 2
A buffer solution contains 0.90 mol of hydrocyanic acid (HCN) and 0.77 mol of sodium cyanide (NaCN) in 3.80 L. The K, of hydrocyanic acid (HCN) is k, = 4.9e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.31 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after...
*PLEASE provide the right answer with detailed steps and explanation and then I will give you...
*PLEASE provide the right answer with detailed steps and
explanation and then I will give you a thumbs up (if it's
right).
A 18.6 ml solution of 0.100 mol -- HOCI is titrated using 0.150 mol (NaOH. What is the pH of the solution after 5.89 mL of the NaOH solution is added? Express your answer to 2 decimal places. You have 5 attempts at this question. Remember you can find KA and/or Kg values in your textbook chapter 15.
Answer Part B please 1.000 mol of formic acid (HCOOH) and 0.500 mol of sodium formate...
Answer Part B please
1.000 mol of formic acid (HCOOH) and 0.500 mol of sodium formate (NaCOOH) are added to water and diluted to 1.00 L. Calculate the pH of the solution. Ka 1.77 x 10-4 (4 marks) Enough HCl is added to the above solution (with negligible volume change) to bring the [H3O] up to 0.100 M. Find the pH of the resulting solution. (5 marks)
A 1100 ml. buffer solution is 0.110 mol L-in NH, and 0.125 mol Lin NH Br....
A 1100 ml. buffer solution is 0.110 mol L-in NH, and 0.125 mol Lin NH Br. Review Constants Periodic Table What mass of HCI will the buffer neutralize before the pH falls below 9.007(K,(NH) - 1.76 x 10-5 Express your answer using two significant figures AERO me Submit Previous Answers Request Answer X Incorrect; Try Again Part B N H, and 0.390 mol L'in NH Br, what mass of HCl could If the same volume of the buffer were 0.265...
I already know the answer to part B, i just need help figuring out how to...
I already know the answer to part B, i just need help figuring out how to do part C, please show me the steps.(: Part B. What is the pH of the solution prepared by allowing 3.65 g of Na2O to react with 450.0 mL of water? Assume that there is no volume change answer :13.418 Part C,How many milliliters of 0.0100 M HCl are needed to neutralize the NaOH solution prepared in the part B?
Please check my answers to part a and b, an help me answer part c. I...
Please check my answers to part a and b, an help me
answer part c. I am not sure if I set it up correctly. Show work
please, thank you.
I LICN is asalt solution. The ka of HCN is 4,2 x 10 - a should the salt solution be auldic, basu, or neutral. o LiGN 7 Li + + CW - LIOH + HEN Basic SB WA b. Write the eauillibrium reaction for theion of the salt that contributes...
Please explain all steps ledgibly the highlighted part is the answer 11. A 500.0 mL buffer...
Please explain all steps ledgibly the highlighted part is the
answer
11. A 500.0 mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium benzoate (Ka 6.4 x 109) and has an initial pH of 4.19. What is the pH of the bu Fer upon addition of 0.010 mol of NaOH (assume no volume increase). (1) 1.70 (2) 4.01 (3) 4.28 4)7 (5) 4.51
i need help with questions for part b only please ZULU Acid-Base Titration (worksheet to be...
i need help with questions for part b only please
ZULU Acid-Base Titration (worksheet to be completed in pairs - dee via e-mail Thursday, April 2, 11:59 pm) Concentration of NaOH: 0.0993 mol/L Part A: The following data was obtained when a 20.00 mL sample of acetic acid was titrated with 0.0993 mol/L sodium hydroxide (NaOH). The indicator changed color when 18.90 mL of NAOH was added (highlighted below). pH pH Volume of Base (mL) 1.00 2.00 Volume of Base...
These are all part of the same problem. please show steps for
each question and explain.
QUESTION 1 · 1 POINT *This is a part of the 6 part titration practice problem. The titration set up is as follows: 35.0 mL of 0.125 M HCN is titrated with 0.200 M KOH. The pka of HCN is 9.21. What is the pH once half of the equivalence volume has been added? Select the correct answer below: 11.34 9.21 O 7.00 10.22...
please answer every part
part 1
part 2
A buffer solution contains 0.90 mol of hydrocyanic acid (HCN) and 0.77 mol of sodium cyanide (NaCN) in 3.80 L. The K, of hydrocyanic acid (HCN) is k, = 4.9e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.31 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after...
*PLEASE provide the right answer with detailed steps and
explanation and then I will give you a thumbs up (if it's
right).
A 18.6 ml solution of 0.100 mol -- HOCI is titrated using 0.150 mol (NaOH. What is the pH of the solution after 5.89 mL of the NaOH solution is added? Express your answer to 2 decimal places. You have 5 attempts at this question. Remember you can find KA and/or Kg values in your textbook chapter 15.
Answer Part B please
1.000 mol of formic acid (HCOOH) and 0.500 mol of sodium formate (NaCOOH) are added to water and diluted to 1.00 L. Calculate the pH of the solution. Ka 1.77 x 10-4 (4 marks) Enough HCl is added to the above solution (with negligible volume change) to bring the [H3O] up to 0.100 M. Find the pH of the resulting solution. (5 marks)
A 1100 ml. buffer solution is 0.110 mol L-in NH, and 0.125 mol Lin NH Br. Review Constants Periodic Table What mass of HCI will the buffer neutralize before the pH falls below 9.007(K,(NH) - 1.76 x 10-5 Express your answer using two significant figures AERO me Submit Previous Answers Request Answer X Incorrect; Try Again Part B N H, and 0.390 mol L'in NH Br, what mass of HCl could If the same volume of the buffer were 0.265...
Please check my answers to part a and b, an help me
answer part c. I am not sure if I set it up correctly. Show work
please, thank you.
I LICN is asalt solution. The ka of HCN is 4,2 x 10 - a should the salt solution be auldic, basu, or neutral. o LiGN 7 Li + + CW - LIOH + HEN Basic SB WA b. Write the eauillibrium reaction for theion of the salt that contributes...
Please explain all steps ledgibly the highlighted part is the
answer
11. A 500.0 mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium benzoate (Ka 6.4 x 109) and has an initial pH of 4.19. What is the pH of the bu Fer upon addition of 0.010 mol of NaOH (assume no volume increase). (1) 1.70 (2) 4.01 (3) 4.28 4)7 (5) 4.51
i need help with questions for part b only please
ZULU Acid-Base Titration (worksheet to be completed in pairs - dee via e-mail Thursday, April 2, 11:59 pm) Concentration of NaOH: 0.0993 mol/L Part A: The following data was obtained when a 20.00 mL sample of acetic acid was titrated with 0.0993 mol/L sodium hydroxide (NaOH). The indicator changed color when 18.90 mL of NAOH was added (highlighted below). pH pH Volume of Base (mL) 1.00 2.00 Volume of Base...
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