Examples-of-bronsted

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Answers:All these models are used to describe acids and bases. The simplest model is the Arrhenius definition. In an aqeuous solution acids will produce Hydrogen (or Hydronium) ions. Hydrogen and Hydronium are used interchangeably (Hydronium is more technically correct) Here's an example HCl <======> H(+) + Cl- (in H2O) Arrenhius bases produce OH- or Hydroxide ions in Aqeuous solutions Ca(OH)2 <======> Ca(2+) + 2OH- The Bronsted Lowry Definition is a little more complex BL Acids will donate a hydrogen proton BL Bases will accept a hydrogen proton. Here's an example NH3 + HCl <=====> NH4(+) + Cl- from this you can see that NH3 (ammonia) a weak base accepts hydrogen proton for HCl a strong acid. Therefore NH3 is a Bronsted Lowry base and HCl is a bronsted lowry acid. The Lewis Definition is the most inclusive Basically a Lewis Acid is a compound that readly accepts an electron pair A Lewis Base is a compound that donates an electron pair. The most common example of Lewis Acid is BH3. Boron has an empty space to accept electrons. As you can see BH3 hasn't filled its octet properly. NH3 if you draw the Lewis structure will have an extra pair of electrons. Thus BH3 is a Lewis Acid and is willing to accept electron pair to satisfy the octet And NH3 the nitrogen has an extra pair of electrons that it is willing to donate. Something that is a BL acid can be a Arrenhius Acid. Something that is a Lewis Acid can be a BL acid as well as Arrenhius acid. Arrenhius acid has limited range because it has to be in aqueous solutions and it has to produce H+ ions or OH- ions depending on if it is an acid or a base.

Question:

Answers:Bronsted-Lowry Acid - a substance that donates protons (H+). Lewis Acid - a substance that accepts an electron-pair from another substance. Bronsted-Lowry Base - a substance that accepts protons (H+) from another substance. Lewis Base - a substance that donates an electron-pair to another substance. The Lewis theory applies to a broader variety of reactions, particularly in organic chemistry. This theory doesn't require that protons (H+) be involved. For example, in the reactin: BF3 + F- ----> BF4- BF3 is an acid and F- is a base; no protons are present.

Question:Assuming that each of the following compounds is soluble in water, predict whether each is likely to be a strong electrolyte, a weak electrolyte, or a non-electrolyte. a. isopropyl alcohol (C3H7OH) b. sodium fluoride (NaF) c. lithium hydroxide (LiOH) d. hydrocyanic acid (HCN) True or False, all insoluble compounds are non electrolytes. Explain. If someone could help me solve these it would be great. And after you are done answering them could you tell me how you got your answer that be awesome! Thanks!

Answers:A. Weak B. Weak C Strong D Weak (Your teacher should give you the sheet called "Relative strengths of Bronsted Lowry Acids and bases. False because nonelectrolytes are substances that dissolve in water but do not produce any ions. An example would be ethanol and sugar. However the reaction of NH3 in water produces NH4^+ and OH^-. (This was in my chem 121 textbook)


From Youtube

MC Titration - If You An Acid [Official Music Video]

www.facebook.com This is a music video made for an AP Chemistry class at Juanita High School. It covers some of the basic concepts of acids, bases and the pH scale. I hope you enjoy it! Lyrics: [Verse 1] Good evening and welcome everybody The first thing we will study Is the Bronsted-Lowry The two dudes said an acid gives a proton Never get it wrong And sing the song If you an acid give a proton If you a base take a proton Now youve probably figured out What the base is all about In the beginning a proton they are without Isnt until the reaction That we see things passing And then its then that the base gets some action Now it gets a little tricky So try to stick with me Lets take for example acid: HA After the reaction it becomes A Call it the conjugate base if you may Same happens to the base in the opposite way [Hook] If you an acid Give a proton If you a base Take a proton If you an acid Give a proton If you a BASE Take a proton [Verse 2] Next is some detail About the pH scale And what it means Its simple and clean Goes from 0 to 14 Acids on bottom Bases on top Another thing that you ought to be taught Is the pH of H2O At seven Its not really high or low But considered very neutral Before you forget the basic concept Ill give you some examples of things you might get Vinegar pH around 3 So we know its an acid by chemistry Milk pH about 6.3 So we know its kind of neutral And also healthy Ammonia pH 11.9 It is a base but I cant really think of a rhyme [Hook] [Verse 3 ...

Acids and Bases

Acids and Bases Verse 1: The first chemist to inform us, His name was Savant Arrhenius. He said acids give the ion H Plus, Bases give the ion OH Minus. HCl shows us a great example Hydronium forms in stock sample. NaOH is the other story Hydroxide makes the base inventory. Chorus: Acids and bases whats left to say? 3 different theories are together today Arrhenius, Bronsted-Lowry, Lewis All their ideas added to this Acids have a pH less than 7 pH 0 is as strong as heaven the pH of 7 is neutral Above which is base, must be well controlled. Verse 2: There was a problem with the first theory Solved by two chemists Bronsted and Lowry They proposed acids were proton donors And that bases were but proton receptors The result of this was acid-base reactions Always wanting equilibrium action Then the rise of conjugate pairs More acids and bases put out there Bridge: These two things can both be quite caustic If it hits you, you should test diagnostics Dont ever mess with the six strong acids They dissociate completely and will leave you roasted Verse 3: A guy called Lewis in 1963 He made the concept much harder for me Lewis bases donate electron pairs Lewis acids accept them there An adduct forms between the compounds This time the protons dont have to move around This is unlike Bronsted-Lowrys theory It makes the subject far from easy


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