(NH4)2CO3 Ionic or Covalent

KEY Solutions Part 2 Name - ________________ 1.) State whether each of the following substances is expected to form an ionic or molecular (covalent) solution. a.) RbBr I c.) CsNO3 (s) I e.) S8 b.) CHCl3 (l) C d.) CuSO4 (s) I f.) CrCl3 (s) C (s) g.) NaCH3COO (s) I (s) h.) ICl I (s) i.) HNO3 j.) CH4 C (g) (l) I C 2.) Write equations to show the dissolving of the following substances in water. a.) (NH4)2SO4 2 NH4+ (aq) (s) c.) K2CO3
+ SO4-2 b.) CH3CH2OH (l) CH3CH2OH (l) 2 K+ (aq) + H2O (l)
(aq) d.) CaCl2 Ca+2 + H2O (l) (s) (s)
+ CO3-2
+ 2 Cl- (aq) (aq) (aq) 3.) Calculate the concentrations of all the ions in each of the following solutions. a.) 0.25  FeCl3 Answer - FeCl3 .       ×       b.) 1.5 × 10  Al2(SO4)3 Answer - .  .  Fe+3 + 3 Cl-
Al2(SO4)3 ! (#$% ) ! (#$% ) ! (#$% ) ! (#$% ) × ×    #$% ! ! (#$% ) c.) 12.0 - of (NH4)2CO3 in 2.50 . Answer -  12.0 - (/0, ) + ×  0.41 - 7(+0) ×  (12% )! $ (12% )! $ 34. 5 (12% )! $ 8($2)! 9,. 5 8($2)!      = 0.75    = 4.5 × 10  *+,  34. 5 (12% )! $  × = 3.0 × 10  (  d.) 0.41 - of Ca(OH)2 in 500 6. of aqueous solution Answer -     2 NH4+ + CO3-2 (NH4)2CO3
12.0 - (/0, ) + ×   2 Al+3 + 3 SO4-2
! (#$% )  . = 0.25    × × 12%    (12% )! $ $ !   (12% )! $ × ×  .    .   Ca(OH)2
  × 8 ! 8($2)! ×  .   = 0.100  /0,  = 0.050  +  Ca+2 + 2 OH- = 0.011  7 1 0.41 - 7(+0) ×  8($2)! 9,. 5 8($2)! × $2    8($2)! e.) 2.50 - of KBr in 150 6. of aqueous solution Answer -  2.50 - :;< × =>? 3 5 =>?  2.50 - :;< × =>? 3 5 =>? × × KEY  × .   KBr
 =  =>?  >?   =>? × ×  .    .   = 0.022  +0  K+ + Br- = 0.140  :  = 0.140  ;<  4a.) Write an equation showing the equilibrium in a saturated solution of lead (II) bromide. Answer - PbBr2 (s) + H2O (l) b.) The solubility of PbBr2 is 0.844 Answer - .A,, 5 BC>?!  × .  BC>?! 5   . F BC>?!  . F BC>?!  × × BC>?! = 0.023  DE;< (aq)  BC !  BC>?!   + 2 Br- (aq) + H2O (aq) . What is its Molarity? 49 5 BC>?! c.) Calculate the concentrations of Pb+2 Answer - Pb+2 
>?  BC>?! and Br- (aq) in a saturated solution of PbBr2? = 0.023  DE  = 0.046  ;<  5.) Calculate the concentration of all the ions present when a.) 25.0 6. of water is added to 20.0 6. of 0.35  Fe+3. Answer - (. )(.) ., = 0.156    b.) 15.0 6. of 6.5 × 10  Cu+2 is mixed with 40.0 6. of 3.2 × 10  ClAnswer - (4. ×H )(. ) . 1:1 ratio (.× )(.,) = 1.8 × 10  I .  = 2.3 × 10    c.) 95.0 6. of 8.65 × 10,  Al(NO3)3 is mixed with 15.0 6. of 7.50 × 104  Ag2SO4. Answer - Al(NO3)3
7.47 × 10,  ((/+ ) × 7.47 × 10,  ((/+ ) × Ag2SO4
(A.4 ×% )(.3 ) Al+3 + 3 NO3    2 Ag+ + SO4-2 .  (1$ ) 1$  (1$ ) = 7.47 × 10,  ((/+ ) = 7.47 × 10,  (  = 2.24 × 10  /+  (9. ×K )(. ) . = 1.02 × 104  (- *+, 2 KEY 1.02 × 10 4  (- *+, × 1.02 × 104  (- *+, × 5   5! #$%  #$% !  5! #$% = 2.04 × 10 4  (-  = 1.02 × 104  *+,  d.) 25.0 6. of 0.360  NH4Br is mixed with 75.0 6. of 0.160  (NH4)2SO4. Answer - NH4Br 0.090  /0, ;< ×  12%   12% >? 0.120  (/0, ) *+, ×   . = 0.090  /0, ;< = 0.090 /0,  0.090  /0, ;< × Ag2SO4 (.4)(. ) NH4+ + Br-

>?    12% >? 0.090 + 0.240 = 0.330 /0,  = 0.090  ;<  (.4)(.9 ) 2 NH4+ + SO4-2 12%  (12% )! #$% . = 0.120  (/0, ) *+, = 0.240  /0,  0.120  (/0, ) *+, ×   #$% ! (12% )! #$% = 0.120  *+,  3