This is a pratice exam please show all steps/work. Points will be awarded I have
ID: 824314 • Letter: T
Question
This is a pratice exam please show all steps/work. Points will be awarded I have a 100% rating.
1) Arrange the following acids in terms of increasing acid strength
a) hypoiodous<periodic<iodic<iodous
b) periodic<hypoiodous<iodous<iodic
c) iodous<periodic<hypoiodous<iodic
d) hypoiodous<iodous<iodic<periodic
e) iodic<iodous<hypoiodous<periodic
2) Which of the following salts would, when dissolved in water, give a neutral pH?
a) (CH3)3NCl
b) NaOCl3
c) AlCl3
d) KC2H3O2
e) NaI
3. Which of the following would dissolve in water to make the most acidic solution?
a) nickel(II) bromide
b) aluminum iodide
c) magnesium iodide
d) ruthenium(II) perchlorate
e) lead(II) nitrate
4. Barium hydroxide is a strong base. What is the pH of 0.014M barium hydroxide solution?
a) 1.85
b) 1.55
c) 12.15
d) 12.45
e) 15.85
5. Which of the following is a weak acid?
a) HI
b) (CH3)3N
c) CH3NH3+
d) (C4H9)2NH
e) CH3CH2CH2NHCH3
6. Calculate the pH of a 0.50 M solution of lactic acid, a monoprotic acid
a) 0.30
b) 2.08
c) 3.77
d) 4.07
e) 9.49
7. What will be the properties of a 0.777 M solutionof the salt hydrazinium hydrazoate?
a) acidic
b) equivalent
c) neutral
d) chiral
e) basic
8. Referring to the attached table of dissociation constants, which of the following is the strongest base?
a) chloroacetate ion b) cyanate ion c) hydroxylamine
d) propanoate ion e) triethylamine
9. For 0.10 M oxalic acid (H2C2O4) (a diprotic acid), what is the concentration of the oxalate ([C2O42-]) ion? Ka,1 = 6.5 x 10-2, Ka,2 = 6.1 x 10-5
a) 0.054 M
b) 0.046 M
c) 6.1 x 10-5 M
d) 1.9 x 10-13 M
e) 1.0 x 10-14 M
10. What is the pH of a solution of 1.21M solution of ethanolamine?
a) 2.34
b) 5.71
c) 7.00
d) 10.97
e) 11.66
Part2
1. For the titration of 100.00 mL of 0.0150M hydrazoic acid (HN3; pKa=4.72) with 0.020 M KOH, calculate the pH of the solution after the addition of 20.00 mL of KOH(aq).
a) 2.79
b) 3.34
c) 4.28
d) 4.72
e) 5.16
2. For the titration of 100.00 mL of 0.015 M hydrazoic acid (pKa = 4.72) with 0.020 M KOH, calculate the pH of the solution after the addition of 37.50 mL of KOH(aq)
a) 2.79
b) 3.34
c) 4.28
d) 4.72
e) 5.16
3. For the titration of 100.00 mL of 0.0150M hydrazoic acid (pKa = 4.72), with 0.020 M KOH, calculate the pH of the solution after the addition of 75.00 mL of KOH(aq).
a) 5.16
b) 5.90
c) 7.00
d) 8.33
e) 9.36
4. One-tenth of a mole (0.1 mol) of the salt of a weak base is dissolved in 500 mL of water. If the pH of this solution is 5.50, what is the Kb of the base?
a) 5.0 x 10-11
b) 2.3 x 10-9
c) 4.4 x 10-6
d) 2.0 x 10-4
e) 1.1 x 10-2
5. For hydrazine (N2H4), pKb = 5.89. What is the pH of an aqueous buffer solution that is 0.336 M N2H4(aq) and 0.197 M N2H5Cl?
a) 9.34
b) 8.77
c) 8.34
d) 8.11
e) 6.12
6. If the value of the solubility product for La(IO3)3(s) is 6.1 x 10-12 at 25oC, calculate the solubility of La(IO3)3(s) in water.
a) 6.9 x 10-4
b) 5.7 x 10-6
c) 6.4 x 10-8
d) 9.5 x 10-11
e) 2.0 x 10-2
LOOK FOR PART ,3,4 UNDER SAME NAME FOR MORE POINTS. THANKS
Earn more points this a series of 3 other questions: (total off 7500 points)
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http://www.chegg.com/homework-help/questions-and-answers/please-show-work-steps-points-awarded-100-ratingthanks-part2-7-solution-0072m-mn-ii-cu-ii--q5042848
Explanation / Answer
1) Periodic, HIO4;
iodic, HIO3:
iodous, HIO2;
hypoiodous HIO
All these acids are monobasic containing an
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