1. QUIZ ON CH. 14 AND 15

2. 1) What does pH measure? What are the terms for a liquid with a pH of 3, a pH of 7, and a pH 10? pH measures [H+] concentration in a solution 3= acid 10=base 7= neutral 2) An acid produces _hydronium___ ___ions___ when added to a solution A base produces __hydroxide____ __ions___ when added to a solution 3) What is a Brownstein-Lowry acid and base? a) Acids take in H+ while bases release OH- b) Acids release H+ while bases take release OH- c) Acids take in OH- while bases take in H+ d) Acids release H+ while bases take in H+

3. 4) What are the 4 types of acid-base reactions? Strong acid + strong base Weak acid+ strong base Strong acid + weak base Weak acid + weak base 5) Which of the following is a strong acid? a) HCl b) H 2 SO 4 c) HC 2 H 3 O 2 d) All of the above e) Some of the above 6) H 3 BO 3 is a…. a) Acidic anhydride b) Monoprotic acid c) Diprotic acid d) Triprotic acid

4. 7) Write the net ionic equation for the neutralization of H 2 SO 4 with NH 3. Is this solution basic, acidic, or neutral? H 2 SO 4 + 2NH 3  (NH 4 ) 2 SO 4 2H + + SO 4 2- + 2NH 3  2NH 4 + + SO 4 2- 2H + +2NH 3  2NH 4 + ; acidic 8) A basic anhydride is…. a) A metal oxide b) A nonmetal oxide c) An covalent oxide compound d) A conjugate acid 9) Between a 0.10 M solution of H 2 SO 4 and a 1.00 M solution of HF, which is more concentrated and which is stronger? a) H 2 SO 4 is stronger and HF is more concentrated b) H 2­ SO 4 is more concentrated and HF is more concentrated c) H 2 SO 4 and HF are both strong but H 2 SO 4 is less concentrated d) It is impossible to tell

5. 10) A 25 ml solution of 0.5 M NaOH is titrated until neutralized into a 50 ml sample of HCl. What was the concentration of the HCl? NaOH + HCl  NaCl + H 2 O V 1 M 1 =V 2 M 2  M 2 =V 1 M 1 /V 2  (25ml)(0.5M)/(50ml)= 0.25M= 0.3M 11) A solution has [OH - ] of 1.0 x 10 -9 M. a) Find [H + ]. [H + ]= 1.0x10 -5 b) Find the pH. pH= 14-9= 5 c) Find the pOH. pOH= -log(1.0x10 -9 )= 9 d) Is the solution ACID, BASE, or NEUTRAL? Acid 12) A solution has [H + ] = 1.0 x 10 -11 M. a) Find [OH - ]. [OH - ] = 1.0x10 -3 b) Find the pOH. pOH = 14-11= 3 c) Find the pH. pH= -log(1.0x10 -11 )= 11 d) Is the solution ACID, BASE, or NEUTRAL? Basic

6. 13) A solution has a pOH of 8. a) Find the pH. pH= 14-8= 6 b) Find [H + ]. [H + ] = 1.0 x10 -6 c) Find [OH - ]. [OH - ] = 1.0x10 -8 d) Is the solution ACID, BASE, or NEUTRAL? Acid 14) A solution has [H + ] = 1.0 x 10 -7 M. a) Find [OH - ]. [OH - ]= 1.0 x10 -7 b) Find the pOH. pOH= 14-7= 7 c) Find the pH. pH= -log(1.0x10 -7 )= 7 d) Is the solution ACID, BASE, or NEUTRAL? Neutral 15) What is the end point of a titration? Point at which the [H + ] = [OH - ].