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pharmaceutics exam 2
| Question | Answer |
|---|---|
| What is a proton acceptor? | Bronsted-Lowry definition of weak base |
| What is the absorption of a weak electrolyte that is determined mainly by extent to which drug exists in unionized form at site of absorption | pH-partition hyopthesis |
| What is used to measure the strength of a buffer? | Buffer capacity |
| What is a electron donor? | Lewis electronic definition of weak base |
| What are substances that do not ionize in water | Nonelectroylte |
| What are substances that partially ionize in water? | Weak electrolyte |
| What is a substance that ionizes in aqueous solutions? | Electrolyte |
| What is an electron aceptor? | Lewis electronic definition of weak acid |
| What is the acid containing two or more ionizable hydrogens | Polyproctic acid |
| What is a solution that resists the pH when acid or bases are added to it? | Buffer |
| What are substances that completely ionize in water? | Strong electrolyte |
| What is used to calculate the pH of a buffer? | Henderson-Hasselbalch equation |
| What is a proton donor? | Bronsted-Lowry definition of weak acid |
| What are the electrolytes that have both acidic and basic functional groups? | Amphoteric electrolytes |
| What is Hydrochloric acid? | Strong electrolyte |
| What is Acetic acid? | Weak electrolyte |
| What is Ethanol? | Nonelectrolyte |
| How to find pka? | pKa= -log(Ka) |
| In which of the following substances does the ionization state depend on the pH of its environment? | Weak electrolytes |
| The pH of a solution containing equal amounts of a weak electrolyte and it's salt form is equal to the pKa of the weak electrolyte. True or false | True |
| Which of the following terms in the equation represent the unionized form of pilocarpine? pH = pKa + 1og ([B]/[BH+]) | B |
| Which of the following terms in the equation represent the unprotonated form of phenol? pH = pKa + log ([A]/[HA]) | A- |
| Which of the following forms of a drug has higher aqueous solubility? | lonized |
| Which of the following is an example of a polyprotic acid? | Phosphoric acid |
| Increasing the temperature of a solution always increases the solubility of the solute. True or False | True |
| How to determine which of the following is most soluble in water? | Bigger number= higher solubility (one that can pack the gram easier) |
| Which of the following best defines "solubility"? | Concentration of solute in a saturated solution |
| Which of the following can affect the solubility of a substance? | Temperature, pH, Polarity of the solvent molecules |
| In which of the following substances will solubility increase as the pH decreases below the pKa? | Weak bases |
| What is the pH of a solution containing 0.001M HCI? | 3 |
| Is a weak acid predominantly (>50%) ionized or (<50%) unionized at pH values above it's pKa? | >50% ionized |
| What is an accurate definition of solubility? | The maximum amount of a solute that will dissolve in a given amount of solvent at a specified temperature |
| Is a weak base is predominantly (>50% ionized) or (<50%) unionized at pH values above it's pKa? | <50% unionized |
| Which of the following is most soluble in water? Pentane Pentanol Pentanoic acid | Pentanoic acid |
| Diclofenac is a weak electrolyte. Based on the salt form, diclofenac sodium, what is diclofenac? | A weak acid |
| Which of the following solubility values is the highest? 1 mg/L 10 mg/L 100 mg/L 0.1 mg//L | 100 mg/L |
| Which of these 12-carbon molecules is most soluble in water? Dimethyl naphthalene Traumatic acid Sucrose | Sucrose |
| What is the process by which molecules leave the solid phase and enter into solution? | Dissolution |
| What studies are performed to assess drug release behavior of solids by determining rate of dissolution in different media? | Dissolution tests |
| What is the breakdown of solid dosage forms to granules or aggregates? | Disintegration |
| What is the breakdown of drug granules or aggregates into fine particles? | Deaggreation |
| What is the small film of saturated liquid surrounding solid drug particles? | Stagnant layer |
| What is the amount of drug dissolved per unit? | Dissolution rate |
| What is the measure of how fast dissolved drug molecules move through a unit area of the solvent? | Diffusion Coefficient |
| What are the solvents with low dielectric constants that are used to enhance solubility of non-polar drugs in aqueous preparations? | Co-solvent |
| What is the measurement of the ability of a substance to store charge, and the measurement of a solvents polarity? | Dielectric constant |
| What is the ability of a liquid to form a homogenous solution when mixed with another? | Miscible |
| pH below which a weak acid precipitates or pH above which a weak base precipitates | pH of precipitation (pHp) |
| What is the concentration of a solute in its saturation solution at a given temperature and pressure? | Solubility |
| What happens when the overall heat of solution is negative (heat is released when solute dissolves)? | Solubility decreases with increasing temperature |
| What happens when the overall heat of solution is positive (heat is required to dissolve solute)? | Solubility increases with increasing temperature |
| What does ionization state of drugs have an effect on? | Stability, Solubility, biological activity, and LADME |
| What affects the ionization state of a weak acid or weak base? | The pH enviroment |
| What is the importance and relevance of ionization states? | To know compounding, proper counseling, and make sure drugs aren't exposed to conditions that will change the properties |
| What are electrolytes able to do? | Able to ionize & conduct electrical currents |
| What electrolyte doesn't depend on pH environment? | Strong electrolytes |
| What does Arrhenius classification of an acid yield? | H+ in aqueous solutions |
