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14. Using the systematic approach, determine the a, b, and c variables needed for the quadratic...
c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml...
c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml of this buffer. For full creds, show your work in detail. (4) aj Calculate the pH if 9.5 mL of 10.0 M NaOH (ag) is added to 200.0 mL ofa freshly prepared solution of this buffer. For full credit, show your work in detail (4) e) You should see from the calculations that this buffer is better able to buffer against added acid than...
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...
Please I need help with F AND G Extra Credit: The Titration of Na2CO3 with HCl...
Please I need help with F AND G
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,...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0 mL of a CH3COOH (acetic acid)/ CH3COONa * 3H2O buffer. The target pH of the buffer is 5.25. The given concentration of [CH3COOH] is equal to 0.10 M. Ka = 1.80 x 10-5 for acetic acid. Use the Henderson-Hasselbalch equation to determine the ratio of [CH3COO-]/[CH3COOH] needed to make the buffer. pH = pKa + log([CH3COO-]/[CH3COOH]) Now calculate the concentration of acetate ion (CH3COO-...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0 mL of a CH3COOH (acetic acid)/ CH3COONa * 3H2O buffer. The target pH of the buffer is 5.25. The given concentration of [CH3COOH] is equal to 0.10 M. Ka = 1.80 x 10-5 for acetic acid. PLEASE EXPLAIN :( Q1:Given the Ka value in the instructions (1.80 x 10-5). Calculate the pKa Q2:Use the Henderson-Hasselbalch equation to determine the ratio of [CH3COO-]/[CH3COOH] needed to...
1) What is the pH when 5.00 mL of 0.200 M NaOH has been added to...
1) What is the pH when 5.00 mL of 0.200 M NaOH has been added to 50.00 mL of 0.100 M CH3CO2? Strategy Step 1: Use stoichiometry of the neutralization to determine the amounts of acid and conjugate base present in solution Step 2: Solve for equilibrium concentrations using ICE tables or Henderson-Hasselbalch approximation 2) Calculate the molar solubility of silver chromate in pure water. Ksp = 1.12 x 10¯12 3) Calculate Kb for the acetate ion from the Ka...
Part 4: Calculating pH values as a Titration Progresses - this is a tough question! Finally, consider a 20.00...
Part 4: Calculating pH values as a Titration Progresses - this is a tough question! Finally, consider a 20.00 mL aqueous solution of 0.20 M H2A, where "H2A" is some arbitrary diprotic acid (Ka1 = 4.35 x 10-7, Kaz = 4.85 x 10-11 Estimate the pH values of the solution after the addition of 0.00, 10.00, 20.00, 30.00, 40.00, and 60.00 mL of 0.20 M NaOH. d) Calculation M4 - 30.00 ml NaOH Added: Here we realize that 20 ml...
Succinic acid (H2C4H6O4), which we will denote H2Suc, is a biologically relevant diprotic acid with the...
Succinic acid (H2C4H6O4), which we will denote H2Suc, is a biologically relevant diprotic acid with the structure shown below он он о нн Q Tap image to zoom . It is closely related to tartaric acid and malic acid. At 25°C the acid-dissociation constants for succinic acid are Kai-6.9 10-5 and Ka2-2.5 x 10-6 Part A Determine the pH of a 0.37 M solution of H2Suc at 25 C, assuming that only the first dissociation is relevant. Express your answer...
I can't figure out how to find the concentration of the conjugate base. Question 2 If...
I
can't figure out how to find the concentration of the conjugate
base.
Question 2 If a 50.00 mL sample of 0.132 M ammonium chloride is titrated with 21.47 mL of 0.149 M NaOH, what is the pH of the titration mixture? (For NH4CI, Ka = 5.75 x 10-10, Selected Answer: 2 Correct Answer: 9.21 +0.02 Response This is in the buffered region of the titration. Therefore, calculate the moles of weak acid initially present and the Feedback: moles of...
A buffer solution having a total volume of 0.50 L is prepared which has the following...
A buffer solution having a total volume of 0.50 L is prepared which has the following composition: [NH4Cl] = 0.25 M, [NH3] = 0.40 M. [Note: Kb of NH3 = 1.8 × 10−5 ] (a) Identify the species that acts as the acid and base in this buffer. (b) What role does the chlorine anion play? (c) Calculate the pH of this buffer solution using the Henderson-Hasselbalch equation. Is there any underlying assumption being made when you use this equation?...
c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml of this buffer. For full creds, show your work in detail. (4) aj Calculate the pH if 9.5 mL of 10.0 M NaOH (ag) is added to 200.0 mL ofa freshly prepared solution of this buffer. For full credit, show your work in detail (4) e) You should see from the calculations that this buffer is better able to buffer against added acid than...
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...
Please I need help with F AND G
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,...
Part 4: Calculating pH values as a Titration Progresses - this is a tough question! Finally, consider a 20.00 mL aqueous solution of 0.20 M H2A, where "H2A" is some arbitrary diprotic acid (Ka1 = 4.35 x 10-7, Kaz = 4.85 x 10-11 Estimate the pH values of the solution after the addition of 0.00, 10.00, 20.00, 30.00, 40.00, and 60.00 mL of 0.20 M NaOH. d) Calculation M4 - 30.00 ml NaOH Added: Here we realize that 20 ml...
Succinic acid (H2C4H6O4), which we will denote H2Suc, is a biologically relevant diprotic acid with the structure shown below он он о нн Q Tap image to zoom . It is closely related to tartaric acid and malic acid. At 25°C the acid-dissociation constants for succinic acid are Kai-6.9 10-5 and Ka2-2.5 x 10-6 Part A Determine the pH of a 0.37 M solution of H2Suc at 25 C, assuming that only the first dissociation is relevant. Express your answer...
I
can't figure out how to find the concentration of the conjugate
base.
Question 2 If a 50.00 mL sample of 0.132 M ammonium chloride is titrated with 21.47 mL of 0.149 M NaOH, what is the pH of the titration mixture? (For NH4CI, Ka = 5.75 x 10-10, Selected Answer: 2 Correct Answer: 9.21 +0.02 Response This is in the buffered region of the titration. Therefore, calculate the moles of weak acid initially present and the Feedback: moles of...
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