ch 10

Question 1

1. Arrhenius describes acids as ……………
2. Acids turn litmus …..
3. Acids taste …………
4. Are acids also electrolytes?

Answer 1

1. substances that produce H+ ions when dissolved in H2O
2. red
3. sour
4. yes

Question 2

1. 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?

Answer 2

1. hydro and non-metal drops “ide” for ic and acid. HCl = hydrochloric acid
2. If polyatomic ion is an “ate”, it will become “ic acid”. If polyatomic ion ends in “ite”, it becomes “ous acid”.

Question 3

1. Arrhenius describes bases as ……..
2. Bases taste ……
3. Bases feel …………
4. Bases turn litmus ………..
5. How do we name Arrhenius bases?
6. According to Arrhenius, are bases also electrolytes? Why?

Answer 3

1. producing OH- ions when dissolved in H2O.
2. bitter or chalky
3. slippery or soapy
4. blue
5. as hydroxides
6. yes, because they dissociate into ions in water.

Question 4

1. According to Bronsted-Lowry, and acid ………… H+, and bases ………….. H+
2. Give example of above :

Answer 4

1. donates, accepts
2. 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.

Question 5

1. Is water an acid, base, or both? Why?
2. What is this called?
3. name another substance that has this ability:

Answer 5

1. 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.
2. amphoteric
3. HCO3- (bicarbonate or carbonic acid).

Question 6

1. what is a strong acid vs a weak acid?
2. What will a strong acid produce when dissolved in water?
3. What is the 1 halogen that forms weak acids?

Answer 6

1. strong acid completely ionizes in water whereas a weak acid only partially ionizes.
2. a large concentration of H3O and the anion.
3. Fluorine

Question 7

Name the 6 strong acids:

Answer 7

1. Hydroiodic acid HI
2. Hydrobromic acid HBr
3. Perchloric acid HClO4
4. Hydrochloric acid HCl
5. Sulfuric acid H2SO4
6. Nitric acid HNO3

Question 8

1. From what groups on the periodic table are strong bases formed from?
2. If the base is formed from another group, what is it?
3. What do strong bases do in water?

Answer 8

1. Groups 1A and 2A
2. a weak base
3. They completely dissociate into OH- and the cation.

Question 9

1. What is equilibrium?
2. T or F, at equilibrium, the concentrations of reactants and products is the same?
3. What is Le Chatelier’s Principle?
4. Make an example of Le Chatelier’s principle

Answer 9

1. there are no further changes in the concentrations of the reactants and products. The rate of forward and reverse reactions is equal.
2. F only the rate of forward and reverse reactions are the same.
3. when equilibrium is disturbed, the rates of forward and reverse reactions change to relieve that stress and reestablish equilibrium.
4. 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.

Question 10

1. In pure water, what are the concentrations of H3O+ and OH- at 25 degrees C?
2. How do we notate the ion product constant of H2O?
3. What is the formula to find the concentrations using the constant?
4. How can we use this info to know whether or not a solution is acidic or basic?
5. Is pure water neutral, acidic, or basic?

Answer 10

1. 1x10^-7 M each
2. Kw = 1.0x10^-14
3. Kw= [H3O+] [OH-]
   so we can replace …..
   Kw= (1.0x10^-7)(1.0x10^-7)=
   1.0x10^-14
4. if [H3O+] = [OH-] it is neutral
   if [H3O+] > [OH-] is is acidic
   if [H3O+] < [OH-] it is basic
5. neutral

Question 11

1. How to determine pH?
2. How to determine pOH?
3. What does pH and pOH always sum?
4. How to determine [H3O+]?
5. How to determine [OH-]?
6. To how many decimal places must pH values be given?

Answer 11

1. -log [H+]
2. -log [OH-]
3. 14
4. 10^-pH
5. 10^-pOH
6. 2 decimal places

Question 12

1. What is a salt?
2. when acid reacts with metals, what does it make?
3. When acid reacts with carbonates and bicarbonates (CO3 or HCO3), what does it make?
4. When acid reacts with a base (OH-), what is produced?

Answer 12

1. an ionic compound that doesn’t have H+ as the cation and OH- as the anion
2. Hydrogen and a salt. The metal replaces the hydrogen on the acid.
3. CO2, H2O, and salt
4. The acid and base neutralize each other and produce water and salt.

Question 13

1. What is titration?
2. What is the indicator in a titration test?
3. At the endpoint, the moles of base are …….. to the moles of acid.
4. How can we find the molarity of the acid?

Answer 13

1. a lab test to determine the molarity of an acid by using a base to neutralize a volume of acid.
2. a substance (phenolphthalein) is added, drop by drop, to determine the endpoint (when solution turns pink).
3. equal
4. Use the formula M=moles of solute/Liters of solution. Remember that moles of base are equal to moles of solute at the endpoint.

Question 14

1. What are the components of a buffer solution?
2. What is the function of the weak acid in a buffer?
3. What is the function of the conjugate base in a buffer?

Answer 14

1. a combo of acid-base conjugate pairs: a weak acid and a salt of its conjugate base. Ex acetic acid HC2H3O2 and C2H3O2 acetate.
2. it neutralizes a base.
3. it neutralizes an acid