Which of the two aqueous solutions will be a better conductor of electricity in the following examples? explain why in each case.
a)1.0m nacl vs. 0.010 m nacl
b)0.10 m nacl vs. 0.10 m al2(so4)3 (assume complete dissociation of both salts).
c) 1.0 mole of nacl added to water vs. 1.0 mole of pbcl2 added to water (hint: remember the solubility rules).

A) The solution with a concentration of 1.0 M NaCl will be a better conductor of electricity since it has a higher number of electrolytes
b) The 0.10 M Al2(SO4)3 will be a better conductor since more ions are formed per mole of the salt dissociated
c) 1.0 mol of NaCl in water because NaCl is very soluble in water

The option closest to the percentage yield is option;

d. 81.1

Explanation:

The given chemical equation of the reaction is presented as follows;

CaO (s) + H₂O (l) → Ca(OH)₂

The mass of CaO in the experiment, m = 2.00 g

The volume of water with which the CaO was reacted = Excess volume of water

Number of moles = Mass/(Molar mass)

The mass of Ca(OH)₂ recovered, actual yield = 2.14 g

The molar mass of CaO = 56.0774 g/mol

The number of moles of CaO in the reaction, n₁ = 2.00 g/(56.0774 g/mol ≈ 0.036 moles

The molar mass of Ca(OH)₂ = 74.093 g/mol

The number of moles of Ca(OH)₂ in the reaction, n₂ = 2.14 g/(74.093 g/mol) ≈ 0.029 moles

From the given chemical reaction, one mole of CaO reacts with one mole of H₂O to produce one mole of Ca(OH)₂

Therefore, 0.036 moles of CaO will produce 0.036 moles of Ca(OH)₂

Mass = Number of moles × Molar mass

The mass of 0.036 moles of Ca(OH)₂ ≈ 0.036 moles × 74.093 g/mol = 2.667348 grams

∴ The theoretical yield of Ca(OH)₂ = 2.667348 grams

The percentage yield = (2.14 g)/(2.667348 grams) × 100 = 80.23%

Therefore, the option which is closest is option d. 81.1.