Which of the following are correct for an ide | vedclass

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(C) An ideal solution is a solution that obeys Raoult's law over the entire range of concentration.Such solutions are formed by mixing two components

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$a, b, c$ only

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(C) An ideal solution is a solution that obeys Raoult's law over the entire range of concentration.Such solutions are formed by mixing two components that are similar in molecular size, structure, and have almost identical intermolecular forces.The characteristics of ideal solutions are:$(1)$ It must obey Raoult's law.$(2)$ The enthalpy of mixing should be zero, i.e.,$\Delta H_{	ext{mix}} = 0$.$(3)$ The volume of mixing should be zero, i.e.,$\Delta V_{	ext{mix}} = 0$, which implies $V_{	ext{solvent}} + V_{	ext{solute}} = V_{	ext{solution}}$.Examples of ideal solutions include $n$-hexane + $n$-heptane and benzene + toluene.The mixture of carbon dioxide and water is not an ideal solution because they react with each other to form $H_2CO_3$, which involves chemical changes and significant enthalpy changes.Therefore, statements $(a)$, $(b)$, and $(c)$ are correct.

Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.

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$A$ mixture of ethanol and acetone shows positive deviation from Raoult's law because:

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Which of the following are correct for an ideal solution?$(a) \Delta V_{\text{mix}} = 0$$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$$(c) \Delta H_{\text{mix}} = 0$$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.