H2SO4 is stronger than HSO4- since HSO4 already has one negative charge - gaining a second is unfavorable compared to H2SO4 which would gain only a -1 charge after deprotonation. HNO3 is stronger than HNO2 since the greater number of O atoms exerts a stronger electron- withdrawing effect on the O-H electrons. Additionally, the NO3- ion has more resonance structures and thus greater resonance stability than the NO2- ion. H2S is a stronger acid than H2O since hydrogen forms weaker bonds to elements lower in the periodic table (larger elements). This is why HI is stronger than HBr, for example. H2S is a stronger acid than PH3 since S is more electronnegative (further to the right in the periodic table) than P. Thus, S prefers to have a negative charge compared to P. For part 2: We know that Kw = [H3O*][OH-] = 10^- 14 M. In pure water, these ions are at equal concentrations, so [H+] = [OH-] = 10^-7 M. Now, we have 1.00 mL = 0.001 L. So, we have 10-7 mol/L * 0.001 L = 10^-10 moles of each ion. Now, 1 mol = 6.02 * 10^23 ions, so we have: 6.02*10^23 * 10^-10 = 6.02 * 10^13 [H3O*] ions and 6.02 * 10^13 [OH-] ions. Solution H2SO4 is stronger than HSO4- since HSO4 already has one negative charge - gaining a second is unfavorable compared to H2SO4 which would gain only a -1 charge after deprotonation. HNO3 is stronger than HNO2 since the greater number of O atoms exerts a stronger electron- withdrawing effect on the O-H electrons. Additionally, the NO3- ion has more resonance structures and thus greater resonance stability than the NO2- ion. H2S is a stronger acid than H2O since hydrogen forms weaker bonds to elements lower in the periodic table (larger elements). This is why HI is stronger than HBr, for example. H2S is a stronger acid than PH3 since S is more electronnegative (further to the right in the periodic table) than P. Thus, S prefers to have a negative charge compared to P. For part 2: We know that Kw = [H3O*][OH-] = 10^- 14 M. In pure water, these ions are at equal concentrations, so [H+] = [OH-] = 10^-7 M. Now, we have 1.00 mL = 0.001 L. So, we have 10-7 mol/L * 0.001 L = 10^-10 moles of each ion. Now, 1 mol = 6.02 * 10^23 ions, so we have: 6.02*10^23 * 10^-10 = 6.02 * 10^13 [H3O*] ions and 6.02 * 10^13 [OH-] ions..

1. H2SO4 is stronger than HSO4- since HSO4 already has one negative charge - gaining a second
is unfavorable compared to H2SO4 which would gain only a -1 charge after deprotonation.
HNO3 is stronger than HNO2 since the greater number of O atoms exerts a stronger electron-
withdrawing effect on the O-H electrons. Additionally, the NO3- ion has more resonance
structures and thus greater resonance stability than the NO2- ion. H2S is a stronger acid than
H2O since hydrogen forms weaker bonds to elements lower in the periodic table (larger
elements). This is why HI is stronger than HBr, for example. H2S is a stronger acid than PH3
since S is more electronnegative (further to the right in the periodic table) than P. Thus, S prefers
to have a negative charge compared to P. For part 2: We know that Kw = [H3O*][OH-] = 10^-
14 M. In pure water, these ions are at equal concentrations, so [H+] = [OH-] = 10^-7 M. Now,
we have 1.00 mL = 0.001 L. So, we have 10-7 mol/L * 0.001 L = 10^-10 moles of each ion.
Now, 1 mol = 6.02 * 10^23 ions, so we have: 6.02*10^23 * 10^-10 = 6.02 * 10^13 [H3O*] ions
and 6.02 * 10^13 [OH-] ions.
Solution
H2SO4 is stronger than HSO4- since HSO4 already has one negative charge - gaining a second
is unfavorable compared to H2SO4 which would gain only a -1 charge after deprotonation.
HNO3 is stronger than HNO2 since the greater number of O atoms exerts a stronger electron-
withdrawing effect on the O-H electrons. Additionally, the NO3- ion has more resonance
structures and thus greater resonance stability than the NO2- ion. H2S is a stronger acid than
H2O since hydrogen forms weaker bonds to elements lower in the periodic table (larger
elements). This is why HI is stronger than HBr, for example. H2S is a stronger acid than PH3
since S is more electronnegative (further to the right in the periodic table) than P. Thus, S prefers
to have a negative charge compared to P. For part 2: We know that Kw = [H3O*][OH-] = 10^-
14 M. In pure water, these ions are at equal concentrations, so [H+] = [OH-] = 10^-7 M. Now,
we have 1.00 mL = 0.001 L. So, we have 10-7 mol/L * 0.001 L = 10^-10 moles of each ion.
Now, 1 mol = 6.02 * 10^23 ions, so we have: 6.02*10^23 * 10^-10 = 6.02 * 10^13 [H3O*] ions
and 6.02 * 10^13 [OH-] ions.