Solved: QUESTION 6 What Is A Conjugate Acid-base Pair For ...
Solved: QUESTION 6 What Is A Conjugate Acid-base Pair For ...
Is NH4 considered an acid or a base? Why? - Quora
Identify the conjugate acid-base pairs in the following ...
One conjugate acid-base pair in the reaction, NH4 + OH ...
A. Give the conjugate base of NH4+ ? B. Give the conjugate ...
Which of the following is an acid-base conjugate pair ...
Chapter 14 acids and bases homework Flashcards Quizlet
Answers (Conjugates) - Acids and Bases
is (NH4)2SO4 a salt, acid, or base? Yahoo Answers
What is the conjugate base of NH4+? Socratic
is nh4 a conjugate acid or base
is nh4 a conjugate acid or base - win
Acid and bases
Hello Everyone! I would like someone to tell me if what I am about to say is correct or not in the next chemical reaction, the conjugate acid is k+? K(OH) one arrow to the right K+ + OH- I know that K(OH) is a base since it increased the concentration of OH- in water but my book never mentions anything about conjugate acids of bases containing OH it only goes over the ones with H in them like NH3 and NH4+ but I think that my conclusion is correct since it agrees with Lewis structure for acids and bases and how cations are always lewis acids since they can accept a pair of electrons. Thank you in advance.
I'm currently learning about acid base reactions, and understand the concepts of arrhenius acid/base and bronsted acid/base pretty well, but I'm confused as to how something like lewis acid/base fits into this idea, and how it differs from the idea of nucleophiles/electrophiles. In the first two models (bronsted and Arrhenius), the idea seems to be that acids increase the hydronium concentration of the solution while bases decrease the hydronium concentration of solution. For instance, in the reaction HCl + NH3 → NH4+ + Cl-, the acid (HCl) dissociates (and reacts with water) creating H3O+ ions and the base (NH3) reacts with water to produce OH- ions, both of which clearly effect the overall concentration of H+ or OH-. In a lewis reaction, however, it often seem as if the reaction has nothing to do with H+ or OH-. For example, BF3 + F- ⇌ BF-. In this reaction, no dissociation occurs, and a singular product is formed instead of a conjugate acid and conjugate base. My question, is how does this constitute an acid base reactions, and how is this different than using the terms nucleophile and electrophile to describe the same exact process?
If the pKa of carboxylic acid is 3, then what is the pKa of the resulting carboxylate anion?
In general, what is the pKa of an acid's conjugate base? If HCl gives away its hydrogen, does Cl- have a pKa at all? I understand that pKa is used to measure the acidity of a molecule, but theoretically do all molecules have a pKa, even if they don't have hydrogen? Or do they not? Or is it infinite? I ask because I know both H2O and H3O+ have significant pKas, as well as NH3 and NH4+. But no one has ever explicitly taught me how to consideignore pKa of other conjugate pairs.
Hi, I cannot seem to find anywhere a straightforward answer to how to figure out at what pH a particular buffer solution will buffer. I am given a buffer system of equal concentrations NH3 and NH4+. I've used the Henderson-Hasselbach eq to calculate the pH of the sol'n to be 9.3. However, my notes from class suggest that the same exact equation in the same exact form:
pH = pKa + log ([A-]/[HA])
gives the pH at which the solution buffers. So is it true that the pH of a buffer solution, by itself, is the pH at which is buffers? I don't believe this to be the case because a conjugate acid/base pair should have a buffering affect at a certain range of pH, both above and below the pH of the buffer itself. EDIT: I merely need to find if the system buffers in the acidic,basic or neutral range. So I don't need an exact pH. I'm assuming it's buffering in the basic range because the buffer's pH is basic? Or would it be the opposite?
Hi guys, I am currently learning about buffers and this is really throwing me off. How come the acidity of a solution is only determined by the H+ ions? For example, if you add a strong acid to a buffered solution the base or conjugate base of the buffer "soaks up" the H+ ion. But then there is still an acid in the solution, its just not H3O. So I guess my question can be rephrased as "why do weak acids or bases not affect the pH of a solution?" I know the math behind the pH calculation but what is the real reason? Why does H3O (just another acid) affect the acidity of a solution but not NH4? Both are acids, so how come only H3O changes the pH? Sorry if my question is confusing but the online course I am taking really is awful at teaching me anything.
Hi all! Trying to solidify some orgo acid-base concepts, and want to make sure I'm understanding/explaining them well. I chose a simple example-- in this given rxn of ammonia & water:
NH*_3_* + H*_2_O* - NH*_4_*'+' + OH*'*
NH3 is our base, H2O is our acid; NH4+ is our conjugate acid, OH- is our conjugate base. (Using Bronsted-Lowry definitions).
