quiz_acids and bases
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The document provides instructions for a 15 question true/false and multiple choice test on acids and bases. It explains that each question should be answered honestly by selecting the best answer, and that explanations will be provided for each question after it is answered. It also provides directions on how to navigate between questions and pages of the test.
1 of 33
![Instruction
There are 15 questions provided.
The questions are in a TRUE or FALSE and Multiple Choice
type of test.
Choose the BEST answer of each question. Just click the
word/s or letter of your desired answer.
After each question, an explanation is given to aid
understanding. Click the icon [ ].
To return, click . Click to proceed to the next page.
Answer HONESTLY.](https://image.slidesharecdn.com/interactivetestveraque-120928180240-phpapp02/85/quiz_acids-and-bases-2-320.jpg)
![Pure water is neutral.
TRUE
In pure water, (H3O+) or more often represented as [H+], is
1.0x10-7 M, and the [OH-] is also 1.0x10-7 M. since [H+] is
equal to [OH-], then water is considered neutral.](https://image.slidesharecdn.com/interactivetestveraque-120928180240-phpapp02/85/quiz_acids-and-bases-22-320.jpg)
![Calculate the pH of 0.0001 M HCl
solution.
D. 4
Given:
[H+] = 0.0001 M
[H+] = 10-4
Solution:
pH = - log [10-4]
pH = - (-4)
pH = 4](https://image.slidesharecdn.com/interactivetestveraque-120928180240-phpapp02/85/quiz_acids-and-bases-29-320.jpg)
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|
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3. Classifying acids and bases as strong or weak such as HCl (strong acid) and acetic acid (weak acid), NaOH (strong base) and NH3 (weak base).
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1. Acids donate hydrogen ions in water, forming hydronium ions, and have characteristics like turning litmus paper red and tasting sour. Bases form hydroxide ions in water and have opposite characteristics.
2. The pH scale measures how acidic or basic a substance is based on its hydronium ion concentration, with values from 0-14. More acidic substances have fewer hydronium ions and lower pH values closer to 0.
3. A substance is neutral when it has equal concentrations of hydronium and hydroxide ions, resulting in a pH of 7.3.3 Acids and Bases
3.3 Acids and BasesMelinda MacDonald
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The pink colour in test tubes #2 and #4 was caused by the basic solution (NaOH) reacting with the phenolphthalein indicator, which turns pink in basic solutions with a pH between 8.2-12.
The colour disappeared in test tube #5 because the acidic solution (HCl) was added, and phenolphthalein is colourless in acidic solutions below pH 8.2.
We could use an acidic solution like HCl to take away the pink colour in test tube #6, as it would neutralize the basic solution and lower the pH below 8.2, making the phenolphthalein colourless again.doFGHFHTRHJTRYTRJYLIOYUJTDHRTRwnload.pdf
doFGHFHTRHJTRYTRJYLIOYUJTDHRTRwnload.pdfRahul Radhakrishnan
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Acids produce hydrogen ions (H+) in water and bases produce hydroxide ions (OH-). Common acids include hydrochloric acid, sulfuric acid, and nitric acid. Common bases include sodium hydroxide and potassium hydroxide. Acids and bases react through a neutralization reaction where hydrogen ions and hydroxide ions combine to form water and a salt. Indicators are used to determine if a substance is an acid or base by changing color in their presence.Acids_&_Bases_Notes.pdfbbhrtyhytttyhuy44rtg
Acids_&_Bases_Notes.pdfbbhrtyhytttyhuy44rtghalegaye256
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The document discusses the properties and behaviors of acids and bases according to both Arrhenius and Lowry-Br淡nsted theories, highlighting their definitions, reactions, and the concept of neutralization. It explains the pH scale, the role of indicators, and provides practical applications and calculations for determining concentrations during titrations. Additionally, it covers the classification of strong and weak acids and bases, their ionization, and the reactions they undergo with various substances.Ad
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quiz_acids and bases
- 1. Instruction Questions and Answers Rationale
- 2. Instruction There are 15 questions provided. The questions are in a TRUE or FALSE and Multiple Choice type of test. Choose the BEST answer of each question. Just click the word/s or letter of your desired answer. After each question, an explanation is given to aid understanding. Click the icon [ ]. To return, click . Click to proceed to the next page. Answer HONESTLY.
- 3. Bases as defined by Arrhenius are Electron pair donors Proton acceptors Substance that produce hydrogen ions in aqueous solution Substance that produce hydroxide ions in aqueous solution All of the above
- 4. An example of a strong acid is dilute nitric acid concentrated acetic acid carbonic acid citric acid H2O
- 5. A given substance is an acid if in aqueous solution the substance has a pH above 7 has a soapy feeling turns litmus paper red reacts with a metal is colorless
- 6. Pure water is neutral.