| What does Arrhenius classification of an base yield? | OH- in aqueous solutions |
| What is the pH in neutral water? | 7 |
| What does pKa+pKb= pKw equal? | 14 |
| How to find the pH of a strong acid? | pH= -logC |
| How to find the pH of a strong base? | pH= pKw + logC |
| How to find the pH of a weak acid? | pH= 1/2 (pKa - logC) |
| How to find the pH of a weak base? | pH= 1/2 (pKw + pKa + logC) |
| What is the Henderson Hasselbalch equation for a weak acid? | pH= pKa + log(A-/HA) |
| What is the Henderson Hasselbalch equation for a weak base? | pH= pKa + log(B/BH+) |
| What is the ionization form of ionized forms (A-,BH+)? | Higher solubility and dissolution rate in water lower lipid solubility & less able to permeate lipid membranes through passive diffusion |
| What is the ionization form of unionized forms (HA,B)? | Lower solubility & dissolution rate in water higher lipid solubility & more able to permeate lipid membranes through passive diffusion |
| What happens if we add more H+ ions to a weak acid? | Makes more HA (more unionized) |
| What happens if we add more OH- to a weak acid? | Makes more A- (more ionized) |
| What is predominantly unionized at pH values below its pKa & predominantly ionized at pH values above its pKa values? | A weak acid |
| What happens if we add more H+ ions to a weak base? | Makes more BH ( more ionized) |
| What happens if we add more H+ ions to a weak base? | Makes more B (more unionized) |
| What is predominantly ionized at pH values below its pKa & predominantly unionized at pH values above its pKa values? | A weak base |
| How is a salt formed? | It's formed from the reaction between an acid and a base |
| How to tell if a drug is a weak acid or weak base? Using Warfarin sodium | sodium is a strong base bc comes from NaOH so warfarin is a weak acid |
| How to tell if a drug is a weak acid or weak base? Using ephedrine hydrochloride | chloride is from HCl a strong acid, so ephedrine is a weak base |
| What is Morphine, Weak acid or Weak Base? Salt : morphine sulfate | Weak base |
| What is Ampicillin, Weak acid or Weak Base? salt: ampicillin sodium | Weak Acid |
| What is Codeine, Weak acid or Weak Base? salt: codeine phosphate | Weak base |
| What is Phenobarbital, Weak acid or Weak Base? salt: phenobarbital sodium | Weak acid |
| What is the importance & relevance of buffers? | Are necessary for aqueous drug preparations to be maintained by particular pH. Minimize drug degradation & optimize drug delivery |
| What is a buffer? | A system usually in aqueous system that has ability to resist a change in pH upon the limited amounts of an acid or base/ dilution with solvent |
| Why use a buffer? | To resist changes in Ph, adjust solution to pH, stability, solubility, absorption. |
| What do buffers consist of? | A weak acid and conjugate base (salt) or weak base and conjugate acid (salt) |
| What is buffer capacity? | Ability to resist changes in pH |
| What is the equation to find Bmax? | 0.576*C |
| What is the importance & relevance of solubility | It determines the maximum concentration of that drug in solution. |
| What is solubility? | The concentration of a solute in its saturated solution (at equilibrium) at a given temperature & pressure |
| What is an unsaturated solution? | When a solution contains less than 36g of NaCl, it is completely dissolved |
| What is an saturated solution? | When a solution has higher than 36g of NaCl, it is not completely dissolved still some particles left. |
| Which is most soluble? | one that can pack the gram easier (bigger number) |
| What is solubility like dissolves like? | It is governed by solute solvent interactions compared to sum of solute solute & solvent solvent interactions |
| When does low solubility occur? | When a solute-solvent interactions are less than solute-solute +solvent-solvent interactions |
| When does high solubility occur? | When solute-solvent interactions are greater than solute-solute +solvent-solvent interactions |
| What are factors affecting solubility? | Temperature, polarity & hydrogen bonding, particle size |
| What is an endothermic reaction? | Dissolution process that requires heat increasing temperature will increase solubility |
| What is an exothermic reaction? | Dissolution process that releases heat increasing temperature will decrease solubility |
| Why are Amorphous solutes more stable than crystalline? | It is disordered so easier to break apart |
| What is 1st rule out of the 4 general solubility rules? | Higher melting point means low water solubility for many molecules. Solubility in water is decreased with increased # of carbons |
| What is 2nd rule out of the 4 general solubility rules? | Solubility in water increases with increasing hydrogen bonding capacity of solute |
| What is 3rd rule out of the 4 general solubility rules? | Cis isomer is more soluble than trans isomer (trans packs better making more difficult to break solute-solute interactions) |
| What is 4th rule out of the 4 general solubility rules? | Increasing unsaturation increases solubility |
| Which of the following is most soluble in water? Butanol, Pentanol, or Heptanol | Butanol |
| Which of the following is most soluble in water? Octane, Octanol, Octanoic acid | Octanoic acid |
| What is the solubility of an weak acid unionized? | Lower solubility |
| What is the solubility of an weak acid ionized? | Higher solubility |
| What is the solubility of an weak base ionized? | Higher solubility |
| What is the solubility of an weak base unionized? | Lower solubility |
| What is the effect of pH on solubility of Weak acid? | pHp is pH below which means precipitates out as neutral acid |
| What is the effect of pH on solubility of Weak base? | pHp is pH above which precipitates out as neutral base |
| What does the term fall out solution mean? | Precipitates |
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Acasi23
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