The Keq for this reaction would be 10-6.3, (calculated by subtracting the pKa for acid from the pKa for the conjugate acid), which means that the reaction would favor the left side, i.e. the reactants. Correct?
The strength of an acid is determined (or can be determined) by the stability of its conjugate base-- which, if we look at the above rxn, makes perfect sense, since H2O and and NH3 are both far more stable molecules than NH4+ and OH- (namely, H2O is more stable than OH-, so, when acting as acids, the reaction should favor H2O), correct?
Is all of the above correct? I know that my language in terms of chemistry is not perfect-- "should favor" (I don't mean to anthropomorphize molecules), but, just in terms of an college-level introductory Organic Chemistry course, does my understanding of the above make sense/sound good? Thanks for any help-- appreciated as always! Cheers :)
Wanted to share my list of mnemonics that I found helpful for the MCAT. Many of these are from SDN but some are my own. I apologize in advanced for the crude and offensive ones but this often helps recall. If there's any mnemonics you use for MCAT topics not on here please share!
Beta vs. alpha carbohydrates
alpha = trans/down, beta = cis/up bow down to alpha, beta beat me up
Sympathetic vs. parasympathetic
Sympathetic = fight or flight, parasympathetic = rest & digest Paraplegics do a lot of sitting & resting (this is bad I'm really sorry but it works)
Electronegativity trend
FONCLBRISCH F > O > N > Cl > Br > I > S > C > H
Diatomic elements
BrINClHOF
Water soluble compounds
NAG SHAm Nitrates (NO3-) Acetate (CH3CO2-) Group 1 metal cations (Li, Na, K, Cs, Rb) Sulfates (SO42-) except with PMS Castro Bar Halogens except with PMS Ammonium (NH4+) PMS = Pb (Lead), Mercury (Hg), Silver (Ag) Castro Bar = Ca (Calcium), Str (Strontium), Ba (Barium)
Acid classifications
Increasing nuance/complexity when in alphabetical order. Arrenhius = acid forms H3O+ & base forms OH- in water (most elementary definition). Brownsted-Lowry = acids donate protons (H+) and bases accept them. Lewis = acids accept electron pairs and bases donate them.
La Chatelier's principle and equilibrium
When K & Q are in alphabetical order the arrow points to the direction the reaction will go to re-establish equilibrium. K > Q then reaction will go right, increasing product concentration. K < Q then reaction will go left, increasing reactant concentration.
Seminiferous tubules, epididymis, vas deferens, ejaculatory duct, urethra, penis SEVEN UP
mRNA post-processing
Exons Expressed, Introns in the trash
Taxonomy
Kingdom Phylum Class Order Family Genus Species King Philip Came Over For Gold & Silver
White blood cells
Neutrophils, lymphocytes, monocytes, eosinophils, basophils Nobody Likes Me Eating Badgers
Valence electrons
H likes to gain 1 e- to be stable, O 2, N 3, C 4 HONC 1234
Ecell site of redox
Reduction at cathode, oxidation at anode REDCAT ANOX
State functions
volume (V), Gibb's free energy (G), pressure (P), enthalphy (H), internal energy (E), entropy (S), temperature (T), potential energy (U), density (D) VG PHESTUD
Basic amino acids
histidine, arginine, lysine HAL
Cardiac cycle
systole = contraction, diastole = relaxation I Contracted a Cyst
Diverging lens image
diminished, upright, virtual DDUV
Acidic cations
Al, Fe, NH4, Zn, Cu, Be, Cr A Fact No Zebra Could Be Creepy
DNA order
DNA is read 3'-5' left to right like we read. But is synthesized 5'-3' largest to smallest just how a pyramid is built.
Bacterial conjugation
sexual reproduction in bacteria like a conjugal visit
Pancreas hormones
insulin, glucagon, somastatin I GLUed ON SOMe TATs to my pancreas
Can someone explain the difference between "salt of an acid" and "conjugate base"?
Got a midterm coming up later today, hoping for some help here. My textbook is describing salts of weak bases and weak acids. It mentions NH4F as an example, saying that NH4 is the salt of NH3, while F is the salt of HF. Can someone explain what "salt" means in this context, and how is it any different from just saying "NH4 is the conjugate acid" or "F is the conjugate base of HF." Is there a difference at all? p.s. Moderator, I think my previous post got caught in the spam filter. Looks like this one went through, so feel free to delete the other one.
