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Typical Math Problems 1) What is the pH of a buffer solution which is 0.12M in...
4. Use the following formation rxn to answer the questions. 1/2 C12(g) + 3/2 F2(g) →...
4. Use the following formation rxn to answer the questions. 1/2 C12(g) + 3/2 F2(g) → CIF3(g) CIF3 can be prepared by the reaction represented by the equation above. For CIF; the standard enthalpy of formation, AH°, is -163.2 kilojoules/mole and the standard free energy of formation, AG°, is - 123.0 kilojoules/mole. a) Calculate the value of the equilibrium constant for the reaction at 298 K. b) Calculate the standard entropy change, AS°, for the above reaction at 298 K...
Absolute Entropy Sº, in moll K1 3. Use the following table and rxn to answer the questions. Standard Heat of Substan...
Absolute Entropy Sº, in moll K1 3. Use the following table and rxn to answer the questions. Standard Heat of Substance Formation, AH, in kJ moli C(s) 0.00 CO2(g) -393.5 H2(g) H2O(1) -285.85 O2(g) 0.00 C3H2COOH(1) 0.00 5.69 213.6 130.6 69.96 205.0 226.3 The enthalpy change for the combustion of butyric acid at 25°C, AH"comb, is-2,183.5 kilojoules per mole. C3H7COOH(1) + 5O2(g) = 4CO2(g) + 4H20(1) a) From the data above, calculate the standard heat of formation, AH,, for butyric...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH,...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Buffer Practice 1.) You wish to prepare 750 mL of a buffer solution of pH =...
Buffer Practice 1.) You wish to prepare 750 mL of a buffer solution of pH = 7.00 and you decide to use NaH2PO4 as the acid, K2 = 6.2 x 10. You have on hand a 0.175 M solution of this acid. Kai = 7.5 x 103, Ka2 = 6.2 x 10-8, K3 = 4.2 x 10-13 a.) Calculate the pH of the NaH2PO4 solution. b.) Calculate the grams of Na2HPO4 that need to be added to 750 mL of...
Problem 1. You are asked to prepare a pH = 10.7 buffer starting from 517 mL...
Problem 1. You are asked to prepare a pH = 10.7 buffer starting from 517 mL of water to which 18.78 of ammonia have been added. The buffer will be prepared by the addition of ammonium chloride. fammonia add to water is 1.90x105. 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 to water. (b) What is the pH of the initial ammonia solution?...
4. What molar ratio of HPO4 2-to H2PO4-in solution would produce a pH of 7.0? Phosphoric...
4. What molar ratio of HPO4 2-to H2PO4-in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotic acid, has 3 pKa values: 2.14, 6.86, and 12.4. Hint: Only one of the pKa values is relevant here. 5. For a weak acid with a pKaof 6.0, calculate the ratio of conjugate base to acid at a pH of 5.0. 6. Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa 3.8), acetic acid...
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic...
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.
1. What is the pH of a buffer solution prepared with a 0.4 M sodium citrate...
1. What is the pH of a buffer solution prepared with a 0.4 M sodium citrate and 1% citric acid (pka for citric acid - 3.13, MW - 192 g/mol)? 8. A buffer solution is prepared using 0.4 mole of a weakly basic drug (pka - 10.1) and an unknown quantity of its salt. The final solution has a pH of 8.99. How much of the salt was used? 9. A buffer solution with a desired pH of 8.15 needs...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
Question two A buffer solution is able to maintain a constant pH when small amounts of...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
4. Use the following formation rxn to answer the questions. 1/2 C12(g) + 3/2 F2(g) → CIF3(g) CIF3 can be prepared by the reaction represented by the equation above. For CIF; the standard enthalpy of formation, AH°, is -163.2 kilojoules/mole and the standard free energy of formation, AG°, is - 123.0 kilojoules/mole. a) Calculate the value of the equilibrium constant for the reaction at 298 K. b) Calculate the standard entropy change, AS°, for the above reaction at 298 K...
Absolute Entropy Sº, in moll K1 3. Use the following table and rxn to answer the questions. Standard Heat of Substance Formation, AH, in kJ moli C(s) 0.00 CO2(g) -393.5 H2(g) H2O(1) -285.85 O2(g) 0.00 C3H2COOH(1) 0.00 5.69 213.6 130.6 69.96 205.0 226.3 The enthalpy change for the combustion of butyric acid at 25°C, AH"comb, is-2,183.5 kilojoules per mole. C3H7COOH(1) + 5O2(g) = 4CO2(g) + 4H20(1) a) From the data above, calculate the standard heat of formation, AH,, for butyric...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Buffer Practice 1.) You wish to prepare 750 mL of a buffer solution of pH = 7.00 and you decide to use NaH2PO4 as the acid, K2 = 6.2 x 10. You have on hand a 0.175 M solution of this acid. Kai = 7.5 x 103, Ka2 = 6.2 x 10-8, K3 = 4.2 x 10-13 a.) Calculate the pH of the NaH2PO4 solution. b.) Calculate the grams of Na2HPO4 that need to be added to 750 mL of...
Problem 1. You are asked to prepare a pH = 10.7 buffer starting from 517 mL of water to which 18.78 of ammonia have been added. The buffer will be prepared by the addition of ammonium chloride. fammonia add to water is 1.90x105. 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 to water. (b) What is the pH of the initial ammonia solution?...
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.
1. What is the pH of a buffer solution prepared with a 0.4 M sodium citrate and 1% citric acid (pka for citric acid - 3.13, MW - 192 g/mol)? 8. A buffer solution is prepared using 0.4 mole of a weakly basic drug (pka - 10.1) and an unknown quantity of its salt. The final solution has a pH of 8.99. How much of the salt was used? 9. A buffer solution with a desired pH of 8.15 needs...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
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