Drug workings Flashcards
questions
You have prepared 300 mL of 5% w/v solution of H2SO4 (98.1 g/mol) using a concentrated, 15% w/v solution.
What is the concentration of the final solution in N?
1.02 N.
You have 500 mL of a 10% w/v solution of
NaOH
NaOH (40 g/mol). You dilute it to a total volume of 2 liters with distilled water.
What is the molarity (M) of the final solution?
0.625 M
You need to prepare 1 liter of a 1 N HCl
solution starting with a concentrated 37% w/v
HCl stock solution. Given that
HCl has a molar mass of 36.5 g/mol, what volume of the concentrated solution should you use?
Approximately 98.6 mL (closest to option B: 100 mL)
You have 400 mL of a 3% w/v solution of
KNO3 (101.1 g/mol). How many moles of
KNO3 are present in the solution?
Approximately 0.12 moles
You have 200 mL of 2 M H2SO4 and you dilute it to a final volume of 1 liter. What is the normality (N) of the diluted solution?
0.8 N
Acids and Bases
If the Ka is higher, what happens to the acidity?
Acidity increases
Acids and bases
What does the Ka refer to?
The dissociation of acids
Acids and bases
How do organic bases generally behave in solution
They act as weak bases
What happens to the basicity the higher the Kb gets?
Basicity gets higher.
Pka=-logKb
The lower the value of Pka, the (stronger/weaker) the base
Stronger
Acids and bases
Which form of a weak base is able to cross cell membranes?
The unprotonated version because it is nonpolar
Acids and bases
Which form of a weak base is soluble in aqueous environments?
The protonated form
Acids and bases
How does pH affect the absorption of a weak base?
Lower pH (more acidic) increases the protonated (BH⁺) form, reducing absorption; higher pH favors the unprotonated (B) form, increasing absorption.
Which will dominate when pH<pKa
If pH < pKa: The protonated (BH⁺) form will dominate, and the base will be more ionized.
Which will dominate when pH> pKa
If pH > pKa: The unprotonated (B) form will dominate, and the base will be less ionized.
