1. Introduction to Biology

2. Chemistry

3. Water

4. Biomolecules

5. Cell Components

6. The Membrane

7. Energy and Metabolism

8. Respiration

9. Photosynthesis

10. Cell Signaling

11. Cell Division

12. Meiosis

13. Mendelian Genetics

14. DNA Synthesis

15. Gene Expression

16. Regulation of Expression

17. Viruses

18. Biotechnology

19. Genomics

20. Development

21. Evolution by Natural Selection

22. Evolution of Populations

23. Speciation

24. History of Life on Earth

25. Phylogeny

26. Prokaryotes

27. Protists

28. Plants

29. Fungi

30. Overview of Animals

31. Invertebrates

32. Vertebrates

33. Plant Anatomy

34. Vascular Plant Transport

35. Soil

36. Plant Reproduction

37. Plant Sensation and Response

38. Animal Form and Function

39. Digestive System

40. Circulatory System

41. Immune System

42. Osmoregulation and Excretion

43. Endocrine System

44. Animal Reproduction

45. Nervous System

46. Sensory Systems

47. Muscle Systems

48. Ecology

49. Animal Behavior

50. Population Ecology

51. Community Ecology

52. Ecosystems

53. Conservation Biology

[BOOK BIO] CLUTCH

The Strongest Bases in the World

Acid-Base Reactions in Solution: Crash Course Chemistry #8

a material that resists changes in the pH of a solution

a compound that donates hydrogen ions to a solution

How do we define an acid?

An acid is __________.

Acids, Bases and pH

lower the hydrogen ion concentration and lower the pH

No. A lower pH means a higher hydrogen ion concentration.

increase the hydrogen ion concentration and lower the pH

No. This describes the result of adding an acid.

increase the hydrogen ion concentration and increase the pH

No. A higher pH means a lower hydrogen ion concentration.

lower the hydrogen ion concentration and increase the pH

It might help to think of a base as the opposite of an acid.

Adding a base tends to __________ of a solution.

H2O &rarr; H+ + OH&ndash;

No. Although hydrogen ions are produced, hydroxyl ions are also produced in equal numbers.

NaOH &rarr; Na+ + OH&ndash;

No. In this reaction, no free hydrogen ion has been produced.

NH3 + H+ &rarr; NH4+

No. This reaction reduces the concentration of hydrogen ions.

HF &rarr; H+ + F&ndash;

Consider the definition of acid.

Which of the following dissociations is that of an acid?

The strengths and weaknesses of acids and bases - George Zaidan and Charles Morton

Consider the reaction between carbon dioxide and water to form carbonic acid:

CO2(g)+H2O(l)⇌CH2O3(aq)

In the ocean, carbonic acid immediately dissociates to form a proton and bicarbonate ion, as follows:

CH2O3(aq)+H+(aq)⇌CHO3−(aq)

If an underwater volcano bubbled additional CO2 into the ocean, would this sequence of reactions be driven to the left or the right? How would this affect the pH of the ocean?

increase the hydrogen ion concentration and raise the pH

No. As the hydrogen ion concentration increases, the pH decreases.

decrease the hydrogen ion concentration and raise the pH

No. Acids increase the hydrogen ion concentration; they do not lower it. Adding a base would produce the results indicated in this choice.

decrease the hydrogen ion concentration and lower the pH

No. Acids increase the hydrogen ion concentration.

Consider the properties of acids.

Adding acid tends to __________ of a solution.

The buffering action of carbonic acid (H2CO3) causes the pH of seawater to rise.

More carbon dioxide causes an increase in carbonic acid (H2CO3), which leads to an increase in the concentration of carbonate ion (CO32&ndash;).

No. The increase in carbon dioxide does cause an increase in carbonic acid. However, the increase in carbonic acid causes a decrease in the concentration of carbonate ion.

There is no cause for concern. Carbonic acid (H2CO3) is an excellent buffer and will help keep the pH of seawater constant.

No. When carbonic acid is present in equilibrium with bicarbonate ion, a buffer system exists. However, if carbonic acid is continually added to the system, the system is not in equilibrium.

More carbon dioxide causes an increase in carbonic acid (H2CO3), which leads to a decrease in the concentration of carbonate ion (CO32&ndash;).

Apply the equation for the carbonic acid/bicarbonate buffer system to the seawater problem.

Why is the increasing amount of carbon dioxide being taken up by the oceans a cause for concern?

Animation: Acids, Bases, and pH

Both the release of H​+​ and an increase in pH.

Both the release of H+ and a decrease in pH.

The release of H+ into the solution only.

The addition of an acid like HCl to an aqueous solution (pure water) would result in:a) An increase in pH only.b) Both the release of H+ and an increase in pH.c) Both the release of H+ and a decrease in pH.d) The release of H+ into the solution only.e) A decrease in pH only.

Acids

increases the oceanic concentration of carbonic acid

No. This is true because when CO2 dissolves in seawater, it reacts with water to form carbonic acid, but there is another correct answer.

No. The absorption of CO2 increases the concentration of carbonic acid, which does increase the acidity and lower the pH of seawater. However, recall that an increase in acidity corresponds with a decrease in pH.

reduces the carbonate ion concentration in the oceans and threatens calcifying organisms in marine ecosystems

No. This is true because the absorption of CO2 by the oceans leads to a decrease in the carbonate ion concentration, which is required for calcification, the production of calcium carbonate (CaCO3) by many marine organisms, but there is another correct answer.

increases the hydrogen ion concentration in the oceans but decreases the carbonate ion concentration and threatens the livability of the oceans for organisms that produce calcium carbonate shells

Consider how certain solutes can affect the relative concentration of hydrogen and hydroxide ions in an aqueous solution.

The absorption of human-generated CO2 by the oceans __________.

When H2 and CO2 react, acetic acid can be formed spontaneously while the production of formaldehyde requires an input of energy. Which of these conclusions can be drawn from this observation?
a. More heat is released when formaldehyde is produced compared to the production of acetic acid.
b.Compared to the reactants that it is formed from, formaldehyde has more potential energy than does acetic acid.
c. Entropy decreases when acetic acid is produced and increases when formaldehyde is produced.
d. Only acetic acid could be produced under conditions that existed in early Earth.

Acids and Bases

What Are Acids & Bases? | Chemistry Basics

a) NH4+ → NH3 + H+

b) H2CO3 → HCO3- + H+

c) NaOH → Na+ + OH-

d) HCl → H+ + Cl-

Which of the following reactions is most consistent with that of a base?a) NH4+ → NH3 + H+b) H2CO3 → HCO3- + H+c) NaOH → Na+ + OH-d) HCl → H+ + Cl-

The Strongest Acids in the World

Increasing the concentration of hydroxide ions.

Decreasing the concentration of hydrogen ions.

Decreasing the concentration of hydroxide ions.

Increasing the concentration of hydrogen ions.

In what way(s) do bases work to increase the pH of a solution?a) Increasing the concentration of hydroxide ions.b) Decreasing the concentration of hydrogen ions.c) Decreasing the concentration of hydroxide ions.d) Increasing the concentration of hydrogen ions.e) Both a &amp; b.f) Both c &amp; d.

Bases

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