I need help with problems from a practice exam involving acids and bases
QUESTION 1
Complete the following equation: (CH3)3N + H2O -->
(CH3)3NH+ + –OH |
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(CH3)3NH+ + H3O+ |
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(CH2)3N + H3O+ |
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H(CH3)3N + –OH |
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No reaction |
1 points
QUESTION 2
The pH of a 0.500 M solution of an unknown acid (HA) is 6.45 at 25 ⁰C. Determine the value of the equilibrium constant for this acid at 25 ⁰C.
3.55 x 10–7 |
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2.82 x 10–8 |
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2.52 x 10–13 |
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1.59 x 10–15 |
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None of the above |
1 points
QUESTION 3
What is the pH of 0.20 M C6H5COOH? (Ka[C6H5COOH = 6.46 x 10–5])
0.70 |
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2.44 |
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4.60 |
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11.56 |
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13.30 |
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None of the above |
1 points
QUESTION 4
What is the pH of a 0.350 M solution of triethylamine [(CH3CH2)3N]? [Kb = 5.2 X 10─4]. Assume that you can neglect x.
0.46 |
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1.87 |
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10.26 |
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12.13 |
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None of the above |
1 points
QUESTION 5
When calculating pH for 0.10 M CH3COOH, which of the following is true?
[CH3COOH]init = [H3O+]equil |
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[CH3COOH]init ≠ [H3O+]equil |
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The –log of 0.10 M is pOH, since CH3COOH is not a strong acid. |
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A Ka value is required. |
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Both b and d. |
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Both b and c. |
ques 5. Both b and c is
correct option.weak acid doesnot disscociate compeletly
I need help with problems from a practice exam involving acids and bases QUESTION 1 Complete...
Titration Curves of Pre-lab questions. rves of Strong and Weak Acids and Bases. e 1. Explain the difference between a stre xplain the difference between a strong acid and a weak acid. **Calculate the pH of an HC Solution in which the H.01 -1.75 x 10°M. Calculate the pH of a NAOH solution in which the (OH) 3.7 x 10" M. Labc 4. Calculate the [H.O') when pH = 7.42 5. Calculate the [H3O+] when pOH = 5.43 6. Calculate...
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anyone help?
Question 6 (5 points) Which of the following will increase when HF is added to pure water at 25 °C? Okw Орн O(OH) Осно*) Ka Question 7 (5 points) aculate the Kb of the conjugate base of an acid with a ka value of 2.9 X 100 25 °C Question 7 (5 points) Calculate the Kb of the conjugate base of an acid with a Ka value of 2.9 x 10-10 at 25 °C. O 3.4 x...
Review of acids/bases and acid-base neutralization: 1. What species is the conjugate acid of HCO? 2. Which species is the conjugate base of HPO 2-? Refresher of Acid/Base Equilibria, Ka, and pK., and buffer solutions: 1. The (H30') in a cabernet Sauvignon wine is 5.9 x 10 M. What is the (-OH) in this wine? 2. The pH of a lime is 1.90. What is the [H30*]? 3. What is the pH of a cleaning solution with a [H3O+] =...
i
need help with these questions please.
Which acid is the strongest? Multiple Choice Hydrogen sulfate ion HS04– (Ka = 1.2 x 10-2 Hydrocyanic acid HCN (KA = 4.9 x 10-10, Hydrofluoric acid HF (Ka = 7.2 x 10-4) Ammonium ion NH4+ (ka =5.6 10-10) Which solution has the highest pH? Multiple Choice 12., 18- o 4.3 x 108 мон o 10 х 10-7м-он o 51 х 10-2м Но* o 19 х 10-8м-он o 10 х 10-2М Н30* Saved The...
Acids and Bases 1) Which of the following is a general property of a basic solution? a. feels slippery b pH less than 7 c. tastes sour d. turns litmus paper red e. none of the above 2) If a vinegar sample has a pH of 5, the solution is which of the following: a. strongly acidic b. weakly acidic c neutral d. weakly basic e. strongly basic 3) Which of the following is a weak Arrhenius acid a. HNO3...
i
need help solving for y. how did we get 2.4 x 10 ^-8 M
here is all the information i need help on how we solved for y
= [C2O4^2-]. dont know what to do with 6.4 x 10 ^ -5 = (y)(0.0528 +
y) / 0.0528 - y
i need a step by step explanation please
Reaction [H2CO3] Initia [HCO3) 4.58 x 10-3 -y 0.00458 - y TOH-1 0.00458 +y Change + y Equilibrium 0.00458 + y •...
17. From the following equilibrium process involving a weak acid (K2), derive the Henderson Hausselbach equation. (show all work) HA(aq) + H2O(lig) + H3O+(ag) + A (ag) 18. If the value of Ka for HCN is 4.9 x 10-10, calculate the equilibrium constant for CN-ag) +H2O(lig) H HCN(aq) + OH(aq) 19. Briefly justify the acidity difference in the following oxyacids: HCIO, HC102, and HC103. 20) What is the pH of a solution made by mixing 100.00 mL of 0.20 M...
please help
The following table, used for question 16, is partially complete: (ОН) pH 2.68 pОН ener 8.4 x 10 euen 16. (3 points) Fill in the six empty cells in the table. The following table, used for questions 2-8, is partially complete: Ka 1.8 x 10 pka Conj. Base formula pKb Acid Formula CH3COOH HOBI HNO2 5.40 3.14 2.2 x 10 Sec 17. (6 points) Fill in the twelve empty cells of the table above. 18. What is the...
I need help with these problems
07 Question (12 points) e See page 816 1st attempt See Hint Part 1 (6 points) Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H20. Ksp = 3.50x10-16 at a specifictemperature. See Hint Part 2 (6 points) What is the pH of this solution of cobalt(II) hydroxide? pH 04 Question |See page 792 (15 points) A buffer solution includes a weak acid and its conjugate base. 1st attempt See Hint Feedback Include...
i need help with finding the ph of an aq solution. im confused
9,10,12,13,14, &15. on 10 I caluclated 14 and 12 the closest
answer i got was 2.67, but i was exact. If its not a big
inconvience can you show me how? thank you
9. Calculate the pH of a 0.65 M NH3 solution if Kb for NH3 is 1.8x10-5. a) 2.47. b) 4.93. c) 11.53. d) 12.68. 10. The pH of a 0.2 M aqueous solution of...