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Ch15-Acids & Bases
Question | Answer |
---|---|
a cation of a strong base is therefore ___ | pH neutral |
a cation is a small, highly charge metal ion (group I & II metal) is therefore ___ | a weak acid |
an cation is the conjugate acid of a weak base is therefore ___ | a weak acid |
an anion is the conjugate base of a strong acid is therefore ___ | pH neutral |
an anion is the conjugate base of a weak acid is therefore ___ | a weak base |
Strong acids | HCl, HBr, HI, HNO3, HClO4, H2SO4 |
Strong bases | LiOH, NaOH, KOH, Sr(OH)2, Ca(OH)2, Ba(OH)2 |
anions tend to form ___ whereas cations tend to form ___ | basic or neutral; acidic or neutral |
Give three example of acid found in the kitchen. | sour juice such as lemon, vinegar, soda, wine, banana, coffe |
What is the Arrhenius definition of acids and bases | In an aqueous solution, an acid produces H+ and a base produces OH- |
Give three example of base found in the kitchen. | soap, baking soda, detergent, lye, drain, ammonia, blood, milk of magnesia |
Define hydronium ion. How does this ion form? | H+ ion produced from the breaking down of acid is highly reactive. This ion bonds to water molecules to form hydronium ion H30+ |
What is the reaction that takes place when water auto-ionize? | H2O(l) + H2O(l) <-> H+ (aq) + OH-(aq) |
Define Kw? | Kw is the ion product constant for water at 25C |
Define pH | pH scale is used to measure the acidity of a solution. pH < 7 : acidic solution pH = 7 : neutral solution pH > 7 : basic solution |
How can the hydronium ion concentration be calculated based on the pH? | In chemistry, "p" stands for "-log". Hence, pH = -log[H+] or [H+] = 10^-pH. Since the pH scale is a log scale, a change of 1 pH unit = 10 fold change in [H30+] |
Define pOH | pOH is similar to the pH but respect to [OH-]. On pOH scale: pOH < 7 : basic pOH > 7 : acidic |
Define pKa | pKa = -log Ka. The smaller the pKa, the stronger the acid |
What is the definition of a Lowry-Bronsted acid and base? | An acid is a proton donor and a base is a proton acceptor. 2 substances related by the transfer of a proton are called conjugate acid-base pair |
What is the chemical difference between strong acid and weak acid? | Strong acids have strong electrolyte that ionizes (break up H+ ions) in solution 100% whereas weak acids under goes less than 100% dissociation |
What is the chemical difference between strong base and weak base? | Strong base have strong electrolyte that ionized (Break up OH-) in solution 100% whereas weak base under goes less than 100% of dissociation |
What is the physical meaning for an acid when Ka <<1? | |
The concentration of an acid (or base) can be solve by treating the problem as an _____ problem. | equilibrium problem |
How does the percent ionization (a) change with concentration of an acid? Does it increase, decrease or not change? | |
What type of polyprotic acid is phosphoric acid? | H3PO4; Triprotic |
Why does the Ka’s of acids decrease after successive loss of H+ ? | The removal of the next H+ is from a negatively charge spiece |
What is the equilibrium constant called that indicates the strength of a base? | Kb |
What is the relationship between Ka and Kb for a conjugate pair ? | Ka * Kb = Kw |
Name two chemicals that exhibit amphoteric behavior? | Water and N |
What acid-base condition increases the solubility of BaF2? Explain | |
Name four factors affecting acid strength? | Their Ka, |
Determine if an aqueous solution has pH >, = or < 7 for: a. Salts from strong base and strong acids. b. Salts from strong base and weak acids c. Salts from weak base and a strong acid. d. NH 4 ClO salt solution. | |
What is the criteria in determining the strength of an organic acid? | |
Give one example of a Lewis acid and a Lewis base. | |
Place the following in order of increasing acid strength. a. HF, HI, HCl, HBr. b. NaH, HF, NH3, CH4 c HOI, HOI, HOBr d. HOCl4, HOCl, HOCl2, HOCl3 | |
Name three chemicals found in the atmosphere that leads to the rain being acidic. | NO2, CO2, SO2 |