Question

In: Anatomy and Physiology

1. Describe the pH scale, and define the terms acid and base. 2. Explain how carbonic...

1. Describe the pH scale, and define the terms acid and base.

2. Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve.

3. Define the terms acidosis and alkalosis, and explain how they relate to hypoventilation and hyperventilation.

4. Explain how ventilation is adjusted to help maintain acid-base balance.

Solutions

Expert Solution

1) pH Scale:

pH Scale is used to determine whether the solution or a water is acidic or base and it has a value scoring from 0-14.From 0-6 it is considered as acidic which donate the hydrogen and it include milk, urine, saliva, citric juices like lemon, tomato juice and hydrochloric acid. From 8-14 it is considered as base which receives or accept the hydrogen ion And it includes sea water, baking soda, ammonia as a solution, bleaches and liquid cleaners. Lastly the 7 is considered as neutral which is between acid and base.

The reciprocal of hydrogen ion in a solution determines the pH value of the solution using a logarithm.

pH scale and logarithm:


Related Solutions

Please explain the pH scale. Be sure to include acid, base, and neutral as well as...
Please explain the pH scale. Be sure to include acid, base, and neutral as well as hydroxide and hydrogen ion concentrations.
In the blood plasma, pH is maintained by the carbonic acid-bicarbonate buffer system. Explain how pH...
In the blood plasma, pH is maintained by the carbonic acid-bicarbonate buffer system. Explain how pH is maintained when (a) acid is added to the buffer system, (b) base is added to the buffer system?
1.Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve....
1.Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve. 2. Define the terms acidosis and alkalosis, and explain how they relate to hypoventilation and hyperventilation. 3. Explain how ventilation is adjusted to help maintain acid-base balance.
Lab Experiment 9 Acid‐Base I – Titration 1. Define and explain titration. 2. In the experimental...
Lab Experiment 9 Acid‐Base I – Titration 1. Define and explain titration. 2. In the experimental procedure, the buret is prepared by pre‐rinsing with NaOH and discarding the rinse. Explain the purpose of pre‐rinsing the buret with NaOH solution and identify what errors might be introduced if prerinsing is not performed before a titration.
A carbonic acid/carbonate buffer is used. Explain the action of said buffer in resisting pH changes...
A carbonic acid/carbonate buffer is used. Explain the action of said buffer in resisting pH changes after the addition of NaOH using relevant chemical equations and Le Chateliers Principle. Thank you.
Calculate the pH of a 0.105 mol/L solution of carbonic acid. Answer is 3.668. How do...
Calculate the pH of a 0.105 mol/L solution of carbonic acid. Answer is 3.668. How do I show my work for this question
Write the expectations for pH at Equivalence in Acid–Base Titrations. 1. Titrating a strong acid with...
Write the expectations for pH at Equivalence in Acid–Base Titrations. 1. Titrating a strong acid with a strong base (OR vice versa) Titrating a strong acid with a strong base (OR vice versa) pH at equivalence point: 2. Titrating a weak monoprotic acid with a strong base pH at 1⁄2 equivalence point: pH at equivalence point: 3. Titrating a weak diprotic acid with a strong base pH at 1st 1⁄2 equivalence point: pH at 1st equivalence point: pH at 2nd...
What is the pH of a 0.65 M solution of carbonic acid? Report your answer to...
What is the pH of a 0.65 M solution of carbonic acid? Report your answer to 2 decimal places.
Calculate the pH and concentrations of the following species in a 0.025 M carbonic acid solution....
Calculate the pH and concentrations of the following species in a 0.025 M carbonic acid solution. (Given Ka1 = 4.3x10-7 and Ka2 = 5.6x10-11) a) H2CO3 b) HCO3- c) CO32- d) H+ e) OH
1. The conjugate base of a stong acid has no effect on the pH. Why or...
1. The conjugate base of a stong acid has no effect on the pH. Why or why not? Include a comment on the conjugate acid of a base. 2. Given the discussion of question one above, then if I were to dissolve the following salt, KNO3, in water, what would the resulting pH be and why?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT