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Chapter: 4.5 / Q: 50
A fresh sample of blood (a buffered solution) is withdrawn from the body and its pH measured at 7.4. A small quantity of strong acid (as an isotonic solution) is added to it
Chapter: 4.5 / Q: 51
Blood in the body is different to a buffered solution held in a beaker. This is because hydronium (hydrogen) ions can be removed from solution in blood almost immediately by:
Chapter: 4.5 / Q: 52
The definition of an acid is a substance that reacts:
Chapter: 4.5 / Q: 53
Choose the INCORRECT statement about buffer solutions
Chapter: 4.5 / Q: 54
In the condition known as acidosis, the blood pH would be
Chapter: 4.5 / Q: 55
As the blood becomes more acidic, hydrogen (hydronium) ions combine with bicarbonate ions to form carbonic acid which in turn dissociates into carbon dioxide (to be breathed out by the lungs) and water
Chapter: 4.5 / Q: 56
A buffer solution consisting of H2PO4 − (acid) and HPO4 2− (base), in a ratio of 1:4, maintains the pH at 7.4. What is the ratio of these two components if the pH were to become 8.4 after the addition of more of the basic component of the buffer
Chapter: 4.5 / Q: 57
Which of the following pH values would you expect to a dilute solution of a weak base to have
Chapter: 4.5 / Q: 58
A buffer solution having a pH of 8.5 has a small amount of strong acid added to it. What is its pH value likely to be closest to
Chapter: 4.5 / Q: 59
Which of the following statements about the role of the kidneys or lungs in the maintenance of acid-base balance within the body is FALSE
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