CHEM 210 Exam 1 Review 2024 With Questions And Answers - Portage Learning.
What is a BL acid? BL base? - Answer Acid is a proton donor while a base is p... [Show More] roton
acceptor
List the 6 strong acids - Answer HClO4, HCl, HBr, HI, HNO3, H2SO4
List the 6 strong bases - Answer LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
What is the eq. for the dissociation of a weak acid? - Answer HA <=> H+ + AKa = ([H+][A-])/[HA]
What is the eq. for base hydrolysis? - Answer B + H2O <=> BH+ + OHKb = ([BH+][OH-])/[B]
What is the equation for pH and pOH? - Answer pH = -log[H+]
pH + pOH = -log(Kw) = 14
pOH = -log10 [OH-]
How would you convert pH to pOH and vice versa? - Answer pH = 14 - pOH
pOH = 14 - pH
How would you convert pH to [H3O+]? - Answer pH = - log[H3O+]
[H3O+] = 10^-pH
How would you convert [H3O+] to [OH-]? - Answer Kw = 1 x 10^-14 = [H3O+][OH-]
Calculate the [OH-] in 6 M HNO3 and [H3O+] in 6.0 M NaOH at 25 C. - Answer Kw =
[OH][H3O] = 1 x 10^-14
(1 x 10^-14) / 6.0 M = 1.7 x 10^-15
The pH of a seawater sample is 8.30 what is [H3O+]? - Answer [H3O+] = 10^-pH
CHEM 210 Exam 1 Review 2024 With Questions
And Answers - Portage Learning
10^-8.3 = 5.01 x 10^-9
An acid at a pH of 0 has an OH concentration of? - Answer 1 x10^-14
and an H+ concentration of 1
What is the Ka and pKa range for a very strong acid?
Weak acid?
Extremely weak? - Answer very strong: ka >0.1 pka <1
weak acid 10^-6 - 10^-3 pka 3-5
extremely < 10^-15 pka>15
Salt is the product of what rxn? - Answer Acid-base
usually strong electrolytes that completely dissociate in water
Strong acid - strong acid
strong acid - weak base
strong base - strong base
weak acid - weak base
Calculate the pH of 0.010 M solution of sodium hypochlorite (NaClO) The Ka is 2.9 x
10^-18 - Answer Kw = Kb x Ka
Kb = Kw/ka
kb = 3.45 x 10^-7
R ClO- + H2O <=> OH- + HClO
I 0.010
C - X + X + X
E 0.010 - X X X
0 = X^2 - 3.45 X 10^-7 X + 3.45 X 10^-9
quadratic eq.
x = 5.86 x 10^-5 = [OH]
-log[OH] = pOH
pH = 14 - pOH
pH = 9.77
What eq. are useful when working with weak acids and bases? - Answer HA <=> H+ +
Aka = [H][A]/[HA]
B + H2O <=> BH + OH
Kb = [BH][OH]/[B]
Calculate [H3O], pH, [HA], [A-], [OH], and alpha of .100 M propanoic acid
(CH3CH2CO2H)
pKa = 4.87 Ka = 1.34 x 10^-5 - Answer HA (aq) + H2O <-> H3O + AF - x x x
Ka = [H3O][A]/[HA] =
x^2 /(F-x)
[H3O] = [A-] = x
1.34 x 10^-5 = x^2 /(0.010-x)
quadratic eq.
x = 1.151 x 10^-3 = [H3O]
pH = -log(H3O) = 2.94
pOH = 14 - 2.94
[A-] = [H3O]
[HA] = F - x = 0.01 - 1.151 x 10^-3
alapha = x/ F (100) = 1.151 x 10^-3/.01 (100)
Calculate the [OH], [H3O], pH [BH], [B], and alpha of 0.1 M CH3NH2 Ka = 2.31 x 10 -11
- Answer B (aq) + H2O <-> BH + OHF - x x x
Kb = [BH][OH]/[B] =
x^2 /(F-x)
[BH] = [OH] = x
kb = kw/ka = 4.33 x 10^-4
x = (-Kb +sq rt(kb)^2 + 4(Kb)(F))/2
x = 6.367 x 10^-3 = [OH] = [BH]
[H3O] = Kw/[OH]
pH = -log [H3O]
alpha = 6.367 x 10^-3 / 0.1 (100)
[B] = 0.1 - 6.367 x 10^-3
What is charge balance? - Answer The sum of the positive charges in solution equals
the sum of the negative charges in solution
n1[C1] + n2[C2] = m1[A1] + m2[A2]
C: concentration of cation
n = charge of cation
A: concentration of anion
m = charge of anion
What is mass balance? - Answer The quantity of all species in a solution containing a
particular atom must equal the amount of that atom delivered to the solution. [Show Less]
