14. A 10.0-g sample of solid NH4Cl is heated in a 5.00-L container to 900.°C. At equilibrium the pressure of NH3(g) is 1.56 atm.<===>The equilibrium constant, Kp, for the reaction is: A) 1.56B) 2.43C) 3.12D) 8.76E) none of thesePage 4
15. You have 100.0 mL of a solution of hydrochloric acid that has a pH of 3.00. You add 100.0 mL of water to this solution. What is the resulting pH of the solution? 16. Determine the molarity of a solution of the weak acid HClO2(Ka= 1.10 10-2) if it has a pH of 1.226. 17. As water is heated, its pH decreases. This means that 18. A 75.0-mL sample of 0.0500 M HCN (Ka= 6.2 ×10-10) is titrated with 0.500 M NaOH. What volume of 0.500 M NaOH is required to reach the stoichiometric point? A) 75.0 mLB) 7.50 mLC) 750. mLD) cannot determine without knowing the pH at the stoichiometric pointE) none of these19. Which of the following will not produce a buffered solution? Page 5
Use the following to answer question 20.You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.050 M HOAc and 0.050 M NaOAc. 20. How do the pHs of the buffered solutions compare?
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