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1. Determine the Ka value for an acid that is 0.294 M in a solution that...

1. Determine the Ka value for an acid that is 0.294 M in a solution that has a pH of 2.80.

A 49 x 10-14

B. 23 x 109

C. 14 x 10-5

D. 20 x 10-5 OE 3.7x 10-7

2. When titrating 25.0 mL of 0.080 M HCIO with 0.060 M NaOH, calibrate the pH after adding 25.0 mL of 0.050 M NaOH (pKa = 7.55)

A. 7.43

b.7.55

C.7.77

D.10.08

E 1248

3. The correct expression for the equilibrium constant that applies to hydrolysis for the NaCH3C00 salt is:

A. K = (Na+] (CH3C00)

B. K =(H3O *) (CH3COO)/CH3COOH)

C. K = [CH3COOH)/ (H3O+) (CH3COO)

D. K = ((OH-] (CH3COO-)/(CH3COOH]

E. K = (OH-] (CH3COOH)/(CH3CO0-)

4. If in separate solutions of nitrates of Sn2+", Zn2+ and Ca2+* we put a coin of Ag (s) in each one it is expected that Ag (s)

Zn2+ * (ac) + 2e + Zn (s) E ° = - 0.76V

Sn2 +* (ac) + 2e → Sn (s) EO 0.14V

Ca2 +* (ac) + 20 + Cd (s) E ° -0.40V

Ag +* (ac) + e + Ag (s) E ° +0.80 V

A. React only with Zn2+ (ac)

B. React only with Sn+ * (ac)

C. React only with Ca2+ (ac)

D. Go Silver will react with all

E. the silver will not react with any.

5. According to the table shown, the best reducing agent is:

Average Reaction E (V)
Sn4+* (aq) + 2 e- Sn2+ * (aq) +0.15
Cr3+ * (aq) + 3 e- Cr(s) -0.74
Au3+ (aq) + 3 e- Au(s) +1.5

A. Au

B. Cr3 +

C. Au3+

D. Cr

E. Sn2 +

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