lakeland acid/base review
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Lakeland Acid/Base Review. Click on a question to begin. Question 1. Try Again. Acids provide H +. Try Again. Correct!. An Arrhenius acid increases the concentration of H + in solution. Next Question. Question 2. Try Again. - PowerPoint PPT PresentationTRANSCRIPT
![Page 1: Lakeland Acid/Base Review](https://reader035.vdocuments.net/reader035/viewer/2022062315/56815755550346895dc4fd31/html5/thumbnails/1.jpg)
Lakeland Acid/Base Review
![Page 2: Lakeland Acid/Base Review](https://reader035.vdocuments.net/reader035/viewer/2022062315/56815755550346895dc4fd31/html5/thumbnails/2.jpg)
Click on a question to begin1 6 11
2 7 12
3 8 13
4 9 14
5 10 15
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An Arrhenius acid has
A) only hydroxide ions in solution B) only hydrogen ions in solution
C) hydrogen ions as the only positive ions in solution
D) hydrogen ions as the only negative ions in solution
Question 1
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Try Again
Try Again
• Acids provide H+
![Page 5: Lakeland Acid/Base Review](https://reader035.vdocuments.net/reader035/viewer/2022062315/56815755550346895dc4fd31/html5/thumbnails/5.jpg)
Correct!
• An Arrhenius acid increases the concentration of H+ in solution
Next Question
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When the pH of a solution changes from a pH of 5to a pH of 3, the hydronium ion concentration is
A) 0.01 of the original content B) 0.1 of the original content
C) 10 times the original content D) 100 times the original content
Question 2
![Page 7: Lakeland Acid/Base Review](https://reader035.vdocuments.net/reader035/viewer/2022062315/56815755550346895dc4fd31/html5/thumbnails/7.jpg)
Try Again
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• The pH scale is based on powers of 10. Strong acids have low pH values, strong bases have high pH values.
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Correct!
• As pH changes from 5 to 3 the acid is stronger so [H3O+] increases by 100.
Next Question
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If 5.0 milliliters of a 0.20 M HCl solution is required to neutralize exactly 10. milliliters of NaOH, what is the concentration of the base?
A) 0.1 M B) 0.2 M
C) 0.3 M D) 0.4 M
Question 3
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• MAVA = MBVB
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Correct!
• MAVA = MBVB so (.2)(5) = MB(10) MB = 0.1 M
Next Question
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Given the reaction: HCl(aq) + LiOH(aq) → HOH(_) + LiCl(aq)The reaction is best described as
A) neutralization B) synthesis
C) decomposition D) oxidation-reduction
Question 4
![Page 13: Lakeland Acid/Base Review](https://reader035.vdocuments.net/reader035/viewer/2022062315/56815755550346895dc4fd31/html5/thumbnails/13.jpg)
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• The products of the reaction are a salt and water
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Correct!
• A neutralization reaction is always an acid and base reacting to form a salt and water
Next Question
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Which ion is produced when an Arrhenius baseis dissolved in water?
A) H+, as the only positive ion in solution
B) H3O+, as the only positive ion in solution
C) OH–, as the only negative ion in solution
D) H– , as the only negative ion in solution
Question 5
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• Arrhenius bases always produce hydroxide
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Correct!
• Hydroxide, OH-, is the negative ion that is always produced by an Arrenhius base
Next Question
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As an aqueous solution becomes more acidic,the hydronium ion concentration
A) decreases B) increases
C) Remains the same D) Impossible to tell
Question 6
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• Acids create hydronium in solution
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Correct!
• The stronger the acid the more hydronium that is produced
Next Question
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Given the reaction: CO32– + H2O HCO3
–+OH–
The H2O molecule serves as a
A) Weak base B) Proton acceptor
C) Strong base D) Proton donor
Question 7
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• Identify a product that is similar to water to decide if it gained or lost a proton
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Correct!
• Water became OH- which means that it donated a H+ ion
Next Question
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Given the ionization constant equation: Kw = [H+][OH–] = 1.0 x 10–14
For water at 25°C, which statement is true?
A) [H+] = [OH–] B) [H+] > [OH–]
C) [H+] = 1.0 x 10–14 M D) [OH–] = 1.0 x 10–14 M
Question 8
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• Water is neutral, so its ions should be even
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Correct!
• Since water is neutral [H+] = [OH-]
Next Question
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What is the pH of a 0.01 M aqueous solutionof HCl?
A) 1 B) 2
C) 3 D) 4
Question 9
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• pH = - log[H+]
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Correct!
• pH = -log[H+] = -log(0.01) = 2
Next Question
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Given the reaction: HSO4– + HPO4
2– SO42– + H2PO4
–
Which pair represents an acid and its conjugatebase?
A) HSO4– and SO4
2– B) SO42– and H2PO4
–
C) HSO4– and HPO4
2– D) SO42– and HPO4
2–
Question 10
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• A conjugate acid/base pair differs by only 1 H+
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Correct!
• HSO4- and SO4
2- differ by only one H+
Next Question
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Given the reaction at equilibrium: HSO4– + NH3 SO4
2– + NH4+
What are the two Bronsted-Lowry acids?
A) NH3 and NH4+ B) HSO4
– and SO42–
C) NH3 and SO42– D) HSO4
– and NH4+
Question 11
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• Bases are proton acceptors
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Correct!
• NH3 and SO42- both gain a H+
Next Question
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Which of the following ionization constants (Kb)represents the strongest base?
A) 1 x 10-13 B) 1 x 10-9
C) 1 x 10-5 D) 1 x 10-3
Question 12
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• The more hydroxide produced, the higher the Kb value
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Correct!
• The strongest bases will have the highest Kbvalue
Next Question
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What is the pH of a [OH-] = 0.001 M solution?
A) 14 B) 11
C) 7 D) 3
Question 13
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• pOH = -log[OH-], pH = 14 - pOH
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Correct!
• pOH = - log(0.001) = 3• pH = 14 – 3 = 11
Next Question
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Nitrous Acid has the formula
A) HN B) HNO
C) HNO2 D) HNO3
Question 14
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• -ous ending of an acid name means that it is made with a polyatomic that ends in -ite
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Correct!
• Nitrous acid is hydrogen nitrite, HNO2
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Hydrobromic acid has the formula
A) HBr B) HBrO
C) HBrO2 D) HBrO3
Question 15
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• Hydrobromic acid means that the formula for the acid should come from the name hydrogen bromide
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Correct!
• HBr is hydrogen bromide. Following the rules for naming acids, hydrogen bromide becomes hydrobromic acid.
Next Question