1. For the following chemicals and molarity find the GRAMS of chemical needed to make 500.0mL of solution at the given Molarity a. NaCl 3.5M b. NaI 0.75M c. C6H12O6 0.15M 2. What volume of each solution is needed to make 0.100mol of the product? a. Ag+ + Cl-  AgCl Solution A) 0.55M Ag+ Solution B) 0.75M Cl- b. Pb2+ + I-  PbI2 Solution C) 0.060M Pb2+ Solution D) 0.175M I- 3. What volume of solution gives the desired moles? a. 0.53mol from a 7.25M solution b. 0.035mol from a 1.25M solution c. 0.0013mol from a 0.090M solution 4. What pressure is needed to obtain the following volumes of gas? a. 12L of 3.0g CO2 at 22⁰C b. 720L of 35mol N2 at -15⁰C 5. Which of the following do NOT affect the rate of reaction? a. Concentration b. Gravity c. Surface Area d. Temp e. Day/Night time f. Energy of activiation g. Using English vs Metric units 6. A + B  C + D For the above reaction which direction does the equilibrium move after the following changes? a. Add more “A” b. Remove some “D” c. Add more “A” and “B” d. Remove “B” and add “C” 7. Find the pH for the following [H+] a. 1.3x10^-5 b. 1.7x10^-2 c. 9.8x10^-7 d. 2.4x10^-10 8. Find [H+] for the following mixture if Ka=1.8x10^-5 HX  H+ + X- [HX] = 0.10M [X-] = 0.10M **Hint, pH is 4.7447 to check your work** 9. Which is more acidic? a. pH = 3 or pH = 5 b. [H+] = 0.05 or [H+] = 0.03 10. If a weak acid/base mixture has 0.15M NH4+, Ka = 5.6x10^-10 and pH = 9.00 find the [NH3] present in solution