5. The acids will have lower pH values, salts will have intermediate pH values, bases will have higher pH values.
The increasing order of pH values is equals to
HNO2(acid) < NH4NO3(acidic salt) < LiNO3(neutral salt) < KClO2(basic salt) < LiOH (base)
8. The given equilibrium reactions are
SO2(g) + 1/2O2(g) SO3(g); K1 = [SO3] / [SO2]*[O2]1/2
2SO3(g) 2SO2(g) + O2(g); K2 = [SO2]2*[O2] / [SO3]2 = ( 1/ ([SO3] / [SO2]*[O2]1/2 )2 = 1/K12
10. The given equilibrium reaction is
2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g); Kp =0.23
Kp = pCO2* pH2O = 0.23
But pCO2 = pH2O = p ======> p2 =0.23
p = 0.48 atm.
The total pressure of the equilibrium mixture = pCO2 + pH2O = 0.48 + 0.48 =0.96 atm
5. You have five different individual aqueous solutions (KCIO2 (aq): LINO, (aq): HNO2 (aq); Lion and...
14- 2.77) E) (-14 +2.77) 4. If pH = 9.33, [OH-] = A) 10 (14 - 9.33) B) 10 -(-14. 9.33) C) 10-14-933) D) 10-933 E) 10 +-7.9.33) 5. You have five different individual aqueous solutions (KCIO, (aq): LINO; (aq); HNO2 (aq); LiOH(aq); and NH4NO3(aq)). These aqueous solutions have different pH values. What is the order of these solutions placed in order of increasing pH: lowest pH to highest pH? A) KCIO2 (aq) <NH4NO3(aq) <LINO3(aq) <LIOH(aq) <HNO2 (aq). B) HNO2...