acid base equilibria 1 to 3 keys

8/14/2019 acid base equilibria 1 to 3 KEYS

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Name: Chemistry 142

cid/Base Equilibria #1Question1. What ar1ht:!1H+]and [OH-] in an aqueous solutionprepared by dissolving 0.50g of HClO4 in 750 mL ofsolution?

0.508 HQ04 I( l~f!C.1DL = (). t)c95D ~ HuLjIf) (). 11~ttc-IDCf{) .0 05"'0 Hc.tD.t ::: 4{0. :t-X 16 3.E- +tc.J0 It "" ~t\+-::\

[o,*J,,- I.GJt...lo'4 "l5)< Ia-I:COW]Question2. What are the pH and pOH of an aqueous solution prepared by dissolving 0.36g of KOH in 250 mL ofsolution.

O.3"gKDf-) y.~~~:~ "': :=:;).0 X /D7-~ f\[)ft. V.?-5l- ::. [DH-Jp1 ~ -131 ('2.b\C.fO):- !. 5'tf----

~f+~ IY.O ~ 1.SC(:; {2.41 -

Qu~"on3. ~a.'~~~;I~~~N:H~O.2~~;f~t:Q J1m1D.7-Lfl- Hcl X-Q.t>s-s ::: L3 XID~~!iC,;+Ajo.b~ --BJ0..D + Hz..V (L-- - . ~tJJ:>H~-tk~ 0t~ ~L'3XI'h::2.~.k~ -~rO)( \(f3M-,eQ,ifxI03~~ ~\:nc =L~~"1 ~ t .. Ii-~ :::. ';)..x. r zr ~Jf- + ~.:::: -lfJ Xlff 1-Page1ot2 V


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Name:

Question 4.

Question 5.

Question 6.

What is the conjugate base of each of the following?a) HCI c,-b) H2P04- ItfOLjJ--c) CCI3COOH

CC)3CO 0-What is the conjugate acid of each of the following?a) H2P04-

H3P~b) NH3

PIl-y+c) CO 2-

HcOiIdentify the Br0nsted-Lowry acids and bases in the following equations.a) CI02- + H2O ~ HCI02 + OW

1;~ ~


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Name: Chemistry 142

!Acid/Base Equilibria #2Question1. Write the equation for the ionization for each of the following.

a) HF + l-+z..D ~ H--:sD"+ F -b) CsHsN + H2O .:;;:::= ~ J-)SJJt-t+ + g) l-\ --c) HC6HsO4-~2-'D :;::: C ~~~O t- t1s'OT

d) CH3NH2 + ~).::;::: C~6'\H+-i +-81-+-Question2. Calculate the pH of a O.SOMaqueous solution of ammonia. Kb=1.8x10-5.

Kb ~pJ~3-\-1+,,0~ P f,}: +-f) ~ --

~~.w4+:J[J9l-.r:) . )~


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Name: Chemistry 142Question 3. A 0.20M solution of hypochlorousacid has a pH of 4.08. Calculate Ka for hypochlorous acid.

Hoc( ~- H+- t- [) C(-[).VJ--lL

()-t7'-

C>

t~G ($). 2-0 ..."r ~ ~t< 0- ::- j)-t +J It(J -]LJ+OC-tJf [-L- 4-.e1);" [1-\ TJ~ l6tt.~


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Name:~ Chemistry 142Ch . try 142 Acid/Base Equilibria #3Question 1. A 0.0010mole sample ofNaOH is added to 1.0Lof a solution that is 0.10M NH3and 0.050MNH4Cl.Whatis the pH of the solution after this addition?

a) Write the equation for the ionization of NH3inwater.

~ It~ + H~O ~- ,:)~l.t+t-OH-. b) With which of the solutes will the added NaOH react? . - (i~ Jj~f:)UUo- ~I;;twdi~~ fJ~-t'/'fk-~" #-~t.JIa-I;~JM> ~ ~"6NIItt-tw.e~''b-L t) . &-516)Jt1 7L- ~- (J ')/i"'::1U;W'='~'h~;J!};~"~ ~ ~

l) t 60 10P\~;L . ifd) Calculate the pH of the solutionprior to adding the NaOH.tJ

!).~y ~Ik'. -S' (0.5519 T\f)"J- - , -s-(I,'b:::-/\~XID =:: ~ -.. ) ~-:;::: 3.b>l..lO {; fp~jl:)' too-~[~+ J"" l~0 ""It>-l~ '" 9-. 'D 1\/O-to .}f'!+ ~ 9.C:,

flH3D'l~-'~

e>.( C}()-Y

+ H~.l)c-: PJtlt~ + 0ff-0 .cso 0t~

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Name: Chemistry 142

e) Calculate the pH after the addition.

0 . 0 $""0-- O.OOlOrl'- ~--y-k" -!:>- (Q. 04 ~ +1t)>

acid base equilibria 1 to 3 keys

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