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8. Answer the following questions based on the equilibrium reaction shown...
Please answer these questions. Thank you so much. 9. Consider the buffer system between the weak...
Please answer these questions. Thank you so much.
9. Consider the buffer system between the weak acid NaH;PO, and Na2HPO4 to answer the following questions. a. Which of the parts of the buffer system would neutralize added acid? Write out the reaction between that part of the buffer and H.O. b. Which of the parts of the buffer system would neutralize added base? Write the reaction between that part of the buffer and OH.
consider the buffer system between the weak acid NaH2PO4 and Na2HPO4 Which of the parts of...
consider the buffer system between the weak acid NaH2PO4 and Na2HPO4 Which of the parts of the buffer system would neutralize added acid? Write out the reaction between that part of the buffer and H30+. Which of the parts of the buffer system would neutralize added base? Write the reaction between that part of the buffer and 0H-
6. Answer the following questions regarding the equilibrium for the reaction below 2 AsH3(g) = 2...
6. Answer the following questions regarding the equilibrium for the reaction below 2 AsH3(g) = 2 As (s) + 3 H2 (9) a. If AsH3 was removed from the equilibrium mixture, what would happen to the equilibrium concentration of H2? (increase, decrease, no change) b. If additional As is added to the reaction, what would happen to the equilibrium concentration of AsH3? (increase, decrease, no change) c. If the value of K decreases as the temperature of the system is...
Write your answer to each of the following questions, on the blanks at the left. C....
Write your answer to each of the following questions, on the blanks at the left. C. Consider HN_O2 Its conjugate base is _____ HNO_2 is a _____ acid (strong or weak). In the reaction between HNO_2 and HCN: HNO_2(aq) + CN^-(aq) HCN(aq) + NO^-_2(aq) K = 1 times 10^6. The predominant species after the reaction reaches equilibrium are _____. (Write both species.) When HNO_2 is titrated with NaOH to the equivalence point, the pH of the resulting solution is _____...
CHEM 2A Class Pack FIB 8. Consider the equilibrium system: HCN (aq) + H20 (1) H,O*...
CHEM 2A Class Pack FIB 8. Consider the equilibrium system: HCN (aq) + H20 (1) H,O* (aq) + CN' (a) a) write an equilibrium expression for this reaction b) Predict the direction the position of equilibrium will shift as a result of the following disturbances, 1. (HCN) increases ii. KCN is added iii. KCl is added iv. pH decreases V. KOH is added 9. Consider the equilibrium system: C(s) + CO2(g) + heat 2 CO (9) 1. write an equilibrium...
6. Use the equilibrium below to answer the following questions: 2H2O+CO2 (e) H2COac)H2O If the system...
6. Use the equilibrium below to answer the following questions: 2H2O+CO2 (e) H2COac)H2O If the system is at equilibrium and then more CO2 was added, how would the system react and why? (Shift to products, shift to reactants, no change) a. If the system is at equilibrium and then CO2 was removed what would happen to the concentration of H2CO3 and why? b.
Can you please answer the part i underlined? Thanks!! Point A,b,c is not given details about...
Can
you please answer the part i underlined? Thanks!!
Point A,b,c is not given details about the points are given so
you have to guess and find it thats the part I was having a hard
time with
Computer-Simulated Titration Curve 12.00 + 0.00 10.00 0.00 12.00 2.00 8.00 4.00 6.00 Drops of Added 0.01 M NaOH Figure 14.10 1 drop of 0.04 M H,PO, with 0.01 M NaOH. H3PO4(aq) + NaOH(aq) + NaH PO,(aq) + H2O(1) Referring to Figure...
QUESTIONS 2C if more A is added; if more B is added; if 1. How is...
QUESTIONS 2C if more A is added; if more B is added; if 1. How is the equilibrium shifted in A+B some of C is removed from the reaction? 2. State Le Chatelier's Principle in clear terms. 3. When a system is at equilibrium, are any chemical reactions going on? NH + OH what would happen if 4. In the equilibrium reaction NH +H,O more ammonium salt were added? If HCI were added? forms under acid conditions, how would you...
is a solution that resists changes in pH when a small amount of acid or base...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
1. Write the balanced chemical equation for the reaction of HF with water. Type your answer...
1. Write the balanced chemical equation for the reaction of HF with water. Type your answer here. 2. What is the pH and concentration of F– in a 0.100M solution of HF? Ans. pH = 2.10 Insert your work image here. 3. Write the balanced chemical equation for the dissolution of NaF in water. Type your answer here. 4. What would happen if the equilibrium [F–] that you calculated in 2 was changed by adding 0.00500 moles of solid NaF to...
Please answer these questions. Thank you so much.
9. Consider the buffer system between the weak acid NaH;PO, and Na2HPO4 to answer the following questions. a. Which of the parts of the buffer system would neutralize added acid? Write out the reaction between that part of the buffer and H.O. b. Which of the parts of the buffer system would neutralize added base? Write the reaction between that part of the buffer and OH.
6. Answer the following questions regarding the equilibrium for the reaction below 2 AsH3(g) = 2 As (s) + 3 H2 (9) a. If AsH3 was removed from the equilibrium mixture, what would happen to the equilibrium concentration of H2? (increase, decrease, no change) b. If additional As is added to the reaction, what would happen to the equilibrium concentration of AsH3? (increase, decrease, no change) c. If the value of K decreases as the temperature of the system is...
Write your answer to each of the following questions, on the blanks at the left. C. Consider HN_O2 Its conjugate base is _____ HNO_2 is a _____ acid (strong or weak). In the reaction between HNO_2 and HCN: HNO_2(aq) + CN^-(aq) HCN(aq) + NO^-_2(aq) K = 1 times 10^6. The predominant species after the reaction reaches equilibrium are _____. (Write both species.) When HNO_2 is titrated with NaOH to the equivalence point, the pH of the resulting solution is _____...
CHEM 2A Class Pack FIB 8. Consider the equilibrium system: HCN (aq) + H20 (1) H,O* (aq) + CN' (a) a) write an equilibrium expression for this reaction b) Predict the direction the position of equilibrium will shift as a result of the following disturbances, 1. (HCN) increases ii. KCN is added iii. KCl is added iv. pH decreases V. KOH is added 9. Consider the equilibrium system: C(s) + CO2(g) + heat 2 CO (9) 1. write an equilibrium...
6. Use the equilibrium below to answer the following questions: 2H2O+CO2 (e) H2COac)H2O If the system is at equilibrium and then more CO2 was added, how would the system react and why? (Shift to products, shift to reactants, no change) a. If the system is at equilibrium and then CO2 was removed what would happen to the concentration of H2CO3 and why? b.
Can
you please answer the part i underlined? Thanks!!
Point A,b,c is not given details about the points are given so
you have to guess and find it thats the part I was having a hard
time with
Computer-Simulated Titration Curve 12.00 + 0.00 10.00 0.00 12.00 2.00 8.00 4.00 6.00 Drops of Added 0.01 M NaOH Figure 14.10 1 drop of 0.04 M H,PO, with 0.01 M NaOH. H3PO4(aq) + NaOH(aq) + NaH PO,(aq) + H2O(1) Referring to Figure...
QUESTIONS 2C if more A is added; if more B is added; if 1. How is the equilibrium shifted in A+B some of C is removed from the reaction? 2. State Le Chatelier's Principle in clear terms. 3. When a system is at equilibrium, are any chemical reactions going on? NH + OH what would happen if 4. In the equilibrium reaction NH +H,O more ammonium salt were added? If HCI were added? forms under acid conditions, how would you...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
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