show work please! (they are two different problems & that is
all im given/ asked for)
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show work please! (they are two different problems & that is
all im given/ asked for)...
1) enough of solution A (0.16 M HAc) is added to solution B (6.4x10^-3 M NaAc)...
1) enough of solution A (0.16 M HAc) is added to solution B (6.4x10^-3 M NaAc) to form a solution that is equimolar in HAc and Ac-. What volume of solution A must be added to 50mL of solution B to produce an equimolar solution? 2) You are asked to prepare 10.00 mL of buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A-). The target pH of the buffer solution is 5.25. Ka of...
Help Asap! 1. You are asked to prepare 10.00 mL of a buffer solution consisting of...
Help Asap!
1. You are asked to prepare 10.00 mL of a buffer solution consisting of 0.15 M weak acid (HA) and 0.15 M conjugate base (A™). The target pH of the buffer solution is 4.50. The K of HA is 8.2 x 10-5. What volume of A- is required to make the buffer? You must show your work to receive credit. (3 pts.) Cypka s logo 1. 1 1 . .1
You are asked to prepare 10.00 mL of a buffer solution consisting of 0.10 M weak...
You are asked to prepare 10.00 mL of a buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A-). The target pH of the buffer solution is 5.25. The Ka of HA is 5.0x10^-6. What volume of HA is required to make the buffer?
Determine how many mL of solution A(acetic acid-indicator solution) must be added to solution B (sodium...
Determine how many mL of solution A(acetic acid-indicator solution)
must be added to solution B (sodium acetate indicator solution) to
obtain a buffer solution that is equimolar in acetate and acetic
acid. You will need to refer to the Experimental Procedure,
partcularly the section on calculations, to answer this question.
Show all calculations.
of an indicator 2. Determine how many ml of solution A (acetic acid-indicator solution) must be added to solution B sodium acetate-indicator solution) to obtain a buffer...
A buffer solution is prepared by mixing the following solutions: SHOW WORK 50. mL of 2.0...
A buffer solution is prepared by mixing the following solutions: SHOW WORK 50. mL of 2.0 M weak acid (HA) solution and 50. mL of 2.0 M conjugate base solution (NaA) solution. The Ka for HA is 2.27 x 10-11. 41. What is the pH of the resulting solution after adding 100 ml of 1.0 M HCl to the original buffer solution? 11.12 b) 10.64 c) 12.32 d) 0.48 e) 5.32
Please show all work, thanks. A hydrocyanic acid buffer solution contains 0.84 M hydrocyanic acid (HCN)...
Please show all work, thanks.
A hydrocyanic acid buffer solution contains 0.84 M hydrocyanic acid (HCN) and 0.61 M of its conjugate base (CN). If a chemist adds 0.15 mol of nitric acid (HNO3), a strong acid, to 0.55 L of the buffer solution, what will be the final pH of the solution? (The pk of HCN is 9.21. Assume the volume of the added HNO3 is negligible.) 4.0
Showing work, please answer questions a and b, thank you! You are asked to prepare a...
Showing work, please answer questions a and b, thank
you!
You are asked to prepare a pH 8.60 buffer starting from 500 mL of 0.10 M solution of hydrocyanic acid, HCN, and excess sodium cyanide, NaCN. (Ka for HCN 4.9 x 10) 18. What is the pH of the hydrocyanic acid solution prior to adding NaCN? a) b) How many grams of NaCN should be added to prepare the buffer solution?
Extra Credit: The Titration of Na2CO3 with HCl (25 pts) (You must show work to earn...
Extra Credit: The Titration of Na2CO3 with HCl (25 pts) (You must show work to earn credit!) 1. A 0.1983 g sample of Na2CO3 was dissolved in 100.00 mL H20. That solution was titrated with 0.1531 M HCl as titrant. The pKai and pKaz of carbonic acid (the conjugate acid of the carbonate ion) are 6.351 and 10.329, respectively. (a) (2.5 pts) Write the equilibrium expressions for Kai and Kaz, using H2A, HA, and A2-for the chemical species. (b) (2.5...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa)...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
please show show work, very confused! will RATE Problem 1. You are asked to prepare a...
please show show work, very confused! will RATE
Problem 1. You are asked to prepare a pH = 10.0 buffer starting from 517 mL of water to which 21.8 g of ammonia have been added. The buffer will be prepared by the addition of ammonium chloride. The Kb of ammonia add to water is 1.99x105. Assume that the volume does not change on the addition of ammonia or ammonium chloride. (a) Write the balanced net ionic equation for ammonia added...
Help Asap!
1. You are asked to prepare 10.00 mL of a buffer solution consisting of 0.15 M weak acid (HA) and 0.15 M conjugate base (A™). The target pH of the buffer solution is 4.50. The K of HA is 8.2 x 10-5. What volume of A- is required to make the buffer? You must show your work to receive credit. (3 pts.) Cypka s logo 1. 1 1 . .1
Determine how many mL of solution A(acetic acid-indicator solution)
must be added to solution B (sodium acetate indicator solution) to
obtain a buffer solution that is equimolar in acetate and acetic
acid. You will need to refer to the Experimental Procedure,
partcularly the section on calculations, to answer this question.
Show all calculations.
of an indicator 2. Determine how many ml of solution A (acetic acid-indicator solution) must be added to solution B sodium acetate-indicator solution) to obtain a buffer...
Please show all work, thanks.
A hydrocyanic acid buffer solution contains 0.84 M hydrocyanic acid (HCN) and 0.61 M of its conjugate base (CN). If a chemist adds 0.15 mol of nitric acid (HNO3), a strong acid, to 0.55 L of the buffer solution, what will be the final pH of the solution? (The pk of HCN is 9.21. Assume the volume of the added HNO3 is negligible.) 4.0
Showing work, please answer questions a and b, thank
you!
You are asked to prepare a pH 8.60 buffer starting from 500 mL of 0.10 M solution of hydrocyanic acid, HCN, and excess sodium cyanide, NaCN. (Ka for HCN 4.9 x 10) 18. What is the pH of the hydrocyanic acid solution prior to adding NaCN? a) b) How many grams of NaCN should be added to prepare the buffer solution?
Extra Credit: The Titration of Na2CO3 with HCl (25 pts) (You must show work to earn credit!) 1. A 0.1983 g sample of Na2CO3 was dissolved in 100.00 mL H20. That solution was titrated with 0.1531 M HCl as titrant. The pKai and pKaz of carbonic acid (the conjugate acid of the carbonate ion) are 6.351 and 10.329, respectively. (a) (2.5 pts) Write the equilibrium expressions for Kai and Kaz, using H2A, HA, and A2-for the chemical species. (b) (2.5...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
please show show work, very confused! will RATE
Problem 1. You are asked to prepare a pH = 10.0 buffer starting from 517 mL of water to which 21.8 g of ammonia have been added. The buffer will be prepared by the addition of ammonium chloride. The Kb of ammonia add to water is 1.99x105. Assume that the volume does not change on the addition of ammonia or ammonium chloride. (a) Write the balanced net ionic equation for ammonia added...
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