Can i please get all questions answered
1. Add 20.0 mL of .120 M HNO3 to 20.0 mL of .120 M sodium benzoate. What is the pH?
KA of benzoic acid is 6.31 x 10-5
2. Which system would you use to construct a buffer with a pH of 6.50?
(you will need a KA table for this)
I C6H5OH / C6H5O- (phenol / phenolate)
II H2CO3 / HCO3- (carbonic acid / hydrogen carbonate)
III HC2H2O2Cl / C2H2O2Cl- (chloroacetic acid / chloroacetate)
IV H2PO4- / HPO42- (dihydrogen phosphate / hydrogen phosphate)
3. Titrate 26.0 mL .147 M H3C6H5O7 with .0664 M Mg(OH)2. How many mL of titrant are needed to completely neutralize the acid?
4. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH of the solution when 22.9 mL of titrant have been added?
5. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH exactly 2.00 mL beyond the equivalence point? hint: you will need the concentration of the titrant to do this
6. A sample of 15.0 mL of .100 M oxalic acid (H2C2O4) requires exactly 30.0 mL of NaOH to completely neutralize it. What is the pH of the solution if you only add 15.0 mL of NaOH instead?
7. The value of KW at 20oC is 1.00 x 10-14, but at 50oC it is 5.48 x 10-14. What is the pH of neutral water at 50oC?
Can i please get all questions answered
1. Add 20.0 mL of .120 M HNO3 to 20.0 mL of .120 M sodium benzoate. What is the pH?
KA of benzoic acid is 6.31 x 10-5
2. Which system would you use to construct a buffer with a pH of 6.50?
(you will need a KA table for this)
I C6H5OH / C6H5O- (phenol / phenolate)
II H2CO3 / HCO3- (carbonic acid / hydrogen carbonate)
III HC2H2O2Cl / C2H2O2Cl- (chloroacetic acid / chloroacetate)
IV H2PO4- / HPO42- (dihydrogen phosphate / hydrogen phosphate)
3. Titrate 26.0 mL .147 M H3C6H5O7 with .0664 M Mg(OH)2. How many mL of titrant are needed to completely neutralize the acid?
4. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH of the solution when 22.9 mL of titrant have been added?
5. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH exactly 2.00 mL beyond the equivalence point? hint: you will need the concentration of the titrant to do this
6. A sample of 15.0 mL of .100 M oxalic acid (H2C2O4) requires exactly 30.0 mL of NaOH to completely neutralize it. What is the pH of the solution if you only add 15.0 mL of NaOH instead?
7. The value of KW at 20oC is 1.00 x 10-14, but at 50oC it is 5.48 x 10-14. What is the pH of neutral water at 50oC?
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
