Acids and Bases
Acids and bases are fundamental concepts in chemistry, pivotal to understanding various natural phenomena and industrial processes. Acids are substances that donate protons, while bases accept them. This interplay of proton transfer defines their characteristic properties, including pH levels and chemical reactivity. From the acidic taste of citrus fruits to the soothing properties of antacids, the influence of acids and bases permeates daily life. In chemistry, they serve as crucial components in reactions, catalysis, and the regulation of biological systems. Understanding their behavior is essential for students, researchers, and professionals across scientific disciplines.
Questions
- Which acid and which base would you combine to form the salt aluminum sulfate, #Al_2(SO_4)_3#?
- How would you use the Henderson–Hasselbalch equation to calculate the pH of each solution?
- Which is a stronger acid: acetic acid or hydrochloric acid?
- What happens when hydrochloric acid is added to water? Why is heat given off?
- If #HCl# is a strong acid, what is its Ka?
- What is the pOH of a #4.8xx10^(-10) M# #H^+# solution?
- What is an example of a neutralization practice problem?
- How do pH values of acids and bases differ?
- When the name of an anion that is part of an acid ends in -ite, what does the acid name include?
- How do strong acid solutions conduct electricity?
- Is nitric acid the strongest acid and acetic acid the weakest?
- What is an oxyacid?
- What happens when you mix an acid and a base together?
- What contains more #OH#- ions?
- Is #HF# a strong acid or weak?
- Why is the normal boiling point of #HF# (#19.5# #""^@C#), so high compared to that of #HCl# (#-85.0# #""^@C#)?
- Why does calcite fizz when it comes in contact with hydrochloric acid?
- Why is the hydrogen ion (H+) the same as a proton?
- What is the pOH of a #8.4x10^-11 M# #OH^-# solution?
- How is the concentration of H+ lons related to the concentration of OH- ions for a substance?