Hi, Im a chem 122 student, I need help with the following problems. Thanks in advance

Worksheet 2 -CH 16 & 17 (10 points) 1. For the reaction: HNO2 (aq) + H20 (1) =H30 (aq) + NO, (aq), identify the Bronsted-Lowry Acid & Base pairs. Then write an expression for Ka for this reaction system. 2. For the reaction: HPO,?(aq) + H2O(0)=H2PO4 (aq) + OH (aq) Use figure 16.4 to predict if equilibrium lies to the left or to the right. If the pOH is 10.5 calculate the [OH-] and [H:0*] 3. The pH of a solution containing 0.063 M hypobromous acid is 4.95, calculate the Ka for HOBI 4. The Ka of HCN is 4.9 x 10-0. Calculate the pH and percent ionization of a 0.100 M HCN solution. 5. What is the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 104)? 6. Write a hydrolysis equation for the part of the salt that has a hydrolysis reaction (if any) with water and predict if the solution is acidic, neutral, or basic? KBro NHACI KCN K CO Rev: 10/6/2016 Worksheet 2 -CH 16 & 17 (10 points) 7. Calculate the pH of solution prepared by dissolving 0.10 mol of NH4Cl and 0.40 mol of NH3 in solution. The total volume of the solution is 0.500 L. Kb for NH3 is 1.8 x 10% 8. Calculate the pH of solution after the addition of 0.010 mol NaOH to 100L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10-5) What is the neutralization reaction that happens? Is the system still a buffer after neutralization? 9. Consider the titration of 50.0 mL of 0.100 M HOCI (Ka = 3.5 x 10) with 0.0400 M NaOH Calculate how many mL of base are required for the titration to reach the equivalence point. Calculate the pH at the equivalence point. 10. The Ksp for BaCO3 is 1.6 x 109. Write a chemical equation for the equilibrium of BaCO3(s) with its ions. When 20.0 mL of a 0.10 M Ba(NO3)2 is added to 50.0 mL of a 0.10 M Na2CO3 calculate the reaction quotient and determine if a precipitate will form? For the same reaction, predict the direction the system once it gets to equilibrium will shift when acid is added to the system Rev: 10/6/2016 Worksheet 2 -CH 16 & 17 (10 points) 1. For the reaction: HNO2 (aq) + H20 (1) =H30 (aq) + NO, (aq), identify the Bronsted-Lowry Acid & Base pairs. Then write an expression for Ka for this reaction system. 2. For the reaction: HPO,?(aq) + H2O(0)=H2PO4 (aq) + OH (aq) Use figure 16.4 to predict if equilibrium lies to the left or to the right. If the pOH is 10.5 calculate the [OH-] and [H:0*] 3. The pH of a solution containing 0.063 M hypobromous acid is 4.95, calculate the Ka for HOBI 4. The Ka of HCN is 4.9 x 10-0. Calculate the pH and percent ionization of a 0.100 M HCN solution. 5. What is the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 104)? 6. Write a hydrolysis equation for the part of the salt that has a hydrolysis reaction (if any) with water and predict if the solution is acidic, neutral, or basic? KBro NHACI KCN K CO Rev: 10/6/2016 Worksheet 2 -CH 16 & 17 (10 points) 7. Calculate the pH of solution prepared by dissolving 0.10 mol of NH4Cl and 0.40 mol of NH3 in solution. The total volume of the solution is 0.500 L. Kb for NH3 is 1.8 x 10% 8. Calculate the pH of solution after the addition of 0.010 mol NaOH to 100L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10-5) What is the neutralization reaction that happens? Is the system still a buffer after neutralization? 9. Consider the titration of 50.0 mL of 0.100 M HOCI (Ka = 3.5 x 10) with 0.0400 M NaOH Calculate how many mL of base are required for the titration to reach the equivalence point. Calculate the pH at the equivalence point. 10. The Ksp for BaCO3 is 1.6 x 109. Write a chemical equation for the equilibrium of BaCO3(s) with its ions. When 20.0 mL of a 0.10 M Ba(NO3)2 is added to 50.0 mL of a 0.10 M Na2CO3 calculate the reaction quotient and determine if a precipitate will form? For the same reaction, predict the direction the system once it gets to equilibrium will shift when acid is added to the system Rev: 10/6/2016