1
Q
- Arrhenius describes acids as ……………
- Acids turn litmus …..
- Acids taste …………
- Are acids also electrolytes?
A
- substances that produce H+ ions when dissolved in H2O
- red
- sour
- yes
2
Q
- How do we name acids with a hydrogen ion and a nonmetal?
2. How do we name acids with a hydrogen ion and a polyatomic ion?
A
- hydro and non-metal drops “ide” for ic and acid. HCl = hydrochloric acid
- If polyatomic ion is an “ate”, it will become “ic acid”. If polyatomic ion ends in “ite”, it becomes “ous acid”.
3
Q
- Arrhenius describes bases as ……..
- Bases taste ……
- Bases feel …………
- Bases turn litmus ………..
- How do we name Arrhenius bases?
- According to Arrhenius, are bases also electrolytes? Why?
A
- producing OH- ions when dissolved in H2O.
- bitter or chalky
- slippery or soapy
- blue
- as hydroxides
- yes, because they dissociate into ions in water.
4
Q
- According to Bronsted-Lowry, and acid ………… H+, and bases ………….. H+
- Give example of above :
A
- donates, accepts
- in the reaction of ammonia and water, NH3 acts as the base, accepting an H from the H2O that donates it. Becomes ammonium and hydroxide.
5
Q
- Is water an acid, base, or both? Why?
- What is this called?
- name another substance that has this ability:
A
- H2O is either an acid or base because it can donate an H or accept an H depending on the basic or acidic strength of the other reactant.
- amphoteric
- HCO3- (bicarbonate or carbonic acid).
6
Q
- what is a strong acid vs a weak acid?
- What will a strong acid produce when dissolved in water?
- What is the 1 halogen that forms weak acids?
A
- strong acid completely ionizes in water whereas a weak acid only partially ionizes.
- a large concentration of H3O and the anion.
- Fluorine
7
Q
Name the 6 strong acids:
A
- Hydroiodic acid HI
- Hydrobromic acid HBr
- Perchloric acid HClO4
- Hydrochloric acid HCl
- Sulfuric acid H2SO4
- Nitric acid HNO3
8
Q
- From what groups on the periodic table are strong bases formed from?
- If the base is formed from another group, what is it?
- What do strong bases do in water?
A
- Groups 1A and 2A
- a weak base
- They completely dissociate into OH- and the cation.
9
Q
- What is equilibrium?
- T or F, at equilibrium, the concentrations of reactants and products is the same?
- What is Le Chatelier’s Principle?
- Make an example of Le Chatelier’s principle
A
- there are no further changes in the concentrations of the reactants and products. The rate of forward and reverse reactions is equal.
- F only the rate of forward and reverse reactions are the same.
- when equilibrium is disturbed, the rates of forward and reverse reactions change to relieve that stress and reestablish equilibrium.
- if a stress is placed on one side of an equation, the reaction will go faster in the direction away from the stress to restore balance.
10
Q
- In pure water, what are the concentrations of H3O+ and OH- at 25 degrees C?
- How do we notate the ion product constant of H2O?
- What is the formula to find the concentrations using the constant?
- How can we use this info to know whether or not a solution is acidic or basic?
- Is pure water neutral, acidic, or basic?
A
- 1x10^-7 M each
- Kw = 1.0x10^-14
- Kw= [H3O+] [OH-]
so we can replace …..
Kw= (1.0x10^-7)(1.0x10^-7)=
1.0x10^-14 - if [H3O+] = [OH-] it is neutral
if [H3O+] > [OH-] is is acidic
if [H3O+] < [OH-] it is basic - neutral
11
Q
- How to determine pH?
- How to determine pOH?
- What does pH and pOH always sum?
- How to determine [H3O+]?
- How to determine [OH-]?
- To how many decimal places must pH values be given?
A
- -log [H+]
- -log [OH-]
- 14
- 10^-pH
- 10^-pOH
- 2 decimal places
12
Q
- What is a salt?
- when acid reacts with metals, what does it make?
- When acid reacts with carbonates and bicarbonates (CO3 or HCO3), what does it make?
- When acid reacts with a base (OH-), what is produced?
A
- an ionic compound that doesn’t have H+ as the cation and OH- as the anion
- Hydrogen and a salt. The metal replaces the hydrogen on the acid.
- CO2, H2O, and salt
- The acid and base neutralize each other and produce water and salt.
13
Q
- What is titration?
- What is the indicator in a titration test?
- At the endpoint, the moles of base are …….. to the moles of acid.
- How can we find the molarity of the acid?
A
- a lab test to determine the molarity of an acid by using a base to neutralize a volume of acid.
- a substance (phenolphthalein) is added, drop by drop, to determine the endpoint (when solution turns pink).
- equal
- Use the formula M=moles of solute/Liters of solution. Remember that moles of base are equal to moles of solute at the endpoint.
14
Q
- What are the components of a buffer solution?
- What is the function of the weak acid in a buffer?
- What is the function of the conjugate base in a buffer?
A
- a combo of acid-base conjugate pairs: a weak acid and a salt of its conjugate base. Ex acetic acid HC2H3O2 and C2H3O2 acetate.
- it neutralizes a base.
- it neutralizes an acid
