Chemistry 12

9. According to Arrhenius, which of the following groups contain:
i)only acids ii)only bases
a. NaOH, H2CO3, KCl
b. MgCl2, H2SO4, HCl
c. HNO3, HCl, H3PO4
d. Mg(OH)2, AgBr, HF
e. KOH, NH4OH, Ba(OH)2

10. Enough water is added to 100 g of sodium hydroxide in order to obtain a one litre solution. What is the concentration of OH- ions in this solution?

11. Consider the following reaction:
CO32-(aq) + H2O(l) ↔ HCO3-(aq) + OH-(aq)
a. Identify the acid and base on the left side of the equation?
b. What is the base on the right side that is paired with the corresponding acid from the left side of the equation?

12. What is the function of water in the following reaction?
CH3COOH + H2O ↔ H3O+ + CH3COO-
In other words, is the water an acid or a base?

13. Calculate the [H+] and [OH-] for a solution containing 100 mL of 0.05 M HNO3.

14. A solution of acetic acid 12 M is a:
a. concentrated, strong acid
b. dilute, strong acid
c. concentrated, weak acid
d. dilute, weak acid

15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is:
a. 2 x 10-14 M
b. 5 x 10-14 M
c. 5 x 10-7 M
d. 2 x 10-1 M

16. Aqueous solutions of strong acids and strong bases:
a. are good electricity conductors
b. make litmus paper become red
c. have a pH of 7.0
d. react with copper to form hydrogen gas

17. Which of the following can be considered as a Brönsted-Lowry base?
a. Na+
b. HCl
c. CH3COOH
d. Cl-

18. What happens when NH3 bubbles in water?
a. NH3 acts as a base
b. NH3 acts as an acid
c. NH3 does not dissolve in water
d. there is no reaction

19. An aqueous solution of NH3 is:
a. an acidic solution
b. a basic solution
c. a neutral solution
d. an indicator solution
20.
a. What is the pH of a solution of 0.05 M HNO3?
b. What does the pH become if 200 mL of this acid is diluted to 1.0 L?

21. Classify the following solutions in order of increasing pH:
a. 0.01 M NaOH
b. pure water
c. 0.10 M HCl
d. 0.05 M NaOH
e. 0.001 M HCl

22. What is the concentration of H+ in the solutions of pH:
a. 1.4
b. 4.8
c. 13.6

23. What is the pH of a solution which [H+] is:
a. a)4.0 x 10-5 M
b. b)2.5 x 10-6 M

24.
a. How many moles of NaOH must be dissolved in 1.0 L of water in order to get a pH of 12.4?
b. What mass of NaOH does this represent?

25. What is the pH of a solution of 0.1 M silver hydroxide, which is only 10% ionized?

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  1. do your own homework.

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  2. Haha you actually posted your homework... smh

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