The conjugate base of ammonium ion, NH_4^+, is ammonia, NH_3..... .....And the conjugate acid of bisphosphate ion, HPO_4^(2-), is H_2PO_4^-. As with all of these conjugate acid/conjugate base problems, I am simply simply exchanging a proton, H^+, and conserving mass AND charge. If mass and charge were not conserved, it would not be a realistic exercise. What are the conjugate bases of H_2SO_4, HSO_4^-, NH_3, HO^-, and NH_2^-? What are their conjugate acids? For each reaction, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base. C5H5N(aq)+H2O(l)⇌C5H5NH+(aq)+OH−(aq) C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH−(aq) H2O donates a proton (H+) to C5H5N, it is the B-L acid C5H5N accepts a proton; it is the B-L base C5H5NH+ is the conjugate acid of C5H5N OH- is the conjugate base of H2O. Write the ... Acid: HSO4 Base: NH3 Conjugate acid: NH4 Conjugate base: SO4 Got the wrong answer? Click Here to review Click Here to go back to the QUIZ!! 4) Identify the acid, base, conjugate acid, and conjugate base of C2H3O2 + HCl -----> C2H4O2 + Cl Acid: HCL Base: C2H3O2 Conjugate acid: C2H4O2 Conjugate base: Cl Got the wrong answer? Click Here to review Click Here to go back to the QUIZ!! 5) Identify ... NH4's conj. base is NH3. OH's conj acid is H2O. this can be seen easily through proton transfer in this reaction. Lewis Acid/Base Defn. NH4(+) is an acid -- electron pair acceptor. NH3 (-) is a... NH4 is a positively charged ion. It is also the conjugate acid to ammonia (it is the protonated form of ammonia). Ammonia is basic and its conjugate acid is acidic. Ammonia is a weak base. H₃O⁺/H₂O and H₂O/OH⁻ are acid-base conjugate pairs, but H₃O⁺/OH⁻ is not. The answer: c. NH₄⁺/NH₃. 2 0. Simonizer1218. Lv 7. 3 years ago. c. NH4+/NH3; NH4+ is the acid and NH3 is the conjugate base. 1 0. Still have questions? Get your answers by asking now. Ask Question + 100. Join Yahoo Answers and get 100 points today. Join. Trending Questions. Trending Questions. is it ... H 2017 + NH 4 (99) NH3 (09) + H 30 (0) A NH4 Is An Acid And NHg Is Its Conjugate Base, B. H2O Is A Base And NH3 Is Its Conjugate Acid. C. H20 Is An Acid And H30* Is Its Conjugate Base. D. H20 Is A Base And NH4 Is Its Conjugate Acid. E. H20 Is An Acid And NH3 Is Its Conjugate Base. This problem has been solved! Explanation: N H + 4 is the acid because it donates an H + ion to the water. It then becomes ammonia ( N H 3 ), which would be the conjugate base of N H + 4. In order to find the conjugate acid of a base, you add a H. In the equation: HCl + NH3 -> NH4+ + Cl-. We can see that from NH3 to NH4+, a H is added because it goes from neutral to a charge of +1... Ummm… when NH4 is added to water, it forms two conjugates, a conjugate acid and conjugate base. Basically, NH4 + H2O -> NH3 + H3O. Due to the definition of an acid by Bronsted and Lowry, which is plainly the acid is a proton donator and the base is the proton receiver, NH4 would be the acid in this situation.
Is NaCl acidic, basic, or neutral (dissolved in water ...
🚀To book a personalized 1-on-1 tutoring session:👉Janine The Tutorhttps://janinethetutor.com🚀More proven OneClass Services you might be interested in:👉One... 🚀To book a personalized 1-on-1 tutoring session:👉Janine The Tutorhttps://janinethetutor.com🚀More proven OneClass Services you might be interested in:👉One... To tell if NaCl (Sodium chloride) forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralization re... View full question and answer details: https://www.wyzant.com/resources/answers/706592/identify-the-following-reaction-label-the-acid-conjugate-acid-base-and... http://www.chemistry.jamesmungall.co.ukAcid Base Chemistry7. Relative acidity and basicity -- competition for H+ a. pKa and pKb of conjugate acids and bases[... To tell if (NH4)2SO4 (Ammonium sulfate) forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralizat... All this talk of conjugate sounds scary! Not really, this video looks at what a conjugate base and acid are with multicoloured equations. Take a look to find... Learn everything about Conjugate Acids and Bases. We explain this with the real world example of vinegar.At Fuse School, teachers and animators come together... Conjugate acids and bases are usually introduced in organic chemistry along with a review of resonance. Category Education; Show more Show less. Loading... Autoplay When autoplay is enabled, a ...