Question

5. You have five different individual aqueous solutions (KCIO2 (aq): LINO, (aq): HNO2 (aq); Lion 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) KClO2 (aq) < NH4NO3(aq) <LINO; (aq) <LIOH(aq) <HNO2 (aq). BHNO2 (aq) < NH4NO3(aq) <LINO, (aq) <KCIO2 (aq) <LIOH(aq). C) LINO, (aq) <HNO2 (aq) <KCIO2 (aq) <NH.NO, (aq) <LIOH(aq). D) NH4NO3(aq) <LINO3 (aq) < HNO2 (aq).<LIOH(aq) <KCIO2 (aq). E) None of the above tinn ORFeo Br(g) + SF2(g) is

Answer 1

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) $\rightleftharpoons$ SO3(g); K1 = [SO3] / [SO2]*[O2]^1/2

2SO3(g) $\rightleftharpoons$ 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)   $\rightleftharpoons$ Na2CO3(s) + CO2(g) + H2O(g); Kp =0.23

Kp = p_CO2* p_H2O = 0.23

But p_CO2 = p_H2O = p _======> p² =0.23

p = 0.48 atm.

The total pressure of the equilibrium mixture = pCO2 + pH2O = 0.48 + 0.48 =0.96 atm