At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? (. Molecular weight :NaCl= 58.5, H2(SO)4=98.0 g(mol)- 1)

Question

At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? (. Molecular weight :NaCl= 58.5, H2(SO)4=98.0 g(mol)- 1) (A) 1 molal NaCl(.aq.) (B) 1 molar NaCl(.aq.) (C) 1 molal H2(SO)4(aq) (D) 1 molar H2(SO)4(aq)

Tardigrade Admin · Accepted Answer

One molar text(1 textM) aqueous solution is more concentrated than one molal aqueous solution of the same solute. In solution, one molecule of H2SO4 provides three ions. While one molecule of textNaCl provides two ions. Hence, vapour pressure of solution of textNaCl is higher (as it gives less ions). Therefore, text1 textmolal textNaCl will have the maximum vapour pressure. Vapour pressure is inversely proportional to concentration of solution.

Q. At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?
$($ Molecular weight $: N a Cl = 58.5, H_{2} (SO)_{4} = 98.0 g (m o l)^{- 1})$

$1$ molal $N a Cl (a q)$

$1$ molar $N a Cl (a q)$

$1$ molal $H_{2} (SO)_{4} (a q)$

$1$ molar $H_{2} (SO)_{4} (a q)$

Q. At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? ( Molecular weight :NaCl=58.5,H2​(SO)4​=98.0g(mol)−1)

1 molal NaCl(aq)

1 molar NaCl(aq)

1 molal H2​(SO)4​(aq)

1 molar H2​(SO)4​(aq)

Q. At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?
$($ Molecular weight $: N a Cl = 58.5, H_{2} (SO)_{4} = 98.0 g (m o l)^{- 1})$

$1$ molal $N a Cl (a q)$

$1$ molar $N a Cl (a q)$

$1$ molal $H_{2} (SO)_{4} (a q)$

$1$ molar $H_{2} (SO)_{4} (a q)$