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BioChem1100.tri-c
Chap10.timberlake
| Question | Answer |
|---|---|
| arrhenius -theory of acids (4) | 1. Taste sour (Latin "acidus" sour) 2. produce hydrogen ions (H+) 3. Change blue litmus to red 4. Corrode some metals |
| Name acids(minus1) - Hydrogen chloride (HCl) | Dissolves in water to form HCl(aq) - hydrochloric acid |
| HBr(minus1) (polyatomic) Bromide | hydrobromic acid |
| HNO3(Minus1) - Nitrate | Nitrous acid |
| SO4(minus2) Sulfate | H2SO4-sulfuric acid |
| SO3(minus2) sulfite | H2SO3 sulfurous acid |
| Hydronium ion | H3O+ Ion formed by the attraction of a proton (H+) to an H2O molecule |
| How does hydrochloric acid form? HCl | HCl = H2O form H3O+ and CL(minus1) |
| How does ammonia form? NH3 | NH3 + H2O forms NH4+ and OH(minus1) - Ammonium ions & hydroxide ions in equilibrium - WATER ACTS AS ACID by donating proton |
| Reaction where water acts as acid | Formation of ammonium & hydroxide |
| Bronsted-Lowry theory | Reaction between acid and base involves a PROTON transfer |
| Arrhenius theory | Acids are substances that produce hydrogen ions (H+) when dissolved in water |
| amphoteric | Can act as both an acid and a base |
| When does water accept H+? | When it reacts with a STRONGER acid |
| When does water donate H+ | When it reacts with a STRONGER BASE |
| Calculate pH | Enter [H3O+] value; presse EE; enter exponent; then enter - sign; press log key; change sign; round to scientific figures |
| What is VALUE of Kw (for all solutions) | Kw=[H3O+] x [OH-] = 1.00 x 10(neg14) |
| How do you find [OH-}? | 1.00 x 10(neg14) Divided by value of [H3O+] will equal [OH-] |
| Hydronium ion | H3O |
| Bronsted-Lowry acid | Donates a proton [H+]; thereby becomes H- |
| Bronsted-Lowry base | Accept a proton; thereby become positive |
| Water can be an acid or a base | True |
| When does water donate H+ | When it reacts with a stronger base |
| When does water accept H+ | When it reacts with a stronger acid |
| STrong acids | Perchloric (HCLO4); sulfuric (H2SO4); hydroidic (HI); Hydrochloric (HCL); nitric acid (HNO3) |
| Identify Conjugate Acid-Base Pairs | HBR(aq) + NH3(aq) ---- Br(neg) + NH4+ (positive) [Br is conjugate base and NH4+ is the conjugate acid |
| Do strong acids dissociate (separates into ions in water) | Yes, a strong acid dissociates completely |
| Do strong bases dissociate (separate into ions in water) | Yes, a strong base dissociates complete |
| Example of a strong base | KOH - solution consists of K+ and OH(neg) Write equation with ONE arrow: KOH(s) --------(addH2O) K+(aq) + OH(neg)(aq) |
| What is equation for acid dissociation constant? | K(asub) = [H3O+][A(neg)/[HA} |
| Acid ionization constant - equation | same as acid dissociation constantK(asub) = [H3O+][A(neg)/[HA} |
| What is ionization of water? | Amphoteric - water can be an acid or base |
| What is ion-product constant of water? | In pure water, the transfer of a proton between two water molecules produce equal number of HcO+ and OH(neg) |
| Ion-product constant of water - equation | Kw = [H3O+] x [OH(neg)] |
| Neutral solution - pure water | [H3O+] and [OH(neg)} are equal (however, most solutions are not neutral) |
| What does the pH scale represent? | A number between 0 and 14 represent the [H3O+] |
| A pH scale less than 7 is | Acid (the smaller the number, the stronger the acid) |
| pH = 7 | Neutral solution |
| pH is greater than 7 | This is a basic solution |
| pH - equation | pH = -log[H3O+] |
| Example of a strong base (home product) | Drano - NaOH (lye) pH value = 14 |
| Active metals | Potassium, sodium, calcium, magnesium, aluminum, zinc, iron & tin - react with acids to produce hydrogen gas (H2) |
| Acids, carbonates & bicarbonates | Strong acids added to a carbonates (or bicarbonates) produce bubbles of carbon dioxide gas, a salt, and water (ingredient in acid rain) |
| Neutralization - between acid & base | Neutralization is a reaction between an acid & base to produce a salt & water - cation in the salt comes from the base - the anion comes from the acid |
| Neutralization of a base (ex.) | HCl(aq) = NaOH (aq) ----- NaCL(aq) this is the salt and H2O water |
| Titration | The addition of BASE to an acid sample to determine the concentration of the acid |
| Name acid with H and a non metal | Use prefix "hydro" and end with ic acid Ex. Hydrochloric acid |
| Name acid with H and polyatomic ion | Change end of polyatomic ion from "ate" or "ite" to "ic acid" or "ous acid" Ex. ClO3 is chlorate - becomes HClO3 - chloric acid |
| Name base | Bases with OH- ions are named as "hydroxide" of metal Ex. Al(OH)3 aluminum hydroxide |
| what produces H+ in aqueous solutions (acid or base?) | Acid |
| What produces H- in aqueous solutions | Base |
| Adding an acid to pure water increases ________ and causes it to _________ and decreases _________ | Adding an acid to pure water increases [H3O+] and increases the concentration to more than 1.0 x 10neg7 power and decreases the [OH(neg)] |
| Adding a base to pure water increases _________ and causes it to _____________ and decreases the ___________ | Adding a base to pure water increases the [OH-] and causes its concentration to increase above 1.0 x 10-7 and decreases the [H3O+] |
| titration process uses an _______________ to measure the concentration of a solution | an INDICATOR will change color to show the concentration |
| End point - what does this mean in titration? | It means the solution has reacted with the indicator & can be compared to the test strips (or other media) |
| Strong acids & strong bases - what will form neutral salts? | BASES -"Lippy (Li) Kissy (K) Salty (Na) Calcium (Ca)Maggy (Mg) Syrup (SR)Barium combine "Clorie" (Cl) Boring (Br) Iodine (I) and "Nitie" Nitric acid |
| What is pH range in blood? | Blood MUST be pH 7.35-7.45 or health is threatened |
Created by:
walterina4327