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| 11653840343 | What is the name of the point of the curve where pH = pKa? | Halfway point |  | 0 |
| 11653840344 | At what point will [H] = [OH]? | Equivalence point |  | 1 |
| 11653840345 | If a weak acid is titrated with a strong base, will the pH at the equivalence point be greater than, less than, or equal to 7? | Greater than 7 |  | 2 |
| 11653840346 | What is the definition of a Buffer solution? | A solution which contains a weak acid (or weak base) and its conjugate base (or acid) | 3 | |
| 11653840347 | Given the data of a titration curve, how would one determine the Ka of the acid which is titrated? | Take the anti-log of the negative value of the solution's pH at the halfway point | 4 | |
| 11653840348 | How does the titration curve of a base differ from that of an acid? | The curve begins with a high pH which decreases as more titrant is added to the solution |  | 5 |
| 11653840349 | Why does the titration of a weak acid with a strong base have an equivalence point that is greater than 7? | When the weak acid reacts with the strong base, the acid's conjugate base is produced. At the equivalence point, all of the weak acid (and the strong base) has reacted, leaving the solution filled with the conjugate base, so the pH is above 7. | 6 | |
| 11653840350 | What is the definition of the equivalence point? | The point on the titration curve where all of the substance being reacted has been eliminated by the titrant substance. The pH at this point is not necessarily 7 | 7 | |
| 11653840351 | Which indicators would be the most useful when titrating a weak acid with a strong base? | Pink phenolphthalein or thymol blue. Both change colors at pH's between 7.6 and 9. These are the values between which the equivalence point of such a titration will lay | 8 | |
| 11653840352 | Is it possible to titrate a strong base with a weak acid? | Yes, but it will require a large volume of the titrant, and the equivalence point will lie above a pH of 7 | 9 | |
| 11653840353 | If a base is being titrated by an acid, at what point on the titration curve will pKb = pOH? | The Halfway Point. Consider the concepts of Kb, pOH, etc. and how they mirror the concepts of Ka, pH, etc. | 10 | |
| 11653840354 | Given an unmarked titration curve, how would you identify the equivalence point? | Isolate the section of the curve where the slope is steepest. Look for the center point of that section |  | 11 |
| 11653840355 | How does the titration of a buffered solution differ from that of a regular acidic or basic solution? | The titration of a buffered solution requires a significantly greater volume of titrant in order to react with all of the acid or base | 12 | |
| 11653840356 | When titrating a weak acid with a strong base, the indicator phenolphthalein is used. How can you tell when the equivalence point has been reached? | Look for when the pink color remains for approximately 5 seconds after the drop of base from the buret. Do not wait until the solution has a homogenous pinkish purple color. At that point, you are past equivalence. | 13 | |
| 11653840357 | acids characterisitics | sour taste acetic acid is found in vinegar citric acid is found in fruits | 14 | |
| 11653840358 | base characteristics | bitter tasting poisonous plants (people reject this flavor) broccoli, turnip, baking soda they feel slippery the react with oils in your skin to form soap many cleaning products contain NH3 blood drain cleanser contains KOH | 15 | |
| 11653840359 | arrhenius acid | they are the acids that dissociate in water to produce H+ ions | 16 | |
| 11653840360 | arrhenius base | they are the bases that dissociate in water to produce OH- ions (groups 1 and 2) | 17 | |
| 11653840361 | bronsted-lowery acid | acids that are proton donors they are willing to give up H+ the easier it becomes to remove an H+, the stronger the acid | 18 | |
