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9. Convert 31.6 MBq to GBq.
10. The half-life of Nitrogen 13 is 10 minutes. A sample of Nitrogen 13 has an activity of 20uCi. How long will it take for the activity of this sample to decrease to 2uCi?
11. Provide the correct term for each of the following descriptions.
a) The chemical formula of an ion produced upon the self-ionization of water. ____________.
b) The chemical formula of the ion present in greater concentration in an acidic solution. ___________.
c) An example of a chemical formula of a compound that produces hydroxide ions in solution is _______________.
d) An example of a monoprotic acid is ______________.
12. Which of the following compounds is a base?
a) NH3 c) H2SO4 b) CH3COOH d) HBr
13. If a solution contains a concentration of H3O + that equals 10-1M, what will be the concentration of OH - in this solution? Will this solution be acidic or basic? Describe its strength.
14. Given the pH of the following solutions, write the solutions in order of the increasing concentrations of hydronium ions.
Solution A pH = 11; Solution B pH = 3; Solution C pH = 6.
15. Calculate the pH of a solution that has a concentration of hydroxide ions equal to 0.00025M? Is this solution acidic, basic or neutral?
16. Complete the following acid base reaction and then answer the questions below. H3PO4 + H2O --------------->
<---------------
a) Which of the above reactants is amphiprotic? __________
b) Which of the above reactants becomes a base? _________
c) True or False. A proton is being donated from H3PO4 to water. ________
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Half life is the time it takes for a sample to reduce its amount to half.
Step-by-step explanation
9. Convert 31.6 MBq to GBq.
?31.6MBq1MBq106Bq?109Bq1GBq?=0.0316GBq?
10. The half-life of Nitrogen 13 is 10 minutes. A sample of Nitrogen 13 has an activity of 20uCi. How long will it take for the activity of this sample to decrease to 2uCi?
11. Provide the correct term for each of the following descriptions.
a) The chemical formula of an ion produced upon the self-ionization of water. OH- or H+/H3O+.
b) The chemical formula of the ion present in greater concentration in an acidic solution. H+ or H3O+.
c) An example of a chemical formula of a compound that produces hydroxide ions in solution is NaOH.
d) An example of a monoprotic acid is HCl.
12. Which of the following compounds is a base?
a) NH3 c) H2SO4 b) CH3COOH d) HBr
13. If a solution contains a concentration of H3O + that equals 10-1M, what will be the concentration of OH - in this solution? Will this solution be acidic or basic? Describe its strength.
?pH=−log(10−1M)=1?
?pOH=14−pH=14−1=13?
?[OH−]=10−pOH=10−13=1x10−13M?
Since the [H3O+] is 1012 times greater than the [OH-] and pH is less than 7, this solution is acidic.
14. Given the pH of the following solutions, write the solutions in order of the increasing concentrations of hydronium ions.
Solution A pH = 11; Solution B pH = 3; Solution C pH = 6.
Increasing pH means decreasing amount of hydronium ions.
Solution A < Solution C < Solution B
15. Calculate the pH of a solution that has a concentration of hydroxide ions equal to 0.00025M? Is this solution acidic, basic or neutral?
16. Complete the following acid base reaction and then answer the questions below.
H3PO4 + H2O ??? H2PO4- + H3O+
a) Which of the above reactants is amphiprotic? H2PO4-
b) Which of the above reactants becomes a base? H2PO4-
c) True or False. A proton is being donated from H3PO4 to water. True