- 7. Which is NOT a base? Mg(OH)2 BF3 H2O NH3 KOH
- 8. Which of the following statements is TRUE for all bases? Bases consist of oxides and hydroxides of metals. When bases react with acids, the only product is salt. Bases are colorless. Bases turn phenolphthalein from colorless to pink. Bases taste sour.
- 9. The color of phenolphthalein in an acid is colorless.
- 10. Indicators used in titration are added to the titrator the acid only the base only both acid and base the acid or base
- 11. A standard solution is one which is basic in nature which is acidic in nature whose concentration is being tested with known concentration which is added to the titrand
- 12. NH4+ is a Lewis base.
- 13. Calculate the pH of 0.0001 M HCl solution. 7 12 1 4 2
- 14. Blood has an acidic pH.
- 15. An acid found in the stomach is CH3COOH HNO3 HCL H2SO4 H2CO3
- 16. A pH of 2 is more acidic than a pOH of 12.
- 17. When the hydrogen ion (H+) is indicated in connection with its water solution, the ion represented is OH- H2O+ H2O2+ H3O+ None of the above
- 19. Bases as defined by Arrhenius are D. Substance that produce hydroxide ions in aqueous solution An Arrhenius base is a substance upon dissociation in water causes an increase in the concentration of the solvent anion, OH+.
- 20. An example of a strong acid is A. dilute nitric acid There are only six strong acids: HCl - hydrochloric acid HNO3 - nitric acid H2SO4 - sulfuric acid HBr - hydrobromic acid HI hydroiodic acid (also known as hydriodic acid) HClO4 - perchloric acid
- 21. A given substance is an acid if in aqueous solution the substance C. turns litmus paper red An acid is a substance whose water solution exhibits the following properties: 1. turns litmus paper red 2. has a sour taste 3. neutralizes bases 4. reacts with active metals to produce hydrogen gas
- 22. Pure water is neutral. TRUE In pure water, (H3O+) or more often represented as [H+], is 1.0x10-7 M, and the [OH-] is also 1.0x10-7 M. since [H+] is equal to [OH-], then water is considered neutral.
- 23. Which is NOT a base? B. BF3 BF3 is a Lewis acid. Mg(OH)2, NH3 and KOH are bases. H2O is amphoteric, it can act as an acid or a base.
- 24. Which of the following statements is TRUE for all bases? D. Bases turn phenolphthalein from colorless to pink. Solutions of bases have slippery, soapy feeling and a biting, bitter taste. Like acids, bases also react with indicators. Bases turn red litmus blue, turn methyl orange from red to yellow, and turn phenolphthalein from colorless to pink. Bases neutralize acids to form water and a salt. Bases have hydroxide ion concentration.
- 25. The color of phenolphthalein in an acid is colorless. TRUE Phenolphthalein is often used in titrations, it turns colorless in acidic solutions and pink in basic solutions. If the concentration of indicator is particularly strong, it can appear purple.
- 26. Indicators used in titration are added to E. the acid or base An indicator is added to the titrand (either an acid or a base), whose concentration is unknown.
- 27. A standard solution is one D. with known concentration A standard solution is a solution containing a precisely known concentration of an element or a substance. Standard solutions are used to determine the concentrations of other substances, such as solutions in titrations.
- 28. NH4+ is a Lewis base. FALSE NH4+ is a Lewis acid. It donates one proton (H+). H2O + NH4+ <--> H3O+ + NH3
- 29. Calculate the pH of 0.0001 M HCl solution. D. 4 Given: [H+] = 0.0001 M [H+] = 10-4 Solution: pH = - log [10-4] pH = - (-4) pH = 4
- 30. Blood has an acidic pH. FALSE The pH of blood is 7.35 7.45. pH < 7.00 acidic solution pH = 7.00 neutral solution pH > 7.00 basic solution Therefore, blood has a slightly basic pH.
- 31. An acid found in the stomach is C. HCL Hydrochloric acid, normally found in the gastric juices, is necessary for the proper digestion of proteins in the stomach.
- 32. A pH of 2 is more acidic than a pOH of 12. FALSE pOH is a measure of the concentration of hydroxide ions. pOH = 14 pH pOH = 14 2 pOH = 12 Therefore, a pH of 2 is equal to a pOH of 12.
- 33. When the hydrogen ion (H+) is indicated in connection with its water solution, the ion represented is D. H3O+ Hydronium ion (H3O+) is responsible for the observed properties of acids in water. For the sake of simplicity, H+ is often use instead of the more accurate H3O+. For aqueous solutions, whenever H+ is written, it should be understood as H3O+.