| 11653840362 | bronsted-lowry base | bases that are proton acceptors | 19 | |
| 11653840363 | conjugate base | what the acid becomes once the proton has been donated | 20 | |
| 11653840364 | conjugate acid | what the base becomes after it accepts the proton | 21 | |
| 11653840365 | 8 strong acids | HNO3 HI HBr HCl H2SO4 HClO3 HClO4 HIO4 | 22 | |
| 11653840366 | what defines a strong acid | they completely dissociate in water willing to give up its protons strong electrolyte it has a weak conjugate base | 23 | |
| 11653840367 | what defines a weak acid | acids that only partially dissociate has a relatively strong conjugate base | 24 | |
| 11653840368 | strong bases | soluble compounds containing the hydroxide ions NaOH KOH LiOH RbOH Mg(OH)2 Ba(OH)2 Ca(OH)2 Sr(OH)2 | 25 | |
| 11653840369 | weak bases containing nitrogen | the lone pair on the nitrogen will accept the protons in solution the nitrogen has the ability to take the hydrogen from water | 26 | |
| 11653840370 | How they electronegativity of Y on oxyacid (H-O-Y) affects acid strength | acid strength increases as the electronegativity of Y increases. the electrons are more attracted to the Y weakening the H-O bond making it easier to remove a H+ | 27 | |
| 11653840371 | How # of oxygens on oxyacids affects acid strength | acid strength increases as more oxygens are added to the central Y increasing the number of electronegative oxygen atoms increases the electrons attraction toward the Y. This will reduce the forces of attraction in the O-H bond making ti easier to remove a H+ | 28 | |
| 11653840372 | carboxylic acids | they are weak organic acids the end with an COOH- | 29 | |
| 11653840373 | Kw | 1.0 X 10^-14 | 30 | |
| 11653840374 | Kw relationship with [OH-] and [H3O+] | kw=[OH-][H3O+] | 31 | |
| 11653840375 | how to find pH when given [H3O+] | pH=-log[H3O+] | 32 | |
| 11653840376 | how to find pOH when given [OH-] | pOH=-log[OH-] | 33 | |
| 11653840377 | how to find pOH when given the pH | 14-pH | 34 | |
| 11653840378 | how to find the pH when given the pOH | 14-pOH | 35 | |
| 11653840379 | how to find the Ka when given pKa | 10^-pKa | 36 | |
| 11653840380 | how to find the Kb when given the pKb | 10^-pKb | 37 | |
| 11653840381 | how to find the [H3O+] when given pH | 10^-pH | 38 | |
| 11653840382 | how to find the [OH-] when given pOH | 10^-pOH | 39 | |
| 11653840383 | Ka and Kb relationship with Kw | Kw=Ka x Kb | 40 | |
| 11653840384 | neutral | [H+] = [OH-] | 41 | |
| 11653840385 | formation of a neutral salt | strong acid + strong base | 42 | |
| 11653840386 | formation of an acidic salt | strong acid + weak base | 43 | |
| 11653840387 | formation of a basic salt | weak acid + strong base | 44 | |
| 11653840388 | larger Ka value means what | stronger acid because the acid is going more into completion | 45 | |
| 11653840389 | larger Kb value means what | stronger base | 46 | |
| 11653840390 | polyprotic acids | they can donate more than one H+ in a solution they have a different Ka value for each possible dissociation (removing one H+ at a time) (Ka1 and Ka2) | 47 | |
| 11653840391 | examples of polyprotic acids | H2SO4 H2CO3 | 48 | |
| 11653840392 | neutralization SA + SB reaction net ionic equation | H+ + OH- ---> H2O | 49 | |
| 11653840393 | what do we know about weak acids when we are writing the net ionic equation | WEAK ACIDS DONT DISSOCIATE SO DONT CANCEL THEM OUT | 50 | |
| 11653840394 | what does it mean to have a pH>7 | basic | 51 | |
| 11653840395 | what does it mean to have a pH<7 | acidic | 52 | |
| 11653840396 | amphoteric | they can accept or donate protons | 53 | |
| 11653840397 | lewis acids | they concern the acceptance or donation of electrons | 54 | |
| 11653840398 | what does and acid-base equilibrium favor | weak acid and a weak base | 55 | |
| 11653840399 | hydrolysis | states that salts (ionic compounds) can make a solution acidic, basic, or even have no effect on the pH | 56 |
