Chemistry test: acids and bases – Flashcards

ACIDS: sour taste, reacts with metals to produce hydrogen gas, change color of litmus paper to red (example: lemons BASES: Bitter taste, slippery feel, reacts with acids to neutralize the characteristic properties, change litmus paper to blue (examples: soap, baking soda)

Arrhenius acid: a substance that produces H⁺ ions (a proton) when dissolved in water Bronsted-lowry acid: can donate a proton tpo another substance Arrhenius base: a substance that produces OH⁻ ions (hydroxide ions) when dissolved in water Bronsted -lowry base: can accept a proton from another substance

ACIDS W/ ONLY ONE ELEMENT: prefix hydro-, stem from element w/ the hydrogen, suffix -ic, word acid; HF- hydrofluoric acid ACIDS W/ 2+ ELEMENTS: contains hydrogen, oxygen, and another element/polyatomic ion; acids with polyacomic ions ending in -ATE, remove -ate and add -IC followed by word acid; acids w/ -ITE, drop -ite and add -OUS BASES: a metal and hydroxide (OH); called by ionic names (example: NaOH - sodium hydroxide

ACIDS: H₃PO₄ = H₃PO₄ + H₂O → H₂O⁺ + H₂PO₄⁻ HI = HI + H₂O → H₃O⁺ + I⁻ BASES: KOH = KOH → K⁺ + OH⁻ Sr(OH)₂ = Sr(OH)₂ → Sr²⁺ + 2OH⁻

Monoprotic: can only lose one p⁺ upon complete ionization (HCl would be HCl + H₂O → H₃O + Cl) Diprotic: can lose 2 p⁺ ions (H₂SO₄ would be H₂SO₄ + H₂O → H₃O⁺ + HSO₄ then to HSO₄ + H₂O → H₃O⁺ + SO₄²⁻) Triprotic: can lose 3 p⁺

HNO₂ + H₂O → NO₂⁻ + H₃O⁺ HNO₂ loses the H therefore it is the acid and NO₂⁻ is the conjugate base H₂O gains the H and forms H₃O⁺ therefore it is the base and forms the conjugate acid

Conjugate acids are formed when the bases accepts a H⁺, and strong bases form weak conjugate acids because the more readily you want something the less readily you will give it up. weak bases form strong conjugate acids because the less you want it the more readily you will give it up (regifting) same with acids - weak acid = strong conjugate base and strong acid = weak conjugate base

you need a chart for this that tells you which acid is stronger : the conjugate acid or the acid HClO₄(aq) + OH⁻(aq) ↔ H₂O (l) + ClO₄⁻(aq) acid is HClO₄ and conjugate acid is H₂O Since the chart says that the acid is stronger in this case, it shifts TO THE SIDE WITH THE WEAKER ACID or in this case to the right

pH scale measures the [H⁺] (molar concentration of protons) in a given solution; less than 7 is acid, more than 7 is base, 7 at 25° C is completely neutral

1) pH = -log [H⁺] so what id pH of solution with 0.05 molarity? pH = -log [0.05] so pH = 1.301 2) How many grams of nitric acid would need to be dissolved is a 750 mL solution to create a pH of 1.55? → 1.55 = -log [H⁺] → H⁺ = 0.02818 → x / .75L = 0.02818 → x= 0.02113 → 0.02113 = 1.33 g nitric acid

LiCl ( ) + AgNO₃ ( ) → AgCl ( ) + LiNO₃ ( ) determine which are aq and which are not with the chart, LiCl (aq) + AgNO₃ (aq) → AgCl (s) + LiNO₃ (aq) you can split up aq but not others to get: Li + Cl+ Ag + NO₃ → AgCl + Li + NO₃ if there is one on both sides cross it out to get Cl + Ag → AgCl SPECTAORS: they are the ones on both sides that you can cross out

Ca(OH)₂ and HCl : How to get equation on right side? first second + second first. also be mindful of charge when putting the elements together as in the case an Ca and Cl so you get: Ca(OH)₂ + HCl → H₂O + CaCl₂ Then balance equation!!!! Ca(OH)₂ + 2HCl → 2H₂O + CaCl₂

ACID: the number of hydroxide (H⁺) or hydronium (H₃O⁺) ions in solution BASE: number of hydroxide (OH⁻) ions in solution ALSO, strong and weak acids determined by ionization, not by concentration, so a change in concentration will not change whether the acid/base is strong or weak