Please help with 5. A) and b), 6., and 7. 5) Write the net ionic equation for th

Question

Please help with 5. A) and b), 6., and 7. 5) Write the net ionic equation for the principal acid/base reaction which occurs when equal volumes of the following solutions are mixed; also, state the extent of the reaction (large/small) strong or weak, as written. a) 0.1 M NaHSO, with 0.1 M NaC,H,O, 24t t ll%, t C2H3O2 Lame edert b) 0.1 MHINO, with 0.1 M LiOH-tip Laras exledt o) Calculate the pH during the titration of 20.00 ml. of 0.1000 M butanoic acid, with 0.1000 M sodium hydroxide solution after the addition of 15.00 mL. 7) Calculate the K, of NH,, ammonium ion.

Explanation / Answer

5.b

HNO3 + LiOH------------ LiNO3 + H2O

H+ + NO3- + Li+ + OH- --------- Li+ + NO3- + H2O

H+ + OPH- ----------- H2O

6.

Butanoic acid = 20.00ml of 0.100M

number of moles of butanoic acid = 0.100M x0.020L= 0.002 moles

NaOH= 15.00ml of 0.10M

number of moles of NaOH= 0.100M x0.015L = 0.0015 mole

CH3-CH2-CH2-COOH     + NaOH ------------ CH3-CH2-CH2-COONa   + H2O

0.002 mole                      0.0015 mole              0

-0.0015                           - 0.0015                  + 0.0015 mole

after additon of NaOH

reamining number of moles of butanioic acid = 0.002 - 0.0015= 0.0005moles

number of moles of salt = 0.0015 moles

Pka of butanoic acid =4.82

PH= Pka + log(salt/acid)

PH = 4.82 + log(0.0015/0.0005)

PH= 5.297

PH= 5.3.

7.

NH3 + H2O ----------- NH4+ + OH-

Kb of NH3 =1.8x10^-5

KaxKb= Kw             where Kw = ioinc product of water = 1.0x10^-14

Ka = Kw/Kb = 1.0x10^-14/1.8x10^-5 = 5.56x10^-10

Ka = 5.56x10^-10

Ka of NH4+ = 5.56x10^-10

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