Hopefully we talked about this today :)
Ya Basic
(Not) Trippin' on Acid
100

You see some sludge and your pal Gary tells you that it has a concentration of 2.00 x 10-4 M hydrogen ion concentration. What is the pH? 

pH = -log[]

pH = -log[2.00 x 10-4] = 3.699

100

List the strong bases

The hydroxides: (LiOH, NaOH, ect...)

100

List the 6 strong acids that you should have memorized.

HCl, HBr, HI, H2SO4 (don't get this on your clothes), HNO3, HClO4

200

A solution has  [OH-] = 5.00 x 10-4 M. What is the pH?

pH = -log[]

pOH = -log [5.00x10-4] = 3.301

14.000 - 3.301 = 10.699

200

Is (CH3)3N a strong or weak base? Why?

Weak base, it is not a group 1 or 2 hydroxide compound. It can accept H+ to become (CH3)3NH+

200

What kind(s) of acid is HBr? (Definition and is it strong or weak?)

Arrhenius, Bronsted-Lowry, and maybe Lewis? eh? Depends on the context prolly

300

The pH of a solution is 4.5. Calculate the [OH-] concentration. 

[] = 10-p[]

pH = 4.5

pOH = 14 - 4.5 = 9.5

[OH-] = 10-9.5 = 3.2 x 10-10

300

Is H2O a strong or weak base? Why?

Weak base. It is not a Group 1 or Group 2 hydroxide containing compound. It can accept a H+ from another water molecule to form H3O+ and OH-
300

Is HF a strong of weak acid? Why? 

**HINT: perhaps you may want to look at a periodic table periodically 

Weak, because fluorine is really electronegative. 

400

We didn't talk about this, so let's do this later :)







CH3CO2H (aq) + H2O (l) ⇌ H3O+ (aq) + CH3CO2- (aq)

At equilibrium [CH3CO2H] =0.0787M; [H3O+] = [CH3CO2-] = 0.00118 M

What is the value for Ka? What is the value for Kb? (Kw = 1.0 x 10-14)

Ka = (0.00118)(0.00118)/0.0787 = 1.77 x 10-5

Kw = Ka x Kb

1.0 x 10-14/1.77x10-5 = 5.65 x 1010

400

If the pH of the solution is 6 in an aqueous solution at 25ºC, what is the pOH?

pOH = 8

400

If the pOH of an aqueous solution at 25ºC  is 9.5, what is the pH?

The ion product of water is 1.00 x 10-14

pH = 4.5

500

The ion product of water at 80ºC is 2.4 x 10-13. What are the concentrations of hydronium and hydroxide ions in pure water at 80ºC?

HINTS: -log[] = p[], [] = 10-p[]

Kw = 2.4 x 10-13

pKw = -log(2.4 x 10-13)= 12.62

12.62 = pH + pOH

pH = pOH

12.62/2 = 6.31

10-6.31 = 4.90 x 10-7

500

List and differentiate between the three definitions of bases.

Arrhenius base: Increases [OH-]

Brønsted-Lowry Base: Proton acceptor

Lewis Base: Any electron rich species


500

List and differentiate between the three acid definitions.

Arrhenius Acid: A substance that increases [H+] in aqueous solution

Brønsted-Lowry Acid: A H+ donor

Lewis acid: Any electron deficient